Test1 Ch15 Kinetics Practice Problems

1General Chemistry IIJasperseKinetics. Extra Practice ProblemsGeneral Types/Groups of problems:Rates of Change in Chemical ReactionsThe look of concentration/time graphsp1p2P9P10P4First Order Rate Law CalculationsReaction Energy Diagrams, ActivationEnergy, Transition States Reaction Mechanisms,Intermediates Mechanism Steps and Rate LawsRates: Average Rates, Determination of Rates fromStoichiometry and Changes of Other ChemicalsReactant Order and Overall Reaction Orderp3Given a Rate Law, How much will rate change withchange in concentrationDetermining Reactant Orders from Actual DataActual Rate Law from Concentration/Rate DataDetermining Rate Constant from Actual Data.Where you yourself need to first deduce the rate law,then plug in the values to solve for “k”.P5CatalystsP14P6P7P8AnswersP15P12P13Rates of Change in Chemical Reactions1. For the reaction A 3B à 2C, how does the rate of disappearance of B compare to the rate of productionof C?a.b.c.d.the rate of disappearance of B is 1/2 the rate of appearance of Cthe rate of disappearance of B is 3/2 the rate of appearance of Cthe rate of disappearance of B is 2/3 the rate of appearance of Cthe rate of disappearance of B is 1/3 the rate of appearance of C2. For the reaction 2A 3B 4C 5D, the rate of the reaction in terms of ΔA would be written as:a. –ΔA/Δt.b. –1/2 ΔA/Δt.c. ΔA/Δt.d. 1/2 ΔA/Δt.e. –2 ΔA/Δt.3. For the reaction 2A 3B 4C 5D, the rate of the reaction in terms of ΔB would be written asa. –ΔB/Δtb. ΔB/Δtc. –1/3 ΔB/Δtd. 1/3 ΔB/Δte. –3 ΔB/Δt4. For the reaction 2A 3B 4C 5D, the rate of the reaction in terms of ΔC would be written asa.b.c. ΔC/Δt d. 4 ΔC/Δt 1/4 ΔC/Δtd.e.–4 ΔC/Δt–1/4 ΔC/Δt5. In the combustion of methane, CH4(g) 2 O2(g) CO2(g) 2 H2O (g), which reactant has the greatest rateof disappearance?a.b.c.d.e.CH4O2CO2H 2OCH4 and O2 have the same rate of disappearance.

2The look of concentration/time graphs6.7.Which of the following is not a possible graph of concentration versus time for a reactant?a.c.b.d.Assuming that each of the following graphs has the same concentration and time axes, which has the greatest initialrate of disappearance of reactant?a.c.b.d.8. The following graph shows the kinetics curves for the reaction of oxygen with hydrogen to form water:O2(g) 2H2(g) 2H2O(g). Which curve is hydrogen?a.the dashed curveb.the gray curvec.the black curved.either the gray or the black curvee. Any of these curves could be hydrogen

3Rates: Average Rates, Determination of Rates from Stoichiometry and Changes of OtherChemicals; Simple Rate Calculations9.A scientist conducts an experiment to determine the rate of the following reaction:N2(g) O2(g) 2NO(g)If the initial concentration of N2 was 0.500 M and the concentration of N2 was 0.450 M after 0.100 s, what is the rate of thereaction?a.b.c.0.500 M/s1.00 M/s5.00 M/sd.e.10.0 M/s0.250 M/s10. A scientist conducts an experiment to determine the rate of NO formation in the reaction:N2(g) O2(g) 2NO(g)If the initial concentration of N2 was 0.500 M and the concentration of N2 was 0.450 M after 0.100 s, what is the rate of NOformation?a.b.c.0.500 M/s1.00 M/s5.00 M/sd.e.10.0 M/s0.250 M/s11. If the rate of appearance of O2 in the reaction:2O3(g) 3O2(g)is 0.250 M/s over the first 5.50 s, how much oxygen will form during this time?a.b.c.1.38 M4.13 M0.69 Md.e.0.25 M0.46 M12. HI dissociates to form I2 and H2:2HI(g) H2(g) I2(g)If the concentration of HI changes at a rate of –0.45 M/s, what is the rate of appearance of I2(g)?a.b.c.0.90 M/s0.45 M/s0.23 M/sd.e.1.00 M/s0.13 M/s13. If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N2?N2 (g) 3 H2 (g) à 2 NH3 (g)a.b.c.0.173 M/s0.345 M/s0.690 M/sd.e.245 M/s0.518 M/s14. If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of H2?N2(g) 3H2(g) 2NH3(g)a.b.c.0.173 M/s0.345 M/s0.522 M/sd.e.245 M/s0.518 M/s

4Reactant Order and Overall Reaction Order15. For the reaction 2A B 2C à D 2E, the rate law is:Which of the following statements is false:a.b.c.d.the reaction is second order in [A]the reaction is first order in [B]the reaction is second order in [C]the reaction is 4th order overall16. For the reaction 1A 2B 1C à 2D 1E, the rate law is:Which of the following statements is false:a.b.c.d.rate k[A]2[B]1[C]1rate k [B]2[C]1the reaction is first order in [A]the reaction is second order in [B]the reaction is first order in [C]the reaction is third order overall17. For the rate law Rate k[A]1/2[B], the partial order with respect to A is , the partial order with respect to Bis , and the total order is .a.b.c.d.e.1/2; 0; 1/21/2; 1; 11/2; 1; 3/21/2The orders cannot be determined without a chemical reaction.18. For the rate law Rate k[A][B]3/2, the order with respect to A is , the order with respect to B is, and the overall reaction order is .a.b.c.d.e.0; 3/2; 3/21; 3/2 ; 11; 3/2 ; 5/21; 3/2; 7/2The orders cannot be determined without a chemical reaction.19. The reaction A 2B Cis first order in B and A. The overall order of the reaction isa.b.c.first.second.third.d.e.zero.fourth.

5Given a Rate Law, How much will rate change with change in concentration20. The reaction CHCl3(g) Cl2(g) CCl4(g) HCl(g) has the following rate law: Rate k[CHCl3][Cl2]. If theconcentration of CHCl3 is increased by a factor of five while the concentration of Cl2 is kept the same, the rate willa.b.c.double.triple.stay the same.d.e.increase by a factor of five.decrease by a factor of one-fifth.21. The reaction 2NO(g) O2(g) 2NO2(g) has the following rate law: Rate k[O2][NO]2. If the concentration of NO isreduced by a factor of two, the rate willa.b.c.double.quadruple.be reduced by one-quarter.d.e.be reduced by one-half.remain the same.22. The rate of a reaction is found to double when the concentration of one reactant is quadrupled. The order of thereaction with respect to this reactant d.

6Determining Reactant Orders from Actual Data23. Given the following data, determine the order of the reaction with respect to Cl2.2NO(g) Cl2(g) 2NOCl(g)Experiment123a.b.c.[NO] (M)0.03000.01500.0150firstsecondthird[Cl2] (M)0.01000.01000.0400d.e.Rate (M/s)3.4 10–48.5 10–53.4 10–4fourthfifth24. Given the following data, determine the order of the reaction with respect to H2.H2(g) 2ICl(g) I2(g) 2HCl(g)Experiment123a.b.c.[H2] (torr)25025050one-halfsecondfirst[ICl] (torr)32581325d.e.Rate (M/s)1.340.3310.266thirdthree-halves25. Given the following data, determine the order of the reaction with respect to NO(g).2NO(g) Cl2(g) 2NOCl(g)Experiment123a.b.c.[NO] (M)0.03000.01500.0150firstsecondthird[Cl2] (M)0.01000.01000.0400d.e.Rate (M/s)3.4 10–48.5 10–53.4 10–4fourthfifth26. Determine the overall order of the reaction: H2(g) 2ICl(g) I2(g) 2HCl(g) from the following data:Experiment123a.b.c.PH (torr)25025050firstsecondthirdPICl (torr)32581325d.e.Rate (torr/s)1.340.3310.266fourthzeroth27. Determine the overall order of the reaction 2NO(g) Cl2(g) 2NOCl(g) from the following data:Experiment123a.b.c.firstsecondthird[NO] (M)0.03000.01500.0150[Cl2] (M)0.01000.01000.0400d.e.fourthfifthRate (M/s)3.4 10–48.5 10–53.4 10–4

7Actual Rate Law from a Table of Concentration/Rate Data28. Given the following data, determine the rate law for the reactionNH4 (aq) NO2–(aq) N2(g) 2H2O()a.b.c.Experiment[NH4 ] (M)[NO2–] (M)Rate (M/s)1230.25000.50000.25000.25000.25000.12501.25 10–32.50 10–36.25 10–4k[NH4 ][NO2–]k[NH4 ]2[NO2–]k[NH4 ][NO2–]1/2d.e.k[NH4 ]1/2[NO2–]2k[NH4 ][NO2–]229. Given the following data, determine the rate law for the reaction2NO(g) Cl2(g) 2NOCl(g)Experiment123a.b.c.Rate k[NO][Cl2]Rate k[NO][Cl2]2Rate k[NO]2[Cl2]30. What is the rate law for the reactionInitial [A]0.2730.8190.2730.273a.b.c.d.[NO] (M)0.03000.01500.0150Initial [B]0.7630.7631.5260.763rate k[A][B][C]rate k[A][B]2[C]rate k[A]3[B]4[C]2rate k[A]2[B]2[C]2[Cl2] (M)0.01000.01000.0400d.e.Rate k[NO]2[Cl2]2Rate k[NO][Cl2]1/22A 2B 2C à productsInitial [C]0.4000.4000.4000.800rate3.09.012.06.0Rate (M/s)3.4 10–48.5 10–53.4 10–4

8Determining Rate Constant from Rate Law and Actual Data. Where you yourself need to firstdeduce the rate law, then plug in the values to solve for “k”.31. The initial rate data for the reaction 2N2O5(g) 4NO2(g) O2(g) is shown in the following table. Determine the valueof the rate constant for this reaction.Experiment[N2O5](M)Rate (M/s)2122.51.28 10222.56 x 1045.0a.b.c.4.09 s–10.176 s–10.0569 s–1d.e.0.225 s–180.1 s–132. Given the following data, determine the rate constant of the reaction2NO(g) Cl2(g) 2NOCl(g)Experiment123a.b.c.1.13 M –2s–19.44 M –2s–137.8 M –2s–1[NO] (M)0.03000.01500.0150[Cl2] (M)0.01000.01000.0400d.e.0.0265 M –2s–159.6 M –2s–1Rate (M/s)3.4 10–48.5 10–53.4 10–4

9First Order Rate Law CalculationsFormulas for First Order Reactions: kt ln ([Ao]/[At])-these formulas will be provided for you on the testkt1/2 0.69333. The first-order reaction A B, has k 8.00 s–1. If [A]0 0.500 M, how long will it take [A] 0.200 M?a.b.c.0.115 s0.100 s8.18 sd.e.0.244 s.0.488 s34. The first-order reaction A B, has k 5.67 s–1. If [A]0 0.500 M, how long will it take [A] 0.124 M?a.b.c.0.122 s0.100 s8.18 sd.e.0.244 s0.488 s35. A reaction is first order in A. If the rate constant of the reaction is 6.00 10–3 s–1, what is the half-life (t1/2) of thereaction?a.b.c.4.98 10–3 s200 s3.45 10–3 sd.e.115 s1.73 10–3 s36. A reaction is first order in A. If the rate constant of the reaction is 3.45 10–3 s–1, what is the half-life (t1/2) of thereaction?a.b.c.4.98 10–3 s201 s3.45 10–3 sd.e.100 s1.73 10–3 s37. The half-life (t1/2) of a first-order reaction is 0.100 s. What is the rate constant?a.b.c.6.93 s–10.693 s–10.0693 s–1d.e.0.144 s–13.01 s–138. The half-life (t1/2) of a first-order reaction is 0.950 s. What is the rate constant?a.b.c.6.93 s–10.729 s–10.0693 s–1d.e.0.144 s–13.01 s–139. What percentage of a material will persist after 60 minutes if it’s half life is 30 minutes?a.b.c.d.e.50%33%25%12.5%none of the above40. What percentage of a material will persist after 80 minutes if it’s half life is 20 minutes?a.b.c.d.e.50%33%25%12.5%6.25%

10Reaction Energy Diagrams, Activation Energy, Transition States 41. Which point as labeled by an asterisk (*) on the following energy profile is the transition state?a.c.b.d.42. The energy profiles for four different reactions are shown. Which reaction requires the most energetic collisions toreach the transition state?a.b.abc.d.cd

1143. The following energy profiles for four different reactions are shown. Which reaction is the most endothermic?a.b.abc.d.cd44. The following energy profiles for four different reactions are shown. Which reaction is the most exothermic?a.b.abc.d.cd45. Collision theory assumes that the rate of a reaction depends ona.b.c.d.e.the energy of collisions.the orientation of colliding molecules.the energy of collisions and the orientation of colliding molecules.the change in energy between the products and the reactants.the change in free energy between the reactants and products.