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Exam 2 Study Guide

by: Raquel Guerra-lewis

Exam 2 Study Guide Chem 101

Raquel Guerra-lewis
GPA 3.5
Chemistry 101
Dr. Michael Finnegan

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This is the Note Review of everything that will be on the test for Exam 2.
Chemistry 101
Dr. Michael Finnegan
Study Guide
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This 8 page Study Guide was uploaded by Raquel Guerra-lewis on Tuesday October 20, 2015. The Study Guide belongs to Chem 101 at Washington State University taught by Dr. Michael Finnegan in Summer 2015. Since its upload, it has received 89 views. For similar materials see Chemistry 101 in Chemistry at Washington State University.


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Date Created: 10/20/15
CHEMISTRY 101 REVIEW WORKSHEET FOR EXAM 2 This worksheet is to aid you in preparing for the exam It will not be collected or graded You should be able to answer all questions on this worksheet using only the information provided This worksheet will be distributed in tutorial and posted on the course web site Your TA can con rm or correct your answers 1 Identify the multiplier that corresponds to each of the following metric pre xes au bn cM dc ed fk 2 Place the following measurements in order from smallest to largest 506x103 m 271x103m 935x102 m 322x104 m 3 Perform the following conversions a a box is 55792 mm long 3025 mm wide and 987 mm high Calculate the volume of the box and convert this volume into L and m3 b Convert 284 ums2 to kmday2 c Convert 392801x108 nm to cm 4 A ceramic object has a mass of 52862 g If the object is placed in a measuring cylinder containing 468 mL of water the water level rises to a reading of 651 mL Calculate the density of the object 5 A metal cube measures 1250 cm on a side and has a density of 1678 gmL Calculate the mass of the metal cube 6 A ask weighs 9627 g when empty If the ask is filled with carbon tetrachloride the ask and the carbon tetrachloride weigh 32524 g Carbon tetrachloride is a liquid with a density of 1595 gmL at 25 C the temperature at which all measurements were performed What is the volume of the ask 7 The specific heat of mercury is 0033246 calg C How much heat in kcal is required to raise the temperature of 237mL of mercury from 187 C to 935 C The density of mercury is 13546gmL 8 1768 kcal of energy are required to heat 3000g of water to a temperature of 963 C What was the initial temperature of the water 9 Consider three solid metal spheres each with a diameter of 1000 cm One is made of iron density 786 gmL one is made of gold density 193 gmL and one is made of titanium density 451 gmL Rank these sphere in order of increasing mass 10 If 5000 cal of energy are applied to 1000 g blocks of chromium Cp 560 calg C and silicon Cp 478 calg C both at an initial temperature of 250 C Which of these substances will have the higher nal temperature 11 Write equations to describe what happens when the following compounds are dissolved in water a potassium dichromate b ironIII bromide 12 Write balanced chemical equations for the following reactions a The decomposition of potassium chlorate to form potassium chloride and oxygen b The combustion of cyclopentane CSHIO c The neutralization reaction between solutions of calcium hydroxide and hydrochloric acid d The reaction between solutions of potassium hydrogen carbonate and sulfuric acid e The reaction between aqueous solutions of copperII sulfate and strontium perchlorate f The reaction of calcium metal with hydrobromic acid 13 Write the formula of the precipitate formed when solutions of the following compounds are mixed a calcium chloride and sodium sulfate b silver nitrate and hydrochloric acid c nickelII nitrate and sodium phosphate 14 Identify the oxidation number of each element in the following compounds a CoClO33 b so2 c CH3CH3 d K3PO4 e CH2C12 i HBro2 15 Identify the element oxidized the element reduced the oxidizing agent and the reducing agent in the following reactions a 5 HZCZO4 aq 2KMnO4 aq 3 HZSO4 aq II 2 MnSO4 aq KZSO4 aq 10 CO2 g 8 H20 1 b 8 NH3 g 6 N02 g quot 7 N2 g 12 Hz0 g 16 Write both the ionic equation and the net ionic equation that correspond to each of the following standard equations 3 PbNO32 31 NH42SO4 31 quot 1313804 S 2 NH4NO3 aq b 2 NaOH aq CoCl2 aq I39 2 NaCl aq CoOH2 s 17 Calculate the mass of 07685 mole of a glycerol C3H803 b strontium thiosulfate 18 For each compound calculate the number of moles of the compound that are present in 2500 g of the compound a silicon tetrachloride b vanadiumV oxide c potassium hydrogen carbonate 19 How many moles of hydroxide ion are present in 5000 g of each of the following compounds a barium hydroxide b IronIII hydroxide 20 What mass of carbon is required to react with excess bismuthIII oxide in order to prepare 10000g of bismuth metal BiZO3 s C s quot Bi s CO g 21 Given the equation NO2 g H20 l quot HNO3 aq NO g How many grams of HNO3 are produced for every gram of NO2 that reacts 22 What mass of iron may be produced by 600g of ironIII oxide and 500g of carbon in the reaction FeZO3 s C s I Fe 1 CO2 g Did you balance the equations in problems 2022 23 Classify each of the following reactions as endothermic or exothermic a 3Fe203 s CO g gt 2 Fe3O4 s CO2 g AH485 kJ b N2 g 02 g gt 2 NO g AH 903 M c NO g 03 g gt N02 g 02 g AH200 U 24 Consider the reaction BaOH2 s 2NH4SCN s 158kcal gt BaSCN2 aq 2NH3 g 2H20 l a What is the sign and value of AH for this reaction b Is this reaction endothermic or exothermic 25 a Write a balanced chemical equation for the combustion of ethene gas C2H4 b AH for this reaction is 3162 M How much heat will be produced by the complete combustion of 193 g of ethene c How much heat will be produced if 3265 g of carbon dioxide are produced by the combustion of ethene 26 For each of the following equations a predict the sign of AS for the reaction and b state the temperature conditions all none high or low under which the forward reaction will be spontaneous i CaCO3 s 2 HCl aq quot CaCl2 aq H20 1 CO2 g AH 342 kcal ii NH3 g HCl g quot39quot NH4Cl s AH 4211 kcal iii CH3OH l I CO g 2 H2 g AH 3994 kcal 27 Xe g 3 F2 g I39 XeF6 g AHo 9608 kcalmol and AG0 6692 kcalmol a Calculate the value of AS0 at250 C b Assuming that the values of AH and AS change do not change with temperature calculate the value of Aer11 at 1000 C c At what temperature does AG 0 for this reaction d At what temperatures will this reaction be spontaneous Don t just say high or low use the actual numbers Such as From X to Y or All temperatures below Z 28 Identify the temperature conditions under which reactions with the follow reaction would be spontaneous Answer with high T low T all T or no T a AH isandAS is b AH isandAS is c AH isandAS is 29 Consider the following reaction 3 H2 g N2 g I 2 NH3 g How would each of the following changes affect the rate of the forward reaction a Increasing the temperature at which the reaction is run b Increasing the concentration of H2 g c Increasing the concentration of NH3 g d Decreasing the concentration of N2 g e Decreasing the volume of the container Gasses are compressible they will conform to the volume of the container f Adding a catalyst 30 a Draw a reaction energy diagram for a reaction with an activation energy of 1000 kcal and a AG of 250 kcal Label the energy levels of the reactants and products the activation energy and the AG b Draw a reaction energy diagram for the reaction in part a when a catalyst that reduces the activation energy by 400 kcal has been added c Draw a reaction energy diagram for a reaction in which the reactants have a free energy of 250 kcal the product have a free energy of 500 kcal and the activated complex has a free energy of 750 kcal d If the temperature and the concentrations of the reactants are the same for all three reactions which of the reactions would be the fastest Explain 31 Write equilibrium constant equations for the following reactions H g 12 g i 2 HI g 2 SO g 2 CI g i 2 SOZCIZ g 02 g v Cuo s H g Cu 1 H20 g 2 NH g CO g CONH2gt2 s H20 9 v 32 Consider the following reaction H20 g C120 g i 2 HClO g AH 300 kcal Keq 00900 at 25 C a Does the equilibrium favor products or reactants at 25 C b Would the equilibrium shift in the favor of reactants left or products right if i The temperature was lowered ii H20 g was added to the reaction mixture iii The volume was increased iv HClO g was removed from the reaction mixture 33 Consider the system below to be at equilibrium before each of the following changes to the system are made For each change determine which direction the equilibrium will shift left right or not at all 2 C s 02 g i 2 CO g AH 221 k a Cool the reaction ask b Increase pressure reducing the size of the container c Add a catalyst which speeds the reaction d Add solid Fe mesh to absorb COg e Add more C s f Add more 02 g 34 Write balanced chemical equations for the following reactions a The combination reaction between potassium metal and nitrogen b The decomposition of ammonium nitrate into its elements c The neutralization reaction between solid zinc hydroxide and nitric acid d The precipitation reaction between solutions of lithium carbonate and titaniumIV chloride e The gas forming reaction between solid potassium carbonate and perchloric acid f The gas forming reaction between iron metal and hydrobromic acid iron gets oxidized to ironIII g the reaction between solutions of barium hydroxide and sulfuric acid 35 a What are the correct values of the initial graduated cylinder reading and the graduated cylinder reading after an object has been added in the pictures below 1 II ISU ISU E6 a LJ39I I LJ39I I mllmllmlHullmlml t Close up View 40 40 5 E an 40 EILTE 30 J H SD FE Close up ViEl W 20 20 m 2 E initial volume reading nal volume reading Before object is added After object has been added b If the mass of the cylinder and water before the object was added is 115497 g and the total mass after the object was added is 208543 g what is the density of the object 36 A mixture of solid NaCl and solid BaC122 H20 has a mass of 1773 g the mixture is dissolved in water Sodium sulfate solution is added in excess to form a precipitate according to the equation BaCl2 aq NaZSO4 aq P BaSO4 s 2 NaCl aq The precipitate is filtered and dried The precipitate has a mass of 0501 g What is the mass percent of barium chloride in the original mixture The Solubility Rules 1 All sodium potassium lithium and ammonium salts are soluble 2 All nitrates acetates chlorates and perchlorates are soluble Silver acetate is slightly soluble 3 All silver lead and mercury salts are insoluble MercuryII chloride is soluble MercuryII bromide is slightly soluble 4 All chlorides bromides and iodides are soluble 5 All carbonates phosphates sul des and oxides are insoluble 6 All hydroxides are insoluble Barium hydroxide and strontium hydroxide are soluble calcium hydroxide is slightly soluble 7 All sulfates are soluble Except those of barium strontium and calcium q CSmAT K C 27315 AG AH TAS ELECTRONEGATIVITIES OF THE ELEMENTS 1A L Li Be 10 15 Na Mg 39029 12 BB 48 SB 68 K Ca Sc Ti V Cr 08V 10 13 15 16 16 Rb Sr Y Zr Nb M0 08 10 12 14 16 18 Cs Ba La Hf Ta W 07 09 10 13 15 17 PERIODIC TABLE OF THE ELEMENTS 1A 8A 1008 4003 H He 1 2A 3A 4A 5A 6A 7A 2 6941 9012 Number above symbol atomic mass 1081 1201 1401 1600 1900 2018 Li 39 Number below symbol atomic number B C N O F Ne 3 4 5 6 7 8 9 10 2299 2430 2698 2809 3097 3207 3545 3995 Na Mg 8B Al Si P S Cl Ar 11 12 3B 4B 53 GB 73 1B 23 13 14 15 16 17 18 3910 4008 4496 4787 5094 5200 5494 5585 5893 5869 6355 6538 6972 7264 7492 7896 7990 8380 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 1 9 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 8547 8762 8891 9122 9291 9596 98 10107 10291 10642 10787 11241 11482 11871 12176 12760 12690 13129 Rb Sr Y Zr Nb Mo Tc Flu Rh Pd Ag Cd In Sn Sb Te l Xe 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 13291 13733 13891 17849 18095 18384 18621 19023 19222 19508 19697 20059 20438 2072 20898 209 210 222 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 55 56 5771 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 223 226 227 267 268 271 272 270 276 281 280 285 284 289 288 293 294 Fr Fla Ac Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Uuq Uup Uuh Uuo 87 88 89 104 105 106 107 108 109 110 111 112 113 114 115 116 118 Elements 113 through 116 have been reported and confirmed but they have not yet been named Element 118 has been reported but has not been independently confirmed Lanthanide series Actinide series 14012 14091 1442 145 15036 15196 15725 15893 16250 16493 16726 16893 17305 17497 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 58 59 60 61 62 63 64 65 66 67 68 69 70 71 23204 231 04 23803 237 244 243 247 247 251 252 257 258 259 262 Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 90 91 92 93 94 95 96 97 98 99 100 101 102 103


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