Solution Found!
The rate law for the reaction 2NO2 (g)?N2O4(g) is rate =
Chapter 13, Problem 88P(choose chapter or problem)
The rate law for the reaction \(2 \mathrm{NO}_{2}(g) \rightarrow \mathrm{N}_{2} \mathrm{O}_{4}(g)\) is rate = \(k\left[N O_{2}\right]^{2}\). Which of the following changes will change the value of k? (a) The pressure of \(\mathrm{NO}_{2}\) is doubled. (b) The reaction is run in an organic solvent. (c) The volume of the container is doubled. (d) The temperature has decreased. (e) A catalyst is added to the container.
Questions & Answers
QUESTION:
The rate law for the reaction \(2 \mathrm{NO}_{2}(g) \rightarrow \mathrm{N}_{2} \mathrm{O}_{4}(g)\) is rate = \(k\left[N O_{2}\right]^{2}\). Which of the following changes will change the value of k? (a) The pressure of \(\mathrm{NO}_{2}\) is doubled. (b) The reaction is run in an organic solvent. (c) The volume of the container is doubled. (d) The temperature has decreased. (e) A catalyst is added to the container.
ANSWER:Step 1 of 3
We are provided with an equation
The rate law is given as
We need to find which of the following changes will change with
