Final Exam Practice Test Q&A Compilation
Final Exam Practice Test Q&A Compilation CHEM 1331
Popular in Fundamentals of Chemistry: Chem 1
Popular in Chemistry
This 18 page Test Prep (MCAT, SAT...) was uploaded by Tyler on Sunday February 14, 2016. The Test Prep (MCAT, SAT...) belongs to CHEM 1331 at University of Houston taught by in Winter 2016. Since its upload, it has received 825 views. For similar materials see Fundamentals of Chemistry: Chem 1 in Chemistry at University of Houston.
Reviews for Final Exam Practice Test Q&A Compilation
Report this Material
What is Karma?
Karma is the currency of StudySoup.
Date Created: 02/14/16
Final Exam Compilation Tuesday December 08 2015 1118 PM 1 Fundamentals Fathers of Chemistry Thompson Rutherford Dalton ect OR Subtraction 2 1 Thomson Who is credited with discovering the atomic nucleus Rutherford Fluorite a mineral of calcium is a compound ofthe metal with fluorine Analysis shows that a 276 sample of fluorite contains 142g calcium Calculate the mass of fluorine in the sample 134g fluorine Avogadro39s hypothesis states that Measured the chargemass ration ofthe electron At the same temperature and pressure equal X2 volumes of different gases contain an equal number of particles Galena a mineral of lead is a compound ofthe metal with 017g Sulfur sulfur Analysis shows that a 127g sample of galena contains 110g lead Calculate the mass of sulfur in the sample If 2000 g of zinc sulfide contains 1342 g of zinc how many grams of sulfur can be obtained 388g S from 118 kg of zinc sulfide The mass ratio of calcium to oxygen in calcium oxide is 25051 What mass of calcium 374 oxide will form when 267 grams of calcium is completely converted to calcium oxide A compound of a transition metal and iodine is 527 metal by massHow many grams of 418 the metal can be obtained from 794 g ofthis compound How many of the following postulates of Dalton39s atomic theory are still scientifically 2 accepted I All atoms of the same element are identical Compounds are combinations of different atoms III A chemical reaction changes the way atoms are grouped together IV Atoms are indestructible Which ofthe following statements from Dalton39s atomic theory is no longer true according All atoms of a given element are identical to modern atomic theory Which ofthe following is NOT a feature of Thompson39s quotRaisin Puddingquot model ofthe atom The number of neutrons in an atom is the same for all neutral atoms of that element False Leadll nitrate is used in photography Calculate the mass of lead in 139 g of PbN032 870 g Who is credited with first measuring the charge ofthe electron Millikan Isotopes and Neutrons Find Elements on the Periodic Table An atom containing 34 protons 43 neutrons and 34 electrons would have the symbol The element rhenium Re exists as two stable isotopes and 18 unstable isotopes Rhenium185 has in its nucleus Bromine exists naturally as a mixture of bromine79 and bromine 81 isotopes An atom of bromine79 contains What is the sum of the numbers of neutrons and electrons in the ion 2 7P0139 What is the sum of the numbers of neutrons and electrons in the ion 2 8P02 Which of the following atomic symbols is incorrect The number of electrons in an atom is the same for all neutral atoms of that element The number of neutrons in an atom is the same for all neutral atoms ofthat element There are how many electrons and neutrons in the aluminum27 isotope How many neutrons are there in the nucleus of a 232Th atom Consider the isotope bromine8181Br Select the combination which lists the correct atomic number number of neutrons and mass number respectively Which ofthese have the same number of electrons Br Kr Sr2 C N 02 III Mg2 Ca2 Sr2 IV 02 0 02 V Ag Cd2 Pd What is the sum of the numbers of neutrons and electrons in the ion 73A52quot Chemistry Page 1 The presence of a nucleus 77Se 75 protons 110 neutrons 35 protons 44 X3 neutrons 35 electrons 208 210 148M True False 13 14 142 35 46 81 V 71 3 Electromagnetic Radiation Section 21 AE hc2 The form of EMR that has more energy per photon than ultraviolet rays but less energy per photon than gamma rays is X ray X3 Calculate the wavelength in nm of light with a frequency of 2446 x 1014Hz Enter your answer with one decimal place and 12265 i 1 no units A Xray photon has a wavelength of 245 nm What is its energy in joules Once you have the value take its log base 10 16091 Which ofthese colors of visible light has the smallest amount of energy per photon red Ultraviolet B radiation often absorbed by sunscreen products has wavelengths roughly between 280 and 315 nm If a 18168 certain UVB wave has a wavelength of 2923 nm what is the energy of one of its photons in J Once you have the value take it log base 10 and enter that with three decimal places as your answer Do not enter units A Xray photon has a wavelength of 531 nm What is its energy in joules Once you have the value take its log base 10 16427 and enter your answer with three decimal places Do not enter units with your answer Visible light has wavelengths of roughly from 400 to 700 nm If a certain color has a wavelength of 616 nm what is the 18491 energy of one of its photons in J Once you have the value take it log base 10 Ultraviolet B radiation often absorbed by sunscreen products has wavelengths roughly between 280 and 315 nm If a 18172 339 certain UVB wave has a wavelength of 2948 nm what is the energy of one of its photons in J Once you have the value take it log base 10 and enter that with three decimal places as your answer Do not enter units UVC light used in sterilizers has wavelengths between 100 to 280 nm If a certain UVC wave has a wavelength of 1604 179066 i 1 nm what is the energy of one of its photons in J Once you have the value take it log base 10 and enter that with three decimal places as your answer Ultraviolet B radiation often absorbed by sunscreen products has wavelengths roughly between 280 and 315 nm If a 18179 certain UVB wave has a wavelength of 3002 nm what is the energy of one of its photons in J Once you have the value take it log base 10 and enter that with three decimal places as your answer Infrared radiation has wavelengths of roughly from 700 nm to 1 mm If a certain infrared wave has a wavelength of 6254 19498 nm what is the energy of one of its photons in J Once you have the value take its log base 10 and enter that with three decimal places as your answer Do not enter units Calculate the wavelength in nm of light with a frequency of 9759 x 1014Hz Enter your answer with one decimal place and 3074 no units Which ofthese colors of visible light has the smallest amount of energy per photon red 4 Hydrogen atoms and their Shells Any set of d orbitals consists of orbitals 25 Calculate the wavelength in nm of the photon released when a hydrogen atom undergoes a transition from the excited 9369 i 2 state where n 6 to the state where n 1 A hydrogen atom in its groundstate absorbs a photon of wavelength 9720nm To what energy level does the electron N 4 X2 move Which ofthe following is an incorrect designation for an atomic orbital 2d According to the Bohr model the energy of the hydrogen atom is given by the equation E 217 x 10 19J nZCalculate 122 x 10 7 m the wavelength of the photon emitted when the atom undergoes relaxation from the first excited state to the ground state In an experiment searching for the photoelectric effect an incident beam of green light produced no ejected electrons Try blue light X2 from a metal In order to eject electrons the experimenter should The Bohr equation for the energy of states in the hydrogen atom is 545 x 103919 EnJ 218 x 103918n2 What is the ionization energy in J for the loss of an electron from the lowest excited state n2 Calculate the wavelength in nanometers ofthe electromagnetic radiation required to raise an electron from the n 3 to 128 x the n 5 energy level of a hydrogen atom a What is the wavelength nm of a photon emitted by a hydrogen atom when its electron falls from n 5 to 4 Do not 4055111 i 2 include units The maximum number of electrons allowed in the fourth energy level of an H atom is 32 From the following list of observations choose the one that most clearly supports the following conclusion Observation A a emission spectrum of hydrogen b the photoelectric effect c scattering of alpha particles by metal foil d diffraction e cathode quotraysquot Electrons in atoms have quantized energies A d sublevel can hold a maximum of 10 The minimum energy needed to eject an electron from a sodium atom is What is the maximum wavelength of light in 451 nanometers that will show a photoelectric effect with sodium Chemistry Page 2 5 Electron Con guration The electron configuration for Ca2 is identical to that of The electron configuration for the bromide ion is identical to that of Which ofthe following ions has the same electron configuration as an argon atom Which element or ion listed below has the electron configuration 1522522p5 Give the groundstate electron configuration symbol and group number from each partial valencelevel orbital diagram Give the full groundstate electron configuration for the element Se Ar Kr X3 K All of these He 2522p5 Ne 8A 18 1522522p63523p64523d104p4 X2 1522522p63523p64523d2 is the correct electron configuration for which of the following atoms Ti What element has the electron configuration 122522p53523p54523d1 4p55524d1 5p56524f145d1 6p2 Pb Given the following electronic configuration of neutral atoms identify the element and state the number of unpaired electrons in its ground state Example HeZs1 Answer Li 1 Ar4513d10 How many unpaired electrons are there in an atom of sulfur in its ground state Give the ground state electron configuration symbol and group number from each partial valence level orbital diagram MI 311111 2s 2 Of the following elements which needs three electrons to complete its valence shell 6 Principal Quantum Number Section 26 The energy of an electron in the hydrogen atom is determined by What is the lowestnumbered principal shell in which 5 orbitals are found What is the lowest numbered principal shell in which d orbitals are found Which of these subshells is incorrect According to the quantum theory the size of an atomic orbital is associated with Which set ofthe following statments includes all those that are fa and none that are true i An atom may be excited to a higher energy state by absorbing photons ofthe correct energy ii Davison and Germer first found experimental evidence for wave behavior of electrons iii Bohr39s model was eventually modified to describe the spectra of nearly all elements Which of the following statements is TRUE Schrodinger39s major contribution to quantum theory was to All the following are true EXCEPT Calculate the energy J of an electron in the hydrogen atom if it resides in energy level number 5 7 Electron Orbitals How many p orbitals have the value n 1 A point in the wave function where the amplitude is zero defines What is the I quantum number for a 4f orbital Areas of zero probability of finding an electron are called Consider the following representation of a 2p orbital Which ofthe following statements best describes the movement of electrons in a porbital Consider the following portion ofthe energy level diagram for hydrogen n 4 01361 X 10 18 n 3 02420 x 10 18 n 2 05445 X 10 18 n 1 2178 x 10 18 Cu 1 2x None ofthese The principal quantum number n ofthe orbital that it occupies only 1 X2 3 3f X2 the principal quantum number n X3 ony The photoelectric effect implies that light is particle like in some of its properties solve the wave equation for electron waves within X2 the hydrogen atom confirming that the electron can only exist in discrete energy levels in that atom the energies of subshell in the shells energy levels of a hydrogen atom vary as s lt p lt d etc 872 X 10 20 0 The node X3 3 X2 Nodes The electron movement cannot be exactly determined 122 x 10 7 m In the hydrogen spectrum what is the wavelength of light associated with the n 2 to n 1 electron transition Chemistry Page 3 Which ofthe following best describes an orbital the space in an atom where an electron is most likely to befound All matter exhibits either particulate or wave properties exclusively False X2 The number of orbitals in a subshell having a given value of l is equal to 2 1 Which ofthe following combinations of quantum numbers n I m m5 do not represent permissible solutions of 6 5 1 12 the Schrodinger equation for the electron in the hydrogen atom ie which combination of quantum numbers is not allowed Ifn 2 how many orbitals are possible 4 8 Atomic Radius Section 211 OR Periodic Table Section 212 Which of the following is a metal Thallium Tl Z81 X2 Which ofthe following has the largest radius C Which ofthe following is not a lanthanide element Hf Rank the ions below in order of decreasing size Cs gt Ba2 gt Sr2 X2 Sr Ba Cs Which one ofthe following groups does not contain any metals C S As H 3 Arrange each set in order of decreasing atomic size Sr gt Sn gt Te X2 Sn Te Sr Arrange each set in order of decreasing atomic size Pb gt Sn gt Ge X2 Ge Pb Sn Which of the following elements is a metal Fe X2 Which ofthe following is a nonmetal Br Which ion among the following has the smallest radius Be2 9 Ionization Energy Arrange each set of atoms in order of decreasing IE1 F gt C gt Be X3 Choose the atom or ion using a periodic table N X2 Larger first ionization energy C or N Choose the atom or ion using a periodic table Be Larger first ionization energy Li or Be What is the full electron configuration ofthe Period 3 element with the following successive IEs in 1522522p 53s2 kJmol IE1 738 IE2 1450 IE3 7732 IE4 10539 IE5 13628 Which set has IE1 for the atoms arranged correctly He gt Ne gt Kr Arrange each set of atoms in order of decreasing IE1 Cl gt Br gt Se a Cl Br Se List the following atoms in order of increasing ionization energy Li Na C O F Na lt Li lt C lt O lt F X2 Which equation correctly represents the Mionization of calcium Cag gt Cag e Order the elements S Cl and F in terms of increasing ionization energy S Cl F Which one of the following equations correctly represents the process involved in the electron Xg e X39g affinity of X Which atom in each pair has the more exothermic electron affinity i Na ii Si iii Cl i Na or Mg ii Si or P iii Cl or Ar 10 Ionic Compounds A arsenic atom needs to gain electrons to achieve a noble gas configuration 3x What stable monatomic ions do strontium Z 38 and selenium Z 34 form Sr2 and SeZ39 X2 The charges on the permanganate ion and ammonium ion are respectively 1 1 fthe arsenate ion has the same charge and number of oxygens as the phosphate ion what is the H3AsO4 formula of arsenic acid The formula of the stable ionic compound containing only phosphorus and aluminum is AIP X2 The formula of polonium oxide is P002 Based on this information the formula ofthe phosphate of P03PO44 polonium is expected to be Which of the following compounds is the product of the reaction Mg 02 MgO X2 The formula of calcium oxide is CaO What is the formula of the ionic compound containing calcium CaSO4 and sulfate ions Chemistry Page 4 Based on electronegativities which of the following would you expect to be most ionic Can Which ofthese ions isare NOT commonly found in stable ionic compounds a b e a Baz39 b Si4 c 5239 d Al3 e Rb2 Magnesium reacts with sulfur to form MgS Metals typically have electronegativity values low 11 LATTICE ENERGIES Which of the following ionic compounds has the largest lattice energy ie the lattice energy most BeO X2 favorable to a stable lattice Given the following information 602kJ X2 Lis gt Lig enthalpy of sublimation of Lis 166 kJmol HBrg gt Na Brg bond energy of HBr 363 kJmol Lig gt Lig e ionization energy of Lig 520 kJmol Brg e gt Br g electron affinity of Brg 325 kJmol Lig Brg gt LiBrs lattice energy of LiBrs 809 kJmol H2g gt 2ng bond energy of H2 432 kJmol Calculate the change in enthalpy for 2Lis 2HBrg gt H2g 2LiBrs The enthalpy of formation AHf of rubidium chloride is 4305 kJmol The enthalpy of sublimation for 691 rubidium is 86 kJmol and the first ionization energy of rubidium is 402 kJmol The bond dissociation energy of C2 is 243kJmol and the electron affinity of chlorine is 349 kJmol Calculate the lattice energy of RbCl in kJmol Calculate the lattice energy kJmol of the hypothetical ionic compound MX from the information 6293 X2 given below IE1M 597 kJmol Ms gt Mg AHO 867 kJmol AHOfUVlX 1566 kJmol X2g gt 2Xg AH 218 kJ EA X 320 kJmol 339 IEl X 271 kJmol Calculate the lattice energy for LiBrs given the following 809 kJmol X2 sublimation energy for Lis 166 kJmol AHffor Brg 97 kJmol first ionization energy of Lig 520 kJmol electron affinity of Brg 325 kJmol enthalpy of formation of LiBrs 351 kJmol Calculate the lattice energy kJmol ofthe hypothetical ionic compound MX from the information 5714 given below IE1M 599 kJmol Ms gt Mg AH 53 kJmol AH fMX 1739 kJmol x2g gt 2Xg AH 163 kJ EA X 336 kJmol IE1 X 271 kJmol Use the information below to calculate the lattice energy of magnesium sulfide 3406 kJmol Mgs gt Mgg AHo 148 kJ mol Mgg gt Mg2g 2e AHo 2186 kJ mol 1 8 585 gt Sg AHo 279 kJ mol Sg 2e gt SZg AHo 450 kJ mol Mgs 1 8585 gt MgSs AHo 343 kJ mol Calculate the lattice energy of RbCl using the following data 696 kJmol X3 Rbs gt Rbg AH 86 kJmol Chemistry Page 5 Rbg gt Rbg e39 AH 409 kJmol 023 gt 2Clg AH 242 kJmol Clg e39 gt Cl39g AH 355 kJmol Rbs 12 C2g gt RbCls AH 435 kJmolx Which ofthe following ionic compounds has the smallest lattice energy ie the lattice energy least Csl favorable to a stable lattice 12 Bond Energies and Enthalpy Estimate the standard enthalpy change Ah for the reaction below a2C0 g 02 gt 2C02 Bond energies kJmol C0 358 CO 799 CEO 1071 O2 498 The least electronegative element of those listed is Which of the following is in the order of decreasing bond strength Using the given bond energies BE calculate AH rxn for the reaction CH4g Cl2g gt CHC3g HClg not balanced Bond BE kJmol Bond BE kJmol CH 413 CC 347 CC 614 CCl 339 H CI 427 CI CI 243 The bond energies for H2g and HFg are 435 and 565 kJmol respectively For the reaction 12 H2g 12 F2g gt HFg the heat of reaction is 268 kJmol of HF produced According to this what is the bond energy of F2 in kJmol Which of the following elements has the greatest electronegativity Which of the following elements has the lowest electronegativity Estimate the standard enthalpy change AH for the reaction below 2H2g 02g 2H20g Bond energies kJmol H H 432 02 494 H O 459 Consider the following reaction A2 B2 gt 2AB AH 377 kJ The bond energy for A2 is half the amount of AB The bond energy of B2 425 kJmol What is the bond energy of A2 Which of the following chemical bonds is SHORTEST Which ofthe following chemical bonds is LONGEST 13 Lew Dot Structures Which ofthe following has a Lewis dot structure most like that of CO How many pairs of valence electrons in methanoic acid HCOOH are involved in bonding and how many are non bondingBonding Non bonding The Lew structure for CHC3 has nine lone electron pairs Draw the Lewis structures of the molecules below and use them to answer the following questions Which ofthe molecules obeys the octet rule I BH3 ll N02 SFs IV 03 V PCl5 How many lone pairs of electrons are there on the Cl atom in CIF3 When molten sulfur reacts with chlorine gas a vilesmelling orange liquid forms that is found to have the empirical formula SCI Which of the following could be the correct Lewis structure for this compound Which ofthe following molecules is incorrectly matched with the number of lone pairs found on the central atom How many lone pairs of electrons are there on the atom in C4 In the Lewis structure for elemental nitrogen there is are a39 Draw the Lewis structures of the molecules below and use them to answer the following questions BH3 N02 SFs IV 03 V PCl5 Which ofthese molecules show resonance Chemistry Page 6 556kJ X2 Ba CICI BrBr II X2 330kJ 159 CI Rb 478 kJ X2 267 kJmol X2 Si F Si Si NO 54 True 2 X2 l 1 5 5 l 1 X2 N02 1 lone pair 1 a triple bond between the nitrogens II N In the Lewis structure for SF5 the central sulfur atom shares electrons 12 Consider the compound crotonaldehyde whose skeleton is H H H H I I I I H Ill Cg Eg C D H How many nonbonding electrons appear in the Lewis structure ofthis molecule 9stIhsf9l399win 39swisstructure 0 i H i H31 2 3 CE C CH 9 3 c How many unshared pairs of electrons are present in this molecule 14 Naming CompoundsFormulas Give the formula and name of the compound formed from the following elements RbBr Rubidium Bromide BaS Barium Sulfide Can Calcium X3 a Rubidium and bromine b sulfur and barium c calcium and fluorine Fluoride Write names for the formulas or formulas for the names of the following Dinitrogen trioxide compounds SFs a N203 Iodine trichloride b sulfur hexafluoride C lCl3 Give the systematic names for the formulas or the formulas for the names Sodium hydrogen phosphate Na2HPO4 K2CO3 2H20 Potassium Carbonate Dihydrate Sodium Nitrite NaNOZ 3 Give the systematic names for the formulas or the formulas for the names ron Bromide FeBr3 ron oxide is used as a pigment Which of the following is its formula Fe203 X2 Which ofthese is FALSE COlz is copper iodide Which ofthese has a name that does NOT include the prefixes quotdiquot or quottriquot MgClz Which name formula combination is INCORRECT manganesell oxide Mn02 Give the systematic names for the formulas or the formulas for the names sodium dihydrogen phosphate What is the correct name of CaOH23HZO calcium hydroxide trihydrate X2 From the following compounds choose the nameformula pair that is NOT lead phosphate PbPO4 correctly matched 15 VSPER Model Section 41 or Bond Polarity 42 Draw the Lewis Dot Structure and the shape ofthe chlorine trifluoride molecule The IDEAL value 180 of the largest F Cl F bond angle in CF3 is The bond angles about the carbon atom in the formaldehyde molecule H2CO are about 120 X2 Ofthe molecules below only is nonpolar C02 The molecular structure of 5032 is pyramidal X3 Which of the following molecules has a nonlinear structure 03 X2 The molecular geometry ofthe BeC2 molecule is and this molecule is linear nonpolar the same because in each case there are the same number of electron pairs around the central atom According to the VSEPR model the arrangement of electron pairs around NH3 and CH4 is The bond angles about the carbon atom in the formaldehyde molecule H2CO are about Which ofthe following has a Tshaped structure The molecular structure of BeF3 is 120 Cl3 trigonal planar The molecular structure of I3 is linear 16 Polarity and Dipole Moments Which ofthe following molecules contains polar bonds but is nonpolar CCI4 Which of the following possesses polar bonds but has a zero overall dipole moment BF3 X2 Which of the following molecules Or ions has a dipole moment PF3 X4 Which of the following molecules is not a polar molecule BF3 X3 Which ofthe following molecules has a dipole moment 02 Chemistry Page 7 Dichloroethylene C2H2Cl2 exists in three different forms isomers shown in the following figure 39 Which ofthese hashave a dipole moment not equal to zerox Which set ofthese molecules is polar ClSCszClz SbF5 ASH3 Select the molecule from the following that has a dipole moment How many ofthe following molecules SFz SF4 SFs SiOz are polar 17 Hybridization Ofthe following the central atom is sp3d2 hybridized only in How many sigma 5 bonds and pi p bonds are in propene CH2CHCH3 What is the hybridization ofthe sulfur atom in sulfur tetrafluoride SF4 The hybridizations of iodine in F3 and F5 are and respectively Ofthe following only has sp3 hybridization ofthe central atom What is the molecular geometry around a central atom that is 5p2 hybridized has three sigma bonds and one pi bond What is the hybridization ofthe central atom in a molecule with a squarepyramid molecular geometry What is the hybridization ofthe central iodine atom in l3 What is the hybridization ofthe sulfur atom in SClz For which of the following molecules and ions does the central atom have sp2 hybridization The central atom is listed first in each formula below Ofthe following only has sp hybridization ofthe central atom What is the molecular geometry around a central atom that is 5p2 hybridized has three sigma bonds and one pi bond For which of the following molecules or ions does the central atom have 5p hybridization N3 03 and If Which ofthe following is incorrectly matched with the hybridization of the orbitals on the central atom 18 Molecular Orbital Model What is the bond order of He2 land iii only cisC2H2C2 and AsH3 SF4 Xe Answer cut off 4 eight 5 one p Sp3d Spd and spd Cut off PF3 Trigonal planar sp3d 2 sp3d 5p3 NOBr X2 C032quot trigonalplanar N3 only H30 sp2 Answer cut off What is the bond order of C2 1 Which of the following species would not have the MO configuration NO X3 Assume all have the same order of MO energies as N2 Which of the following molecules or ions is not paramagnetic in its ground state F2 X2 The configuration 02520252Tt2py1rt2px1 is the molecular orbital description for the ground state of B2 How many ofthe following F2 B2 02 N2 are paramagnetic 2 Assuming a molecular orbital energy level diagram like that of 02 how many unpaired electrons are present in 0 NO Larger bond order means greater bond strength True As the bond order of a bond increases the bond energy and the bond length According to molecular orbital theory predict the bond order for N21 According to molecular orbital theory predict the bond order for 0239 Increases decreases 25 15 According to molecular orbital theory and assuming a molecular orbital diagram with the same order of energies 25 as that for 02 predict the bond order for CO 19 Average Atomic Mass What is the mass of 6 atoms in copper in grams 633 x 1022g x2 Naturally occurring copper exists in two isotopic forms 63Cu and 65Cu The atomic mass of copper is 6355 amu What is the 70 X2 approximate natural abundance of 63Cu The average mass of a carbon atom is 12011 Assuming you were able to pick up only one carbon unit the chances that you 0 X3 would randomly get one with a mass of 12011 is Naturally occurring argon consists of three isotopes the atoms of which occur in the following abundances 034 N 359676 3995 amu amu 007 38Ar 379627 amu and 9959 40Ar 399624 amu The calculated atomic weight of argon is Chemistry Page 8 An element with two isotopes approximately 45 and 55 abundance has a periodic table atomic mass of 16171 u One ofthe 164 isotopes has a mass of 159 u Which choice is most likely to be the mass number ofthe second isotope Obtain the average atomic mass of gallium from the periodic table Given that gallium has two isotopes 69Ga 6893 amu and 604 71Ga 7093 amu calculate the percentage of 69Ga Obtain the average atomic mass of gallium from the periodic table Given that gallium has two isotopes 59Ga 6893 amu 396 and 71Ga7093 amu calculate the percentage of71Ga There are two isotopes of Element X Their percent abundances and atomic masses are X20 6296 X21 3704 2037 X2 Calculate the weighted average atomic mass in amu If the mass of the only two isotopes of an element are 1153026 u and 1228251 u and the weighted average mass is 1181471 u 622 X2 what is the percent abundance of the lighter isotope 20 Mole Ratios IE How many atoms or Moles What is the number of oxygen atoms in 550g of iron hydroxide FeOH2 molar mass 8995gmol In the reaction of aluminum metal and oxygen gas aluminum oxide is formed How many moles of 02 will react with 20 moles Al Give in order the correct coefficients to balance the following reaction stnCle H25 gt ShSz HCl How many oxygen atoms are there in 2 formula units of Al25033 When the following equation is balanced what is the sum of the coefficients Al2SO43 C3OH2 AlOH3 C3504 Calculate the mass in grams of 0250 mol iron How many hydrogen atoms are present in 42 g of ammonium carbonate When 10 mol of Fe reacts with Clz forming FeCI3 how many moles of Clz are required to react with all ofthe iron What is the sum of the coefficients of the following equation when it is balanced using smallest whole numbers NaNHz NaN03 NaN3 NaOH NH3 How many atoms of hydrogen are present in 292 g of water Calculate the number of atoms in 100 g He What is the coefficient for water when the following equation is balanced AsOH3s HZSO4aq AszSO43aq HZOI 21 Empirical Formula or Metal Oxide or 100 divide by moles A metal oxide with the formula MO contains 2853 oxygen Type the symbol for the element represented by M Which compound contains the highest percent by mass of hydrogen A metal oxide with the formula M02 contains 2123 oxygen by mass Type the symbol for the element represented by M A 15g sample of lithium is reacted with 15 g of fluorine to form lithium fluoride 2Li F2 gt 2LiF After the reaction is complete what will be present 737 X 1023 15 moles X2 1 2 1 6 X2 18 9 140 21 x 1024 X2 15 mole 195 x 1023 150 x 1024 6 H20 Sn 0789 moles lithium fluoride and X2 137 moles lithium A 1567 g sample of a titanium chloride was decomposed to pure titanium which had a mass of 0487 g ts TiC3 empirical formula is What is the empirical formula and empirical formula mass for the following compound AlBr3 2667 gmol AlzBl s A chloride of silicon contains 791 mass Cl What is the empirical formula of the chloride SiCl3 X3 What is the empirical formula for a compound containing only carbon and hydrogen whose elemental C1H2 X2 analysis mass is 8563 and 1437 Calcium reacts with sulfur forming calcium sulfide What is the theoretical yield g of CaSs that could be 531 i 1 prepared from 777 g of Cas and 236 g of sulfurs A gaseous hydrocarbon was analyzed and found to consist of 8365 carbon by mass The molar mass ofthe C5H14 compound is 862 gmol What is the molecular formula ofthe compound The mass percent of hydrogen in NH4C is 754 22 Aqueous Solutions Section 62 A electrolyte dissociates to a great extent in an aqueous solution Strong X2 Which one ofthe following substances is predicted to be most soluble in water MoN032 How many total moles of ions are released when the following sample dissolves completely in water 273 Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and 2Agaq aqueous barium nitrate The balanced complete ionic equation contains which ofthe following terms Chemistry Page 9 Predict whether an aqueous solution of each of the following substances will conduct an electric a conducts b does not conduct c current does not conduct a Potassium hydroxide GIUCOSE C5H1205 c Ethanol C2H5OH Aqueous solutions of sodium sulfide and copper chloride are mixed together Which CUS Wi predpitate from SOIUtiOn39 statement is correct Which of the following is not a strong base NH3 How many total moles of ions are released when the following sample dissolves completely in water 618 206 mol K2504 The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the 3OH aq X2 following species Which of the following is a strong acid HCO4 The man who discovered the essential nature of acids through solution conductivity studies is Arrhenius How many moles of H ions are present in the following aqueous solution 054 2945 mL of 0183 M nitric acid A solid acid HX is mixed with water Two possible solutions can be obtained Which of the following is In case I HX is acting like a strong acid true and in case M HX is acting like a weak acid H 3 H E39 H H 339 Hi Hi 3 1 g H 1 I 3 5quot 3 Ht 339 H Ht 339 Him 1quot g I H 2H H n H HE Equot 23 The Composition of Solutions 63 and Molarity Calculate the molarity of a hydrochloric acid solution that is 1825 HCI by mass and has a density of 120gmL 601 Calculate the number of moles of HCI in 6285 mL of 0453 M hydrochloric acid 00285 mol What would be the molarity of a solution obtained by diluting 125 mL of 600 M HCI to 500 mL 15 Calculate the molarity of a solution containing 925 mol of H2504 in 275 L of solution 336 Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate What is the formula of the solid Ca3PO42 formed in the reaction A 7044g sample of BaOH2 is dissolved in enough water to make 1800 liters of solution How many mL of this solution must be 438 mL a diluted with water in order to make 1000 L of 0100 M BaOH2 What is the molarity of chloride in a solution containing 0074 M CaClz 015 X2 How many moles of Haq ions are present in 125 L of 075 M nitric acid 094 mol A 184g sample of HF is dissolved in water to give 20 x 102 mL of solution The concentration of the solution is 46 M X2 Calculate the molarity of a solution prepared by dissolving 1495 moles of LiOH in enough water to give a final volume of 750 mL 199 M X2 An analytical procedure requires a solution of chloride ions How many grams of MgClz must be dissolved to make 140 L of 329g 00493 M CI A 0150 M sodium chloride solution is referred to as a physiological saline solution because it has the same concentration of salts as 241 g normal human blood Calculate the mass of NaCl solute needed to prepare 2750 mL of a physiological saline solution 24 OxidationReduction Given the reaction 10 2Mn04 5H202 6H gt 2Mn2 8H20 502 In the reaction Cu 4311 E hg39l ag 4 C133quot mg E 153 the reducing agent if any is What is the average oxidation number of the irons in Fe307 Note that average oxidation numbers are not 4 X2 restricted to integer values All of the following reactions oxidationreduction reactions X3 2Als 3Br2l gt 2ABr3s 2Ag20s gt 4Agls 029 CH4U 2029 gt C02lg 2H20lg can be classified as Identify the oxidizing agent and the reducing agent in the following i ox agent Cr2072 red Chemistry Page 10 i8Haq Cr2072 aq 35032 aq gt 2Cr3aq 3504239aq 4H20l ii N0339aq 4Zns 70H39aq 6H20l gt 4ZnOH4239aq NH3aq Which ofthe following are oxidationreduction reactions I PC3 Clz PC5 Cu 2AgN03 CuN032 2Ag C02 2Li0H Li2C03 H20 IV Fer 2Na0H Fe0H2 2NaCl Zn land When the redox equation shown below is balanced the 3 stoichiometric coefficient of Br2 will be KC03aq HBraq gt Br2l H20l KCI Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate The balanced complete ionic equation contains which ofthe following terms An oxidizing agent What is the oxidation number of S in Na25205 assume both sulfurs have the same ox no 5 Balance the following oxidationreduction reaction using the oxidation number method 6 Fe Brz Fe3 Br In the balanced equation the coefficient of Br is Which species is the oxidizing agent in the following reaction F2 4KBr 2F2 gt 2Br2 4KF 25 HeatEnergyWork Systems AE QW A system receives 5162J of heat and delivers 4033 J of work to its surroundings What is the change in internal ofthe system in J A system releases 255 cal of heat to the surroundings while delivering 428 cal of work What is the change in internal energy of the system in cal For a particular process q 17 kJ and w 21 kJ Which ofthe following statements is false agent 5032 ii ox agent N0339 red agent 2Aglaq none ofthese 1129 683 cal X2 The system does work on the surroundings Calculate AE given the following information q 41 kJ w 23 kJ 64 kJ What is the change in internal energy in J of a system that absorbs 0615 kJ of heat from its surroundings and has 0247 165 x 103J kcal of work done on it involves the transfer of energy between two objects due to a temperature difference heat A system receives 9437J of heat and delivers 1667 J of work to its surroundings What is the change in internal energy 77700 of the system in J Enter your answer with two decimal places and no units 39 What is the specific heat capacity of graphite if it requires 266J to raise the temperature of 15 grams of graphite by 25 071 Jg C C 0f energy work enthalpy and heat how many are state functions 2 A chunk of aluminum at 914 C was added to 2000 g of water at 155 C The specific heat of aluminum is 0897 Jg C 437 g and the specific heat of water is 418 Jg C When the temperature stabilized the temperature of the mixture was 189 C Assuming no heat was lost to the surroundings what was the mass of aluminum added Calculate the work associated with the compression of a gas from 1210 Lto 800 L at a constant pressure of 167 atm 685 L atm A system receives 268J of heat and has 436J of work done on it by its surroundings What is the change in internal 704 energy of the system in J Exactly 2480J will raise the temperature of 100 g of a metal from 250 C to 600 C What is the specific heat capacity of 0709 Jg C the metal Calculate the work for the expansion of C02 from 10 to 30 liters against a pressure of 10 atm at constant temperature 20 Latm 26 Enthalpy of Formation Given that the standard enthalpy of the formation of Hg0s 9084 kJmol calculate Ah rxn for the reaction below 18168 kJmol 2Hg0 s gt 2Hg I 02 g For the reaction 422 kJ H2g 1202g gt H20I deltaH 286 kJmol calculate the enthalpy change when 266 g of water is produced The heat of formation of Fe203 is 826 kJmol Calculate the heat ofthe reaction 4Fe 302 gt 2Fe203 when a 206 kJ 2786g sample of iron is reacted Using the following thermochemical data calculate AHf of EuZ03s 16514 kJmol 2EuC3s 3H20I gt EU2035 6HClg H 5242 kJmol 2Eus 3C2g 2EuC3s H 18720 kJmol Chemistry Page 11 4HCIg 029 gt 2029 2H20l H 2024 kJmol Consider the following processes AH kJmol 3B 2C D 125 12A B 150 E A D 350 Calculate AH for B E 2C Consider the reaction H2g 02g H20 AH 286 kJ Which of the following is true Using the following thermochemical data 25bs 6HFg gt ZSbF3s 3H2g AH 16318 kJmol ZSbs 6HCIg gt ZSbCI3s 3H2g AH 2106 kJmol 39 calculate AH for the following reaction SbF3s 3HCIg gt SbC3s 3HFg When a 135g sample of ethyl alcohol molar mass 4607 gmol is burned how much energy is released as heat When 1 mol of KBrs decomposes to its elements 394 kJ of heat is absorbed Which ofthese is a balanced thermochemical equation for this reaction Calculate Aern for 2NOClg gt N2g 02g Cl2g given the following set of reactions N0g 12Cl2g gt NOCIg Aern 386 k Calculate the standard enthalpy of formation of acetaldehyde CH3CH0g given the information below CH3CH0g 5202g gt 2CO2g 2H20 AH rxn 1194 k AH f C02g 394 kJmol AH f H20l 286 kJmol2 Given CU20s 02g 2Cu0s AH 144 kJ CU20s Cus Cu0s AH 11 kJ Calculate the standard enthalpy of formation of Cu0s Determine the enthalpy change when 242 g of carbon is reacted with oxygen according to the reaction Cs 02g gt C02g deltaH 394 kJmol Given the information below calculate the AH of combustion of glucose C6H1206AHf of glucose 1275 kJmol AHf of C02 390 kJmol AHf of H20 285 kJmol 27 Gas Laws PVnRT with Constants 175 kJmol A and C are true 7106 kJmol X2 401 x 102 kJ KBrs gt Ks 12Br2l Aern 103 k 166 kJmol 155 k 794 kJ 2775 kJmol A gas sample is heated from 200 C to 57 C and the volume is increased from 2L to 45L If the initial pressure is 0118 00684 atm atm what is the final pressure A flexible container is charged with a certain volume of gas at 3183 K Under conditions of constant pressure and moles of gas how does the volume of the gas change when the temperature is decreased by afactor offour The volume decreases by a factor of four A flexible container is charged with 51L of gas at 368 K Under conditions of constant pressure and moles of gas what 153L is the volume of the gas when the temperature is tripled What is the effect of the following on the volume of 1 mol of an ideal gas Both the pressure and temperature are reduced by one fourth oftheir initial values What is the effect of the following on the volume of 1 mol of an ideal gas The pressure changes from 760 torr to 202 kPa and the temperature changes from 37 C to 155 K A sample of oxygen gas has a volume of 560 L at 27 C and 8000 torr How many oxygen molecules does it contain For an ideal gas which pairs of variables are to each other if all other factors remain constant 1 P and T 2 n and T 3nandP 4 Vand n What is the effect of the following on the volume of 1 mol of an ideal gas The temperature changes from 305 K to 32 C and the pressure changes from 2 atm to 101 kPa How many moles of gas are in a gas sample occupying 0738 L at 135 mmHg and 30 C What volume of gaseous water H20 has the same moles of gas as 100 L of xenon gas at the same temperature and pressure Chemistry Page 12 Volume does not change V decreases by 75 144 x 1023 2 only Volume increases by 100 000527 mol 100 L What is the effect of the following on the volume of 1 mol of an ideal gas The pressure changes from 760 torr to 202 kPa and the temperature changes from 370 C to 155 K What volume of methane gas CH4 has the same number of atoms as 600 L of krypton gas at the same temperature and pressure A 449g sample of Ne gas exerts a certain pressure in a container of fixed volume What mass of Ar is required to exert half the pressure at the same conditions of volume and temperature New volume is 25 of the original volume 120 L 444g Ar A flexible vessel is filled to a certain pressure with 1200 L of gas Under conditions of constant temperature and moles The volume increases by X2 of gas how does the volume of the gas change when the pressure of the gas is decreased by afactor of three 28 Density of Gases Molar mass dRT p What is the density in gL of the Freon CF3C at 1745 C and 021 atm A 224 L high pressure reaction vessel is charged with 03910 mol of iron powder and 120 atm of oxygen gas at standard temperature On heating the iron and oxygen react according to the balanced reaction below 4Fes 302g 2Fe203s After the reaction vessel is cooled and assuming the reaction goes to completion what pressure of oxygen remains The density of a gas is 196gL at STP What is its molar mass The density of 02 gas at 4 C and 157 atm is A vessel with a volume of 325 L contains 280 g of nitrogen gas 0403 g of hydrogen gas and 799 g of argon gas At 25 C what is the pressure in the vessel The balanced chemical equation for the conversion of nitrogen to ammonia is 2N2g 3H2g 2NH3g Which of the following statements concerning this chemical equation isare correct 1 In a 224 L container at standard temperature 2 atm of nitrogen gas will react with 3 atm of hydrogen gas to produce 2 atm of ammonia gas 2 At standard pressure and temperature 224 L of nitrogen gas will react with 224 L of hydrogen gas to produce 224 L of ammonia gas 3 At standard pressure and temperature 448 L of nitrogen gas will react with 672 L of hydrogen gas produce 224 L of ammonia gas A 100L sample of a gas at STP has a mass of 116 g The molar mass of the gas is What is the density in gL of Freon11 CFCI3 at 458 C and 066 atm Use decimal format do not type the units The density of 02 gas at 4 C and 157 atm is A mixture consisting of 0120 mol N2 0018 mol 02 0112 mol CH4 and an unknown amount of C02 occupies a volume of 904 L at 25 C and 117 atm pressure How many moles of C02 are there in this sample A 193g mixture of oxygen and argon is found to occupy a volume of 162 L when measured at 6759 mmHg and 434 C What is the partial pressure of oxygen in this mixture At standard conditions it was found that 1114 L of gas had a mass of 695 g What is the molar mass of the gas An unknown gaseous hydrocarbon consists of 8563 carbon by mass A 0335g sample of the gas occupies a volume of 0107 L at STP What is the identity of the gas 29 Effusion OR Average Speed 87 What is the ratio of the average speed of CH4 molecules to that of 02 molecules at 298K At the same temperature lighter molecules have a higher average kinetic energy than heavier molecules At a particular pressure and temperature it takes 455 min for a 15L sample of He to effuse through a porous membrane How long does it take for 15L of F2 to effuse under the same conditions A sample of H gas 20 L at 35 atm was combined with 15 L of N gas at 26 atm pressure at a constant temperature of 25C into a 70 L flask The total pressure in the flask is atm Assume the initial pressure in the flask was 000 atm A sample of He gas 20 mmol effused through a pinhole in 53 s The same amount of an unknown gas under the same conditions effused through the pinhole in 248 s The molecular mass of the unknown gas is gmol What would happen to the average kinetic energy of the molecules of a gas sample if the temperature of the sample increased from 20 C to 40 C If 250 mL of methane CH4 effuses through a small hole in 28 s the time required for the same volume of helium to pass through the hole under the same conditions will be A sample of oxygen gas 0 was found to effuse at a rate equal to three times that of an unknown gas The molecular weight of the unknown gas is gmol Under what set of conditions does HClg deviate the most from ideal behavior Which of the following statements concerning gas molecules is incorrect Chemistry Page 13 a factor of three 597 903 atm 439 gmol 221gL 173 atm X2 1 only 260 gmol 344 221 gL 0182 mol 437 mmHg X2 13976 C5H10 21 False 14 min X3 16 X2 Cut Off 88 X2 It would increase 14 s 288 low temperature and high pressure Attraction is greater between fastmoving molecules than between slowmoving molecules The molar mass of an unknown gas was measured by an effusion experiment It was found that it took 63 s for 48 gmol the gas to effuse whereas nitrogen gas required 48 s The molar mass ofthe gas is 30 Intermolecular Forces The strongest intermolecular interactions between pentane C5H12 London dispersion forces X2 molecules arise from When the adhesive forces between a liquid and the walls of a capillary tube are greater than the cohesive forces within the liquid Which ofthe following would you expect to have the highest boiling point Which ofthe following substances would you expect to have the lowest boiling point The relatively weak forces that exist among noble gas atoms are Choose the correct Hbonded structure that shows the member of each pair of compounds that forms intermolecular H bonds CH32NH or CH33N Which ofthe compounds below is an example of a network solid The freezing point of helium is 270 C The freezing point of xenon is 112 C Both of these are in the noble gas family Which ofthe following statements is supported by these data The resistance of a liquid to an increase in its surface area is the ofthe liquid A certain solid substance that is very hard has a high melting point and is nonconducting unless melted is most likely to be Which ofthe following substances would you expect to have the lowest boiling point On the basis of your knowledge of bonding in liquids and solids which of the following has the lowest melting temperature Which of the following intermolecular forces of attraction is the strongest 31 Bonding in Metals Which set of these statements is FALSE the liquid level in a capillary tube will rise above the surrounding liquid and the surface in the capillary tube will have a concave meniscus l2 methane CH4 London dispersion forces X2 A Cut Off Sl02 The London dispersion forces between the helium molecules are less than the London dispersion forces between the xenon molecules Surface tension NaCl methane CH4 Clz Hydrogen bonding I Electrical conductivity of a pure semiconductor like Si results from both the movement of positive holes and electrons in the valence band Aluminum doped with silicon would be a ptype semiconductor Si Ge and alphaSn are all intrinsictype semiconductors For which of the following elements in their normal stable forms would it be correct to describe the bonding as involving a quotsea of electronsquot Which if any of the band molecular orbital energy arrangements below is consistent with metallic bonding r r In metals the conduction bands and valence bands ofthe molecular orbitals are separated by a large energy gap Which of the following best describes the bonding in metals Which one of the following substances does not exist in the indicated solid type Chemistry Page 14 iAnd only Lithium X2 b Only X2 False The valence electrons of a each metal X2 atom are delocalized over all of the atoms in the piece of metal Si02 molecular According to the band theory as applied to metallic bonding what set of these statements is TRUE ii and iii only X2 i the bonds between neighboring metal atoms can be described as localized electron pair bonds ii the valence electrons of representative metals are free to move within the solid leading to thermal conductivity iii the electrical conductivity of metallic solids decreases with increasing temperature In which ofthese substances are the atoms held together by metallic bonding Cr If a metal crystallizes in a bodycentered cubic lattice each metal atom has quotnearest neighborsquot 8 X2 The energy gap between the conduction band and the valence band is large for insulators 32 Chapter 9 Molecular Structures in Solids What is the distance in atom radii r along any edge of a primitive unit cell 2 X r X3 At room temperature CsF is expected to be A brittle solid How would you expect the melting point of CF4 to compare to that of NaF It should be lower because NaF form as an X3 extended ionic crystal lattice whereas CF4 is a covalently bonded small molecule Calcium sulfide has a facecentered cubic unit cell with calcium ions in octahedral 4 calcium ions 4 sulfide ions X2 holes How many ions of each element are contained in each unit cell Which equation represents the number of atoms in a bodycentered cubic unit cell V 7 l X2 a tnm 1 E 3 Which equation represents the number of atoms in a facecentered cubic unit cell Sel led A wri 1 1 atoms a E LEI E E Q Ana imr 1 atuma ll 3 39339 Cubic closest packing is another name for facecentered cubic packing Table salt and table sugar are both crystalline solids True Solid MgO has the same crystal structure as NaCl How many oxide ions surround each 6 Mg2 ion as nearest neighbors in MgO 33 Enthalpy of vaporization sublimation The enthalpy heat of vaporization for ethanol C2H50H is 433 kJmol How much heat in kilojoules is required to 108 vaporize 115g of ethanol at 25 C The vapor pressure of water at 80 C is 048 atm In which of the following process will energy be evolved as heat crystallization X2 The enthalpy of sublimation of mercury at 25C is 6130 kJmol If the of mercury is at its melting point of 389C 59 Cut Off estimate the for mercury at 25C in kJmol The enthalpy of sublimation for a particular compound at 250 C is 324 kJmol The enthalpy of fusion for this 22 X2 compound at its melting point is 104 kJmol Calculate the enthalpy of vaporization for this compound Which one of the following decreases as the strength of the attractive intermolecular forces increases the vapor pressure of a X2 liquid Given below are the temperatures at which two different liquid compounds with the same empirical formula have a The normal boiling X2 vapor pressure of 400 torr point of dimethyl ether will be higher than the Compound T C normal boiling point of ethanol dimethyl ether CH3 O CH3 378 ethanol CH3CH20H 635 Which of the following statements a d is false Classify the following processes as exothermic or endothermic Freezing of Water a a exothermic b endothermic How many grams of ice would be melted by the energy obtained as 191 g of steam is condensed at 100 C and cooled 153g to 0 C How much heat in k is released when 158 g OH is condensed at 25C 188 Cut off A 0025 g sample of O is injected into a 100 L flask at 300 C What forms of water will be present at equilibrium gas Chemistry Page 15 Vapor pressure of water at 300 C is 318 mm Hg 34 Phase Diagram Examine the following phase diagram and determine what phase exists at point F Vapor X2 l i htnl my C and A Consider the phase diagram for substance X l mi E 5 E e l l empaam39ium 3Ilt Which points represent Xg and Xs respectively Examine the following phase diagram and identify the feature represented by point A Triple Point l f it E a Point D on the phase diagram is referred to as the point triple H l I Consider the phase diagram for substance X C and A Diagram a Missing Which points represent Xg and Xs respectively Consider the phase diagram for C02 The point on the graph labelled E represents C02 as a supercritical fluid X2 Chemistry Page 16 Plum Waging flu LTquot t139iu Dammit F551 lamTiara inst lea infill 39El lmmum amt to emit A sample consisting of C02g and C02s at equilibrium at 78 C and 1 atm pressure is heated to 30 C and the pressure is increased to 8 atm Based on the phase diagram below what will happen What process occurs when the temperature of a substance is at Point A increased at constant pressure until the substance is at Point B E Fm55ugg Eh I I Which pomt corresponds to the critical point Examine the following phase diagram and identify the feature represented by point B The phase diagram of a substance can be used to obtain the vapor pressure of that substance at a given temperature Difficulty M Shown below is a phase diagram for compound Y At 25 C and 1 atm Ywill exist as a 1 atm Ffatm T 0 Compilation of Tester Practice Final Chem 1331 Alexander Potthast x Chem Practice Final Shadaan Rupani Chem final pratice test Nimair Ghulamani x Final Chem Review Ruben Vargas FE Practice Chem dris Yusuf Chem 1331 practice final Batool Kazimi Practice Final Flavio G Castillo Practice Final Hieu Nguyen Chemistry Page 17 All of the C02 will be Diagram converted to C02l Missing Melting D Critical point Diagram missing True X2 liquid Practice final william PracticeFinalExam Practice Final Chem 1331 Chem Final Practice Exam Chem Practice Final FE Practice PF CHEM Chem Practice Final ChemPracticeFlnal William Ferguson Astrid Torres Frank Nguyen Abhishek Prajapati Ayesha Sydea Phoung Nguyen Duncan Gerungan Simrat Kaur Dorothy Nguyen Chemistry Page 18