For a reaction,the temperature increases from $10\,^\circ\text{C}$ to $50\,^\circ\text{C}$. The rate of the reaction will increase by a factor of ........

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 .......... $\text{kcal} / \text{mol}$ $(\ln \, 2 = 0.7)$

Plots showing the variation of the rate constant $k$ with temperature $T$ are given below. The plot that follows Arrhenius equation is

According to the Arrhenius equation, which of the following statements is correct?

The activation energy for the reaction $X \rightarrow Y$ is $150 \text{ kJ mol}^{-1}$. The change in enthalpy for the above reaction is $-135 \text{ kJ mol}^{-1}$. What is the activation energy for the reverse reaction $Y \rightarrow X$?

For a certain gaseous reaction,the temperature is increased by $10\,^{\circ}C$ from $25\,^{\circ}C$ to $35\,^{\circ}C$. If the rate of the reaction doubles,what will be the value of the activation energy $(E_a)$?