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by: Dahlia Douglas


Marketplace > Texas A&M University > Chemistry > CHEM 107 > GEN CHEM FOR ENGINEERS
Dahlia Douglas
Texas A&M
GPA 3.63


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Class Notes
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This 10 page Class Notes was uploaded by Dahlia Douglas on Wednesday October 21, 2015. The Class Notes belongs to CHEM 107 at Texas A&M University taught by Staff in Fall. Since its upload, it has received 142 views. For similar materials see /class/226241/chem-107-texas-a-m-university in Chemistry at Texas A&M University.

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Date Created: 10/21/15
Texas A amp M University Department of Chemistry CHEM107 Spring 2011 Instructor MasudMonwar PhD Study Guide for Exam 4 Posted on 26 April 2011 Chapter 11 Chemical Kinetics l a Give the relative rates of disappearance of reactants and formation of products for each of the following reactions i 2 03g gt 3 02g ii 2HOFg gt 2HFg 02g b In reaction ai the rate of formation of 02 is 15 X 10393molLs What is the rate of decomposition of 03 2 a Using the rate equation Rate k A2B de ne the order of the reaction with respect to A and B What is the total order of the reaction b The reaction between ozone and nitrogen dioxide at 231 K is first order in both the N02 and 03 2N02g 03g gt N205s 02g i Write the rate equation for the reaction ii Ifthe concentration of N02 is tripled what is the change in the reaction 7 iii Whata the effect on reaction rate if the concentration of O3 is halved c The data in the table are for the reaction of NO and 02 at 660 K 2NO 02g gt 2NOzg Reactant Rate NO 0010 0020 i Determine the order of the reaction for each reactant ii Write the rate equation for the reaction Continued to page 2 MasudMonwar 2011 Ref Kotz 6medn l iii Calculate the rate constant iv Calculate the ratein molLs at the instant when NO 0015 molL and Oz00050 molL V At the instant when NO is reacting at the rate 10 X 10394molLs what is the rate at which 02 is reacting and N02 is forming d A reaction has the following experimental rate equation Rate kA2B If the concentration of A is doubled and the concentration of B is halved what happens to the reaction rate 3 Data for the reaction 2NOg 02g quot9 2N02g are given in the table rate 36gtltl 34gtltl 36gtltl 68gtltl 18gtlt1 17gtltl l8gtltl a What is the rate law for this reaction b What is the rate constant for the reaction c What is the initial rate of the reaction in experiment 4 4 a The rate equation for the hydrolysis of sucrose to fructose and glucose C12H22011 aq H200 quot9 2C6H1206aq Is AsucroseAt kC12H22011 After 257 h at 27 C the sucrose concentration decreased from 00146 M to 00132 M Find the rate constant b The decomposition of SOzClz is a firstorder reaction SOzC12g quot9 S02g C12 The rate constant for the reaction is 28 X 10393 min391 at 600K If the initial concentration of SOzClz is l24gtlt10393molL how long will it take for the concentration to drop to 03lgtlt1039 3 molL 5 a The rate equation for the decomposition oszO5 giving N02 and 02 is ANZO5At kN205 The value ofk is 50 X 10394 s391 for the reaction at a particular temperature i Calculate the halflife of N205 ii How long does it take for the N205 concentration to drop to one tenth of its original value Continued to page 3 MasudMonwar 2011 Ref Kotz 6medn 2 b Gaseous azomethane CH3NNCH3 decomposes in a firstorder reaction when heated CH3NNCH3g quot9 N2g C2H6g The rate constant for this reation at 425 C is 408 min39l If the initial quantity of azomethane in the ask in 200 g how much remains after 00500 min What quantity of N2 is formed in this time c Formic acid decomposes at 550 C according to the equation HCOOHg quot9 C02g H2g The reaction follows firstorder kinetics In an experiment it is determined that 75 of a sample of HCOOH has decomposed in 72 seconds Determine 172 for this reaction 6 Gaseous N02 decomposes at 573 K 2 NOzg quot9 2N0g 02g The concentration of N02 was measured as a function of time A graph of lNOz versus time gives a straight line with a slope of 11 Lmols What is the rate law for this reaction What is the rate constant 7 a Calculate the activation energy Ea for the reaction N205g quot9 2N02g 12 02g Form the observed rate constants k at 25 C 346 X 10395 s391 and k at 55 C 15 X 10393 s39 b Whenheatedto ahigh r e 39 39 C4HgJ r to ethylene C4H8g quotquotquotquot quot9 2C2H4g The activation energy Ea for this reaction is 260 kJmol At 800 K the rate constant k 00315 s39l Determine the value ofk at 850 K c The reaction of Hz molecules with F atoms Hzg H9 quot9 HFg Hg has an activation energy of 8 kJmol and an energy change of l33 kJmol Draw a reaction coordinate diagram activation energy diagram for this process Indicate the activation energy and enthalpy of reaction on this diagram Continued to page 4 MasudMonwar 2011 Ref Kotz 6medn 3 8 a What is the rate law for each of the following elementary reactions i NOg N03g quot9 2N02g ii Clg H2 iii CH33CBraq quot9 CH33Caq Br39aq b Ozone 03 in the earth s upper atmosphere decomposes according to the equation 203g quot9 302g The mechanism of the reaction is thought to proceed through an initial fast reversible step followed by a slow second step Step 1 Fast reversible 03g c 02g 0g Step 2 Slow 03g 0 g quotquotquot quot9 202g i Which step is ratedetermining ii Write the rate equation for the ratedetermining step c Iodide ion is oxidized in acid solution by hydrogen peroxide H202aq 2Haq 2139aq quot9 12aq 2H20l A proposed mechanism is Step 1 Slow HzOzaq I39aq quot9 HzOl OI39aq Step 2 Fast Haq OI39aq quotquot9 HOIaq Step 3 Fast HOIaq Haq I39aq 9 12aq HzOl i Show that the three elementary steps add up to give the overall stoichiometric equation ii What is the molecularity of each step iii For this mechanism to be consistent with kinetic data what must be the experimental rate equation iv Identify any intermediates in the elementary steps in this reaction d A proposed mechanism for the reaction of N02 and CO is Step 1 Slow endothermic 2NOzg quot9 NOg N03g Step 2 Fast exothermic NO3g COg 9 NOzg COzg Overall reaction Exothermic N02g COg NOg C02g i Identify each of the following as reactant product or intermediate NOzg COg N03g COzg NOg ii Draw a reaction coordinate diagram for this reaction Indicate on this drawing the activation energy for each step and the overall reaction enthalpy Continued to page 5 MasudMonwar 2011 Ref Kotz 6medn 4 9 a The decomposition of ammonia is rst order with respect to NH3 2NH3g quotquot9 Nzg 3Hzg i What is the rate equation for this reaction ii Calculate the rate constant k given the following data NH3 molL Time s 067 0 026 19 iii Determine the halflife of NH3 b Ammonium cyanate NH4NCO rearranges in water to give urea NH22CO NH4NCOaq quot9 NH22COaq X 107 X 1 230 X 1 600 X 1 Using the data in the table i Decide whether the reaction is rst order or second order ii Calcualtek for this reaction iii Calculate the halflife of ammonium cyanate under these conditions iv Calculate the concentration of NH4NCO after 120 h c The decomposition of gaseous dimethyl ether at ordinary pressures is rst order Its halflife is 250 min at 500 C CH300H3g quot9 CH4g 00g Hzg i Starting with 800 g of dimethyl ether what mass remains in grams after 125 min and after 145 min ii Calculate the time in minutes required to decrease 760 ng nanograms to 225 ng iii What fraction of the original dimethyl ether remains after 150 min d The gasphase reaction 2N205g quot399 4 N02 02 has an activation energy of 103 k and the rate constant is 00900 min391 at 3280 K Find the rate constant at 3180 K Continued to page 6 MasudMonwar 2011 Ref Kotz 6medn 5 10 a The following statements relate to the reaction with the following rate law Rate lezlllzl Hzg12g9 2HIg Determine which of the following statements are true If a statement is false indicate why it is incorrect i The reaction must occur in a single step ii This is secondorder reaction overall iii Raising the temperature will cause the value of kto decrease iv Raising the temperature lowers the activation energy for this reaction v If the concentrations of both reactants are doubled the rate will double vi Adding a catalyst is the reaction will cause the initial rate to increase b Describe each of the following statements as true or false Iffalse rewrite the sentence to make it correct i the ratedetermining elementary step in a reaction is slowest step in a mechanism ii It is possible to change the rate constant by changing the temperature iii As a reaction proceeds at constant temperature the rate remains constant iv A reaction that is third order overall must involve more than one step Chapter 12 Chemical Eguilibrium 11 Write equilibrium constant expressions for the following reactions For gases use either pressures or concentrations i 2H202g G 2H20g 02g ii COg 12 02g G COzg iii Cs 002g cgt 2COg iv NiOs COg lt3 Nis 002g 12 a K 56 X 103912 at 500 K for the dissociation of iodine molecules to iodine atoms 12g a 21 g A mixture has 12 0020 molL and I 20 X 108 molL Is the reaction at equilibrium at 500 K If not which way must the reaction proceed to reach equilibrium 13 a The reaction P015gcgt Pcmg 0mg was examined at 250 C At equilibrium PC15 42 X 10395molL PC13 13 X 1039 2molL and C12 39 x 10393molL Calculate Kfor the reaction Continued to page 7 MasudMonwar 2011 Ref Kotz 6medn 6 b The reaction Cs COzg cgt 2COg occurs at high temperatures At 700 C a 20 L ask contains 010 mol of CO 020 mol of C02 and 040 mol of C at equilibrium i Calculate K for the reaction at 700 C ii Calculate K for the reaction also at 700 C if the amounts at equilibrium in the 20 L ask are 010 mol of CO 020 mol of C02 and 080 mol of C iii Compare the results of i and ii Does the quantity of carbon affect the value of K Explain 14 The equilibrium constant for the dissociation of iodine molecules to iodine atoms 12gcgt 21 g Is 376 X 10393 at 1000 K Suppose 0105 mol of I is placed in a 123 L ask at 1000 K What are the concentrations of I and I when the system comes to equilibrium 15 a Which of the following correctly relates the equilibrium constants for the two reactions shown A B cgt 2C K1 2A 2B cgt 4C K2 K2 2K1 K2 lK1 iii K2 K12 iv K2 1K12 b Calculate K for the reaction SnOzs 2COg Sns 2 COzg Given the following information SnOzs 2Hzg Sns 2HZO g K 812 H2g COzg cgt H20g CO g K 0771 ON Dinitrogen trioxide decomposes to NO and NO in an endothermic process AH 405 ldmol N203g G N0 N02g Predict the effect of the following changes on the position of the equilibrium that is state which way the equilibrium will shift left right or no change when each of the following changes is made i adding more N203g ii adding more NOzg iii increasing the volume of the reaction ask iv lowering the temperature Continued to page 8 MasudMonwar 2011 Ref Kotz 6medn 7 17 a The equilibrium constant Kc for the following reaction is 105 at 350 K 2CH2C12g G CH4g CCl4g If an equilibrium mixture of the three gases at 350 K contains 00206 M CHzClzg and 00163 M CH4 what is the equilibrium concentration of CCl4 b Heating ametal carbonate leads to decomposition BaC03s Ba0s COzg Predict the effect on the equilibrium of each change listed below Answer by choosing no change shz39 ts le t or shifts right i add BaC03 ii addBaO iii add C02 iv raise the temperature V increase the volume of the ask containing the reaction 18 Decide whether each of the following statements is true or false If false change the wording to make it true i The magnitude of the equilibrium constant is always independent of temperature ii When two chemical equations are added to give a net equation the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations iii Only the concentration of C02 appears in the equilibrium constant expression for the reaction CaC03s Ca0s COzg iv For the reaction CaCO3s lt3Ca0s COzg the value of K is numerically the same no matter whether the amount of C02 is expressed as moles liter or as gas pressure 19 Characterize each of the following as product or reactantfavored a COg 12 02g cgt 002g KP 12 X 1045 b H20 g Hzg 12 02g KP 91 x 10quot c COg 012g cgt COClzg KP 65 X 1011 20 The reaction of hydrogen and iodine to give hydrogen iodide has an equilibrium constant KC of 56 at 435 C a What is the value of KP b Suppose you mix 045 mol osz and 045 mol OH in a 100 L ask at 425 C What is the total pressure of the mixture before and after equilibrium is achieved c What is the partial pressure of each gas at equilibrium Continued to page 9 MasudMonwar 2011 Ref Kotz 6medn 8 Chapter 13 Electrochemistry l The halfcells Fe2 aq I Fe s and 02 g I H20 in acid solution are linked to create a voltaic cell a Write equations for the oxidation and reduction halfreactions and for the overall cell reaction b Which halfreaction occurs in the anode compartment and which occurs in the cathode compartment c Complete the following sentences Electrons in the external circuit ow from the electrode to the electrode Negative ion move in the salt bridge from the halfcell to the halfcell 2 Calculate the value of E for each of the following reactions Decide whether each is productfavored in the direction written a Zn aq Ni s quot9 Zn s Ni aq b 2 Cl39 aq Cu2 aq quot9 Cu s Cl2 g 3 Consider the following halfreactions 3e l66 a Based on E values which metal is the most easily oxidized Which metals on this list are capable of reducing Fe2 aq to Fe Write a balanced chemical equation for the reaction of Fell aq with Sn s Is this reaction productfavored or reactant favored d Write balanced chemical equation for the reaction of Zn2 aq with Sn s Is this reaction productfavored or reactantfavored as 4 Which of the following ions is most easily reduced Cu aq 3853 N B 3 3 V e A13 aq V39 Four voltaic cells are set up In each one halfcell contains a standard hydrogen electrode The second halfcell is one of the following Cr3 aq 10 M I Crs Fe2 aq 10M l Fes Cu aq 10 M l Cu s and Mg aq 10 M l Mg s Continued to page 10 MasudMonwar 2011 Ref Kotz 6medn 9 a In Which of the voltaic cells does the hydrogen electrode serve as the cathode b Which voltaic cell produces the highest voltage Which produces the lowest voltage Disclaimer 0 These questions can only be used as Study Guide and for practicing the contents of the syllabus announced for 4th Exam 0 The questions in the real exam might not have the samesimilar format but it will cover the similar concepts 0 These are only the highly possible questions not all the types of question to expect in the exam 0 This attempt has been made to help you do better in the exam not to raise issues If any issue is raised by any student regarding this type of attempt it might not be possible to continue further in future MasudMonwar 2011 Ref Kotz 6medn 10


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