$A$ reaction having equal activation energies for forward and reverse reaction has:

For the reaction $A \rightleftharpoons B$,if $E_a$ is the activation energy of the forward reaction,then the activation energy of the backward reaction is:

For an endothermic reaction,$\Delta H$ represents the enthalpy of the reaction in $kJ \ mol^{-1}$. The minimum amount of activation energy will be

Assertion : According to transition state theory for the formation of an activated complex,one of the vibrational degrees of freedom is converted into a translational degree of freedom.
Reason : Energy of the activated complex is higher than the energy of reactant molecules.

The energy profile diagram for a multi-step reaction,$A$ $\xrightarrow{1} B$ $\xrightarrow{2} C$ $\xrightarrow{3} D,$ is given below. The rate-determining step of the reaction is:

For a particular reaction,the rate constant becomes double on increasing temperature from $27^{\circ} C$ to $37^{\circ} C$. Calculate the approximate activation energy (in $kcal \ mol^{-1}$,$R=2 \ cal \ mol^{-1} \ K^{-1}$).