For a first order reaction,the rate constant is $0.04 \, \text{min}^{-1}$ at $27 \, ^\circ\text{C}$ and $0.08 \, \text{min}^{-1}$ at $37 \, ^\circ\text{C}.$ The activation energy of reaction is .......... $\text{kcal} / \text{mol}$ $(\ln \, 2 = 0.7)$

For a chemical reaction at $27^{\circ} C$, the activation energy is $600 R$. The ratio of the rate constants at $327^{\circ} C$ to that of at $27^{\circ} C$ will be

For a first order chemical reaction,

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:

The velocity constant of a reaction at $290 \ K$ was found to be $3.2 \times 10^{-3}$. At $310 \ K$,it will be about:

On introducing a catalyst at $500 \, K,$ the rate constant of a first order reaction increases $2.718$ times. If the activation energy in the presence of a catalyst is $4.15 \, kJ \, mol^{-1},$ then what will be $E_a$ in the absence of a catalyst? (Value of $e = 2.718$ and $R = 8.314 \times 10^{-3} \, kJ \, K^{-1} \, mol^{-1}$)