Question

the gas - phase reaction 2o3(g) → 3o2(g) has been studied in a closed reaction container, and the rate law is determined to be: rate = (\frac{deltao_3}{delta t}=ko_3). which one of the following actions is least likely to cause a change in the rate of the reaction? continuously removing o2(g) as it is formed. using a larger reaction container, but the same initial amount of o3(g). lowering the temperature. using a larger initial amount of o3(g) in the same reaction container.

Explanation:

The rate law Rate = k[O₃] shows that the reaction rate depends only on the concentration of O₃. Changing the volume of the container (while keeping the initial amount of O₃ the same) doesn't directly affect the concentration of O₃ in terms of the rate - law expression. Lowering temperature affects the rate constant k, using a larger initial amount of O₃ changes the concentration of O₃ which affects the rate, and removing O₂ affects the equilibrium position and potentially the forward - reaction rate as the reaction proceeds. But changing the container volume without changing the amount of O₃ has the least impact on the rate based on the given rate law.

Answer:

Using a larger reaction container, but the same initial amount of O₃(g).