A.P. Chemistry Practice Test - Ch. 12 - Kinetics

Sep 30, 2026

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A.P. Chemistry practice test covering reaction kinetics and chemical rate laws for Chapter 12, Kinetics. Multiple-choice problems address average rates of disappearance/appearance, valid units for reaction rates, concentration-time data tables, and calculation of reaction order with respect to reactants. Additional questions determine half-life and solve first- and second-order integrated rate law problems using given rate constants, including reaction-rate factor changes and graph interpretation for slopes and constants.

LanguageEnglish

CategoryExam

FormatPDF

Pages15

Reading Time38 min

AccessFree to download

Multiple Choice Questions

Reaction Rates and Units

Rate Laws and Reaction Order

Integrated Rate Laws and Half-Life

Interpreting Data Tables and Graphs

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 ofA 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) | 1 | 10 | 20 | 30 | 40 | | --- | --- | --- | --- | --- | --- | | Moles of A | 0.124 | 0.110 | 0.088 | 0.073 | 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 (S 2O82- ) 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 ofS2O82-ion and 0.072 M ofI-is prepared, and the progress of the reaction followed by measuring [I- ]. The data obtained is given in the table below. | Time (s) | 0 | 400 | 800 | 1200 | 1600 | | --- | --- | --- | --- | --- | --- | | [I- ](M) | 0.072 | 0.057 | 0.046 | 0.037 | 0.029 | 5) The concentration of S2O82-remaining at 800 s is M. A) 0.015 B) 0.041 C) 0.076 D) 4.00 ˛10-3 E) 0.046 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 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 The data in the table below were obtained for the reaction: 2 ClO2(aq) + 2 OH- (aq) ¬ ClO3- (aq) + ClO2- (aq) + H2O (1) | Experiment
Number | [ClO 2](M) | [OH- ](M) | Initial Rate
(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 D) 2 10) What is the order of the reaction with respect to OH-? A) 0 B) 1 C) 2 D) 3 11) What is the overall order of the reaction? A) 0 B) 1 C) 4 D) 3 12) What is the magnitude of the rate constant for the reaction? A) 115 B) 1.15 x 104 C) 713 D) 4.6 13) For a first-order reaction, a plot of versus is linear. A) ln [A]t, t B) ~~ [~~1A~~]~~t~~ ~~, t C) In [A] t, ~~ ~~1t~~ ~~ D) [A] t, t E) 3 E) 4 E) 2 E) 230 E) t, ~~ [~~1A~~]~~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)

FAQs

How do you relate the average rate of appearance of B to the rate of disappearance of A?

Use stoichiometry from the balanced reaction. The relationship comes from comparing D[B]/Dt with the corresponding D[A]/Dt multiplied by the stoichiometric coefficients and sign changes.

What determines the order of a reaction with respect to a reactant like B or ClO2?

The order is inferred from how the reaction rate changes when that reactant concentration is changed while other reactants are held constant, using the rate law proportionality.

How are first-order and second-order integrated rate laws used in these problems?

First-order problems use ln[A] versus time (or equivalent integrated form) and half-life relations; second-order problems use 1/[A] versus time (or equivalent integrated form) to solve for time or concentration changes.

Sep 30, 2026

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