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A.P. Chemistry Practice Test: Ch. 12, Kinetics




A.P. Chemistry Practice Test: Ch. 12, Kinetics;MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.;1) Consider the following reaction;3A 2B;The average rate of appearance of B is given by D[B]/Dt. Comparing the rate of appearance of B and the rate of;disappearance of A, we get D[B]/Dt = _____ x (-D[A]/Dt).;A) -2/3;B) -3/2;C) +2/3;D) +3/2;E) +1;2) A burning splint will burn more vigorously in pure oxygen than in air because;A) nitrogen is a reactant in combustion and its low concentration in pure oxygen catalyzes the combustion.;B) oxygen is a reactant in combustion and the concentration of oxygen is higher in pure oxygen than it is in;air.;C) oxygen is a product of combustion.;D) nitrogen is a product of combustion and the system reaches equilibrium at a lower temperature.;E) oxygen is a catalyst for combustion.;3) Of the following, all are valid units for a reaction rate except __________.;A) mol/L;B) M/s;C) mol/hr;D) mol/L-hr;E) g/s;A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) B(g). The following data are;obtained for [A] as the reaction proceeds;Time (s);Moles of A;1;0.124;10;0.110;20;0.088;30;0.073;40;0.054;4) The average rate of disappearance of A between 10 s and 20 s is __________ mol/s.;A) 1.1 10-3;B) 4.4 10-3;C) 454;D) 9.90 10-3;E) 2.2 10-3;The peroxydisulfate ion (S2O82-) reacts with the iodide ion in aqueous solution via the reaction;S2O82- (aq) + 3I - 2SO4 (aq) + I3- (aq);An aqueous solution containing 0.050 M of S2O82- ion and 0.072 M of I- is prepared, and the progress of the reaction followed by;measuring [I- ]. The data obtained is given in the table below.;Time (s);[I- ] (M);0;400;800;1200;1600;0.072 0.057 0.046 0.037 0.029;5) The concentration of S 2O82- remaining at 800 s is _________ M.;A) 0.015;B) 0.041;C) 0.076;D) 4.00 10-3;6) Of the units below, ________ are appropriate for a first-order reaction rate constant.;A) L mol -1 s-1;B) s -1;C) M-1 s-1;D) mol/L;1;E) 0.046;E) M s-1;7) If the rate law for the reaction;2A + 3B products;is first order in A and second order in B, then the rate law is rate = __________.;A) k[A]2[B] 3;B) k[A]2[B]2;C) k[A][B];D) k[A]2[B];E) k[A][B] 2;8) The kinetics of the reaction below were studied and it was determined that the reaction rate increased by a;factor of 9 when the concentration of B was tripled. The reaction is __________ order in B.;A + B P;A) zero;B) first;C) second;D) third;E) one-half;D) 2;E) 3;C) 2;D) 3;E) 4;C) 4;D) 3;E) 2;D) 4.6;E) 230;The data in the table below were obtained for the reaction;2 ClO2 (aq) + 2 OH- (aq) ClO3- (aq) + ClO2- (aq) + H2O (1);Experiment;Initial Rate;Number;[ClO2] (M) [OH- ] (M) (M/s);1;0.060;0.030;0.0248;2;0.020;0.030;0.00276;3;0.020;0.090;0.00828;9) What is the order of the reaction with respect to ClO2?;A) 4;B) 1;C) 0;10) What is the order of the reaction with respect to OH-?;A) 0;B) 1;11) What is the overall order of the reaction?;A) 0;B) 1;12) What is the magnitude of the rate constant for the reaction?;A) 115;B) 1.15 x 104;C) 713;13) For a first-order reaction, a plot of __________ versus __________ is linear.;1;1;A) ln [A]t, t;B),t;C) In [A]t;D) [A]t, t;[A]t;t;2;E) t;1;[A]t;14) The rate law for a reaction is;rate = k [A][B]2;Which one of the following statements is false?;A) If [B] is doubled, the reaction rate will increase by a factor of 4.;B) The reaction is second order in B.;C) The reaction is first order in A.;D) k is the reaction rate constant;E) The reaction is second order overall.;15) The half-life of a first-order reaction __________.;A) is constant;B) is the time necessary for the reactant concentration to drop to half its original value;C) can be calculated from the reaction rate constant;D) does not depend on the initial reactant concentration;E) All of the above are correct.;16) The reaction;CH3-NC CH3-CN;is a first-order reaction. At 230.3e C, k = 6.29 x 10-4 s -1. If [CH3-NC] is 1.00 x 10-3 initially, [CH3-NC] is;after 1.000 x 103 s.;A) 4.27 x 10-3;B) 2.34 x 10-4;C) 5.33 x 10-4;3;D) 1.88 x 10-3;E) 1.00 x 10-6;17) Which one of the following graphs shows the correct relationship between concentration and time for a reaction;that is second order in [A]?;A);B);C);D);E);18) A first-order reaction has a rate constant of 0.33 min-1. It takes __________ min for the reactant concentration;to decrease from 0.13 M to 0.088 M.;A) 1.2;B) 1.4;C) 0.13;D) 0.85;E) 0.51;19) The rate constant for a second-order reaction is 0.13 M-1s -1. If the initial concentration of reactant is;0.26 mol/L, it takes __________ s for the concentration to decrease to 0.13 mol/L.;A) 1.0;B) 4.4 x 10-3;C) 0.017;D) 0.50;E) 30;4;20) The graph shown below depicts the relationship between concentration and time for the following chemical;reaction.;The slope of this line is equal to __________.;A) -k;B) -1/k;C) k;D) ln[A]o;21) The rate constant of a first-order process that has a half-life of 225 s is __________ s -1.;A) 3.08 x 10-3;B) 12.5;C) 1.25;D) 4.44 x 10-3;E) 1/k;E) 0.693;22) At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN);CH3NC (g) CH 33CN (g);The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9e;C.;The rate constant for the reaction is __________ s-1.;A) -5.2 10-5;B) +1.9 104;C) +6.2;D) -1.9 104;E) +5.2 10-5;23) The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction;2N2O5 (soln) 4NO2 (soln) + O2 (soln);The reaction is first order and has a rate constant of 4.82 10-3 s-1 at 64e C. The rate law for the reaction is rate;= _________.;[N2O5]2;[NO2]4 [O2];A) k;B) k[N2O5]2;C) k[N2O5];D) 2k[N2O5];E) k;[NO2]4 [O2];[N2O5]2;5;24) The rate of a reaction depends on __________.;A) collision frequency;B) collision orientation;C) collision energy;D) all of the above;E) none of the above;25) Which energy difference in the energy profile below corresponds to the activation energy for the forward;reaction?;A) x;B) y;C) x + y;D) y - x;E) x - y;26) In the energy profile of a reaction, the species that exists at the maximum on the curve is called the __________.;A) product;B) enthalpy of reaction;C) atomic state;D) activated complex;E) activation energy;27) In the Arrhenius equation;k = Ae-Ea/RT;is the frequency factor.;A) k;B) A;C) e;6;D) R;E) Ea;28) At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN);CH3NC (g) CH 3CN (g);The dependence of the rate constant on temperature is studied and the graph below is prepared from the;results.;The energy of activation of this reaction is _______ kJ/mol.;A) 4.4 10-7;B) 1.9 104;C) 1.6 105;D) 160;E) 4.4 10-4;D) D;E) X;29) The mechanism for formation of the product X is;A + B C + D;B + D X;(slow);(fast);The intermediate reactant in the reaction is __________.;A) A;B) B;C) C;30) For the elementary reaction;NO3 + CO NO2 + CO2;the molecularity of the reaction is __________, and the rate law is rate = __________.;A) 4, k[NO3][CO][NO2][CO2];B) 2, k[NO3][CO]/[NO2][CO2];C) 4, k[NO2][CO2]/[NO3][CO];D) 2, k[NO2][CO2];E) 2, k[NO3][CO];31) Of the following, __________ will lower the activation energy for a reaction.;A) increasing the concentrations of reactants;B) adding a catalyst for the reaction;C) raising the temperature of the reaction;D) removing products as the reaction proceeds;E) increasing the pressure;7;32) The rate law of the overall reaction;A + B C;is rate = k[A]2. Which of the following will not increase the rate of the reaction?;A) increasing the concentration of reactant A;B) increasing the temperature of the reaction;C) increasing the concentration of reactant B;D) adding a catalyst for the reaction;E) All of these will increase the rate.;33) A particular first-order reaction has a rate constant of 1.35 102 s -1 at 25e C. What is the magnitude of k at 75e C;if Ea = 85.6 kJ/mol?;A) 670;B) 3.47 104;C) 3.85 106;8;D) 1.93 104;E) 1.36 102;Answer Key;Testname: CH_12_PRAC_TEST_KINETICS.TST;MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.;1) C;ID: chem9b 14.1-1;2) B;ID: chem9b 14.1-2;3) A;ID: chem9b 14.1-3;4) E;ID: chem9b 14.1-9;5) B;ID: chem9b 14.1-19;6) B;ID: chem9b 14.1-24;7) E;ID: chem9b 14.1-26;8) C;ID: chem9b 14.1-28;9) D;ID: chem9b 14.1-37;10) B;ID: chem9b 14.1-38;11) D;ID: chem9b 14.1-39;12) E;ID: chem9b 14.1-40;13) A;ID: chem9b 14.1-41;14) E;ID: chem9b 14.1-42;15) E;ID: chem9b 14.1-45;16) C;ID: chem9b 14.1-47;17) E;ID: chem9b 14.1-49;18) A;ID: chem9b 14.1-50;19) E;ID: chem9b 14.1-52;20) A;ID: chem9b 14.1-54;21) A;ID: chem9b 14.1-60;1;Answer Key;Testname: CH_12_PRAC_TEST_KINETICS.TST;22) B;ID: chem9b 14.1-65;23) C;ID: chem9b 14.1-67;24) D;ID: chem9b 14.1-69;25) A;ID: chem9b 14.1-70;26) D;ID: chem9b 14.1-71;27) B;ID: chem9b 14.1-72;28) D;ID: chem9b 14.1-74;29) D;ID: chem9b 14.1-75;30) E;ID: chem9b 14.1-77;31) B;ID: chem9b 14.1-80;32) C;ID: chem9b 14.1-81;33) D;ID: chem9b 14.2-12;2


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