Assertion (A): If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason (R): Lower the activation energy, faster is the reaction.

The Arrhenius expression is k=Ae-Ea/RT When the activation energy is zero, the term e-Ea/RT becomes equal to 1. Hence, the rate constant becomes independent of the temperature. When the value of the activation energy is low, the value of the rate constant is higher. Hence, the rate of the reaction is also high. Comprehension Based Questions Concentrations measured as a function of time when gaseous N₂O₅ at initial concentration of 0.0200 M decomposes to gaseous NO₂ and O₂ at 55ºC. The change in concentration with time is given by the following graph.