Collision Model Practice Test

In a kinetics lab, a student reacts aqueous iodide ions with aqueous hydrogen peroxide under acidic conditions to produce iodine. Two trials are run with the same total volume, the same temperature, and the same reaction mechanism (no catalyst; same species present). Trial 1 is vigorously stirred throughout, while Trial 2 is left unstirred. The iodine color develops faster in Trial 1. Which statement best explains why Trial 1 proceeds faster in terms of collision frequency or collision effectiveness?

A student studies the same reaction in two sealed flasks: $\text{NO}(g)+\text{O}_3(g)\rightarrow \text{NO}_2(g)+\text{O}_2(g)$. The mechanism is unchanged between trials, and the only difference is the temperature.

Condition 1: The gases are mixed at a lower temperature.

Condition 2: The gases are mixed at a higher temperature.

Which statement best explains why the reaction occurs faster in Condition 2 than in Condition 1, based on collision effectiveness?