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.

Verified step by step guidance

Identify the general form of the rate law: \( \text{Rate} = k[A]^m[B]^n[C]^p \).

Determine the order of reaction with respect to each reactant: \( m = 0 \) for A, \( n = \frac{1}{2} \) for B, and \( p = 2 \) for C.

Substitute the orders into the rate law expression: \( \text{Rate} = k[A]^0[B]^{1/2}[C]^2 \).

Simplify the expression by noting that any concentration raised to the power of zero is 1: \( \text{Rate} = k[B]^{1/2}[C]^2 \).

The final rate law for the reaction is \( \text{Rate} = k[B]^{1/2}[C]^2 \).

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

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

Order of Reaction

The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate law. It indicates how the rate of reaction is affected by the concentration of that reactant. For example, a zero-order reaction means the rate is independent of the concentration of that reactant, while a first-order reaction means the rate is directly proportional to its concentration.

Rate Law

The rate law is an equation that relates the rate of a chemical reaction to the concentrations of the reactants, each raised to a power corresponding to its order in the reaction. It is typically expressed in the form: Rate = k[A]^m[B]^n[C]^p, where k is the rate constant, and m, n, and p are the orders of the reactants A, B, and C, respectively. Understanding the rate law is crucial for predicting how changes in concentration affect the reaction rate.

Rate Constant (k)

The rate constant, denoted as k, is a proportionality factor in the rate law that is specific to a given reaction at a specific temperature. It reflects the intrinsic speed of the reaction and is influenced by factors such as temperature and the presence of catalysts. The value of k can vary with the order of the reaction and is essential for calculating the rate of the reaction under different conditions.

Recommended video:

Guided course

01:14

Equilibrium Constant K

Related Practice

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.)

views

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. b. What is the overall order of 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. 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? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?

views

Textbook Question

Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.

[A] (M) Initial Rate (M/s)

0.050 0.100

0.075 0.225

0.090 0.324