2 NO(g) + 2 H2(g) N2(g) + 2 H20() Trial Initial Conc. Initial Conv. Initial Rate of NO (M). H2(M). Formation N2 (M/S) 1 0.10 0.10 1.2 x 10-3 2 0.10 0.20 2.4 x 10-3 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 H2(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. The activation energy of the reaction is smaller in trial 2 than it is in trial 1 The value of the rate constant for the reaction is greater in trial 2 than it is in trial 1. The value of the rate constant for the reaction is smaller in trial 2 than it is in trial 1. The frequency of collisions between reactant molecules is greater in trial 2 than it is in trial 1