The information in the data table above represents two different trials for an experiment to study the rate of the reaction between NO_(g) and H_2(g), as represented by the balanced equation above the table. Which of the following statements provides the correct explanation for why the initial rate of formation of N₂ is greater in trial 2 than in trial 1? Assume that each trial is carried out at the same constant temperature.

Transcribed Image Text:

O The activation energy of the reaction is smaller in trial 2 than it is in trial1 O The value of the rate constant for the reaction is greater in trial 2 than it is in trial 1. O The value of the rate constant for the reaction is smaller in trial 2 than it is in trial 1. O The frequency of collisions between reactant molecules is greater in trial 2 than it is in trial 1. O The activation energy of the reaction is smaller in trial 2 than it is in trial1 O The value of the rate constant for the reaction is greater in trial 2 than it is in trial 1. O The value of the rate constant for the reaction is smaller in trial 2 than it is in trial 1. O The frequency of collisions between reactant molecules is greater in trial 2 than it is in trial 1.