The rate constants for decomposition of acetaldehyde have been measured over the temperature range $700-1000 \mathrm{K}$. The data has been analysed by plotting $\mathrm{lnk}$ vs $\frac{{10}^3}{ \mathrm{T}}$ graph. The value of activation energy for the reaction is ${\mathrm{kJmol}}^{-1}$. (Nearest integer) (Given : $\mathrm{R}=8.31 \mathrm{J}{\mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$)

The rate constant for a first order reaction is given by the following equation :

$\mathrm{lnk}=33.24-\frac{2.0\times {10}^4 \mathrm{K}}{ \mathrm{T}}$

The Activation energy for the reaction is given by ${\mathrm{kJmol}}^{-1}$. (In Nearest integer) (Given : $\mathrm{R}=8.3 \mathrm{J}{ \mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$)

$\begin{array}{ccc}\left[\mathrm{A}\right]& \to & \left[\mathrm{B}\right]\\ \mathrm{Reactant}& & \mathrm{Product}\end{array}$

If formation of compound $\left[\mathrm{B}\right]$ follows the first order of kinetics and after $70$ minutes the concentration of $\left[\mathrm{A}\right]$ was found to be half of its initial concentration. Then the rate constant of the reaction is $\mathrm{x}\times {10}^{-6}{ \mathrm{s}}^{-1}$. The value of $\mathrm{x}$ is____

For a reaction, given below is the graph of $\mathrm{lnk} \mathrm{vs}\frac{1}{ \mathrm{T}}$. The activation energy for the reaction is equal to____$\mathrm{cal} {\mathrm{mol}}^{-1}$.(Given : $\mathrm{R}=2{\mathrm{calK}}^{-1}{ \mathrm{mol}}^{-1}$)

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The reaction between $\mathrm{X}$ and $\mathrm{Y}$ is first order with respect to $\mathrm{X}$ and zero order with respect to $\mathrm{Y}$.

Examine the data of table and calculate ratio of numerical values of $\mathrm{M}$ and $\mathrm{L}$.