12.3 Exercise 4

How will the rate of reaction change for the process: $\text{CO}( g \left.\right) + \text{NO}_{2} \left(g\right) \rightarrow \text{CO}_{2} \left(g\right) + \text{NO}( g \left.\right)$ if the rate law for the reaction is $\text{rate} = k \left[\text{NO}_{2}\right]^{2} ?$

(a) Decreasing the pressure of NO₂ from 0.50 atm to 0.250 atm.

(b) Increasing the concentration of CO from 0.01 M to 0.03 M.