Based on the provided energy profile diagram,how many steps are in the mechanism of the reaction?

The rate constants of a reaction at $500 \, K$ and $700 \, K$ are $0.02 \, s^{-1}$ and $0.07 \, s^{-1}$ respectively. Calculate the values of $E_{a}$ and $A$.

Which of the following is true for a reaction as per collision theory?

The energy of activation is

For a gaseous reaction,a large increase in the rate of reaction with a small increase in temperature indicates:

Among the following graphs showing the variation of rate constant $(k)$ with temperature $(T)$ for a reaction,the one that exhibits Arrhenius behaviour over the entire temperature range is: