Suppose that when the two reactions described in Practice Problems 13.17 and 13.18 are run at the same temperature and the same concentrations, the NO reaction goes much, much faster than the H₂O₂ reaction.

(a) What can you say about the relative sizes of the k values for the reactions?

(b) What can you say about the relative sizes of the E_a values for the reactions?

(c) What are three ways you might speed up the slow reaction to make it faster than the fast reaction?

Data from Problem 13.17

Write a general rate law for the reaction 2NO + O₂ → 2 NO₂ using x and y as orders.

Data from Problem 13.18

Write a general rate law for the reaction

using x, y and z as orders.

Transcribed Image Text:

H,Oz(aq)+3I(aq)+2H*(aq)→I (aq)+2H,O(l)