The reaction described by this equation O_3(g) + NO(g) rightarrow O_2(g) + NO_2(g) has the...

Question:

The reaction described by this equation

{eq}O_3(g) + NO(g) \rightarrow O_2(g) + NO_2(g) {/eq}

has the following rate law at 310 K.

rate of reaction = {eq}K[O_3][NO]; k = 3.0 \times 10^6 M^{-1} \cdot s^{-1} {/eq}

a. Given that {eq}[O_3] = 8.0 \times 10^4 {/eq} M and {eq}[NO] = 8.0 \times 10^{-5} {/eq} M at t = 0, calculate the rate of the reaction at t = 0.

b. What is the overall order of this reaction?

A. 0

B. 1

C. 2

D. 3

Rates of Reaction

The rate of a chemical reaction is often written in terms of a rate constant and the concentrations of the reagents. The respective powers to which the concentrations of the species are raised are known as the orders of the reaction with respect to that species. The overall order is the sum of all the powers.

Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answer

The rate of reaction can be computed by direct substitution of the data in the question:

{eq}rate = (3.0 \times 10^6)(8.0 \times 10^4)(8.0 \times...

See full answer below.


Learn more about this topic:

Loading...
Rate Constant and Rate Laws

from

Chapter 12 / Lesson 2
15K

Rate law is defined as the relationship between the rate of reaction and the concentration of the reactants. Learn about rate law, rate constant, and how to use rate law equations to determine reaction order for one or two reactants.


Related to this Question

Explore our homework questions and answers library