The reaction of nitrogen dioxide with carbon monoxide is given below:
NO2 + CO NO + CO2

Is second order in NO2 and zero order in CO.

a. Complete the rate law for this reaction.
b. In an experiment to determine the rate law, the rate constant was determined to be 0.790 M-1s-1. Using this value for the rate constant, the rate of the reaction when [NO2] = 1.23 M and [CO] = 0.221 M would be:

Explanation:

NO2 + CO --> NO + CO2

Is second order in NO2 and zero order in CO.

A. Rate law for the reaction:

Rate = K[NO2]²[CO]⁰

Rate = K[NO2]²

B.

k = 0.790 M-1s-1

[NO2] = 1.23 M

[CO] = 0.221 M

Rate = ?

Rate = K[NO2]²[CO]⁰

Rate = 0.790  *  1.23² * 0.221⁰

Rate = 0.790  *  1.23² * 1 =  1.1952M/s

metric time was an attempt to create a standard unit of time based off of 10, but it never took off an is not included in the metric system (si)