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Ch.14 - Chemical Kinetics
All textbooksBrown 14th EditionCh.14 - Chemical KineticsProblem 89b
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Chapter 14, Problem 89b

Consider the reaction A + B → C + D. Is each of the following statements true or false? (b) If the reaction is an elementary reaction, the rate law is second order.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Elementary Reactions

An elementary reaction is a single step process in which reactants are converted to products in a single transition state. The rate of an elementary reaction is directly related to the molecularity, which is the number of reactant molecules involved. For example, a reaction involving two reactant molecules is bimolecular and typically has a rate law that reflects this molecularity.
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Rate Law

The rate law of a chemical reaction expresses the relationship between the rate of the reaction and the concentration of its reactants. It is determined experimentally and can vary depending on the reaction mechanism. For elementary reactions, the rate law can be directly derived from the stoichiometry of the reaction, meaning that the exponents in the rate law correspond to the coefficients in the balanced equation.
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Order of Reaction

The order of a reaction is the sum of the powers of the concentration terms in the rate law. It indicates how the rate of reaction is affected by the concentration of reactants. A second-order reaction can arise from either a single elementary reaction involving two reactant molecules or from two first-order reactions, thus the statement in the question can be true if the reaction is indeed second order.
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Textbook Question

The enzyme urease catalyzes the reaction of urea, 1NH2CONH22, with water to produce carbon dioxide and ammonia. In water, without the enzyme, the reaction proceeds with a first-order rate constant of 4.15 * 10-5 s-1 at 100 C. In the presence of the enzyme in water, the reaction proceeds with a rate constant of 3.4 * 104 s-1 at 21 C. (c) In actuality, what would you expect for the rate of the catalyzed reaction at 100 C as compared to that at 21 C?

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Textbook Question

The activation energy of an uncatalyzed reaction is 95 kJ/mol. The addition of a catalyst lowers the activation energy to 55 kJ/mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (a) 25 C

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Textbook Question

The activation energy of an uncatalyzed reaction is 95 kJ/mol. The addition of a catalyst lowers the activation energy to 55 kJ/mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (b) 125 °C?

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Textbook Question

Consider the reaction A + B → C + D. Is each of the following statements true or false? (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order.

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Textbook Question

The reaction 2 NO(g) + O2(g) → 2 NO2 (g) is second order in NO and first order in O2. When [NO] = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10-5 M/s. (b) What is the value of the rate constant?

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Textbook Question

The reaction 2 NO(g) + O2(g) → 2 NO2 (g) is second order in NO and first order in O2. When [NO] = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10-5 M/s. (c) What are the units of the rate constant?

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