Final answer:
The rate of reaction for CO(g) + NO₂(g) will only increase with the square of the concentration of NO₂, according to the rate law rate = k[NO₂]². The concentration of CO does not affect the rate, as it is zero order with respect to CO, and changes in products NO and CO₂ are not accounted for in the rate law.
Step-by-step explanation:
The rate of reaction for the process: CO(g) + NO₂(g) ➡ CO₂(g) + NO(g) can be affected by changes in the concentrations of the reactants according to the given rate law.
Looking at the rate law, rate = k[NO₂]², we see that the reaction rate depends only on the concentration of nitrogen dioxide (NO₂). It is second order with respect to NO₂, which means that if the concentration of NO₂ is doubled, the rate increases by a factor of four (since 2² = 4).
Accordingly, answering the question directly based on the rate law rate = k[NO₂]²:
a) The rate of the reaction will not increase with an increase in the concentration of CO, since the rate law indicates the reaction is zero order with respect to CO.
b) The rate of the reaction will not increase with an increase in the concentration of NO, since NO is a product and does not appear in the rate law.
c) The rate of the reaction will not decrease with an increase in the concentration of CO₂ since CO₂ is a product and does not influence the rate according to the rate law.
d) The rate of reaction will increase with the square of the concentration of NO₂, as indicated by the reaction being second order in NO₂.