The Maxwell-Boltzmann energy distribution curves for a closed system containing a gas-phase mixture at two different temperatures, T1 T_1\,T1 and T2T_2T2, are shown.
Which of the following statements correctly identifies the relative temperatures and explains the primary reason for the increased rate of reaction at the higher temperature?
T2>T1T_2 > T_1T2>T1; the increase in reaction rate at T2T_2T2 is primarily due to a significant increase in collision frequency.
T2>T1T_2 > T_1T2>T1; the increase in reaction rate at T2T_2T2 is primarily because a much greater proportion of molecules have energy greater than or equal to EaE_aEa, while EaE_aEa remains constant.
T1>T2T_1 > T_2T1>T2; the reaction rate is higher at T1T_1T1 because the higher peak represents a greater proportion of reactant molecules colliding with the most probable energy.
T2>T1T_2 > T_1T2>T1; the increase in reaction rate at T2T_2T2 is because the average kinetic energy of the particles is higher, which lowers the activation energy EaE_aEa.