At $T(\mathrm{~K})$ the following equation is obtained for a first order reaction $\log \frac{k}{A}=-\frac{x}{T}$. The activation energy for this reaction is equal to ( $R=$ gas constant)

Consider the reaction given below

$$ A+2 B \longrightarrow 3 C+2 D $$

If rate of disappearance of $B$ is $x \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$, the ratio of rate of reaction and rate of appearance of $C$ is

Activation energy for the hydrolysis of sucrose by acid is $X \mathrm{~kJ} \mathrm{~mol}^{-1}$ whereas activation energy for the hydrolysis of sucrose by sucrase is $Y \mathrm{~kJ} \mathrm{~mol}^{-1} . X$ and $Y$ respectively are

$A \rightarrow$ products, is a first order reaction. The following data is obtained for this reaction at $T(\mathrm{~K})$. The value of $x: y$ is

$$ \begin{array}{cc} \hline \text { Rate }\left(\mathrm{molL}^{-1} \mathrm{~min}^{-1}\right) & {[A]} \\ \hline 0.2 & 0.02 \mathrm{M} \\ \hline 0.4 & x \mathrm{M} \\ \hline 1.0 & y \mathrm{M} \\ \hline \end{array} $$