A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C. b. What is the overall order of the reaction?

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Identify the order of the reaction with respect to each reactant: first order in A, second order in B, and zero order in C.

Recall that the overall order of a reaction is the sum of the orders with respect to each reactant.

Add the orders of the reactants: first order (A) + second order (B) + zero order (C).

Calculate the sum: 1 (from A) + 2 (from B) + 0 (from C).

The overall order of the reaction is the result of this sum.

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Key Concepts

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

Reaction Order

The reaction order is a key concept in chemical kinetics that indicates the relationship between the concentration of reactants and the rate of the reaction. It is determined by the sum of the powers of the concentration terms in the rate law. For example, if a reaction is first order in A and second order in B, the overall order is the sum of these orders.

Rate Law

The rate law expresses the rate of a chemical reaction as a function of the concentration of its reactants, each raised to a power corresponding to its order in the reaction. The general form is Rate = k[A]^m[B]^n[C]^p, where k is the rate constant, and m, n, and p are the orders with respect to reactants A, B, and C, respectively. Understanding the rate law is essential for determining the overall order of the reaction.

Zero Order Reactions

In zero order reactions, the rate of reaction is independent of the concentration of the reactant. This means that changes in the concentration of a zero-order reactant do not affect the rate of the reaction. In the given question, since C is zero order, it does not contribute to the overall order, which is calculated solely from the other reactants.

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Textbook Question

This reaction is first order in N₂O₅: N₂O₅(g) → NO₃(g) + NO₂(g) The rate constant for the reaction at a certain temperature is 0.053/s. a. Calculate the rate of the reaction when [N₂O₅] = 0.055 M

Textbook Question

This reaction is first order in N₂O₅: N₂O₅(g) → NO₃(g) + NO₂(g) The rate constant for the reaction at a certain temperature is 0.053/s. b. What would the rate of the reaction be at the concentration indicated in part a if the reaction were second order? Zero order? (Assume the same numerical value for the rate constant with the appropriate units.)

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Textbook Question

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.

a. Write a rate law for the reaction.

Textbook Question

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if the concentrations of all three reactants are doubled?

Textbook Question

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. a. Write a rate law for the reaction.