In the given graph,$E_{a}$ for the reverse reaction will be (in $kJ$)

For a certain reaction,consider the plot of $\ln k$ versus $1/T$ given in the figure. If the rate constant of this reaction at $400 \ K$ is $10^{-5} \ s^{-1}$,then the rate constant at $500 \ K$ is:

The activation energy for a simple chemical reaction $A \to B$ is ${E_a}$ in the forward direction. The activation energy for the reverse reaction:

Define the following terms:
$(1)$ Fraction of molecules
$(2)$ Frequency factor

The minimum energy that reactant molecules must possess at the time of collision for an effective collision is called ...

At a constant temperature,the activation energy of a reaction is found to be $2.303 \, RT \, J \, mol^{-1}$. The ratio of the rate constant to the Arrhenius constant will be $......$.