Which one of the following given graphs represents the variation of rate constant $\left(\mathrm{k}\right)$ with temperature $\left(\mathrm{T}\right)$ for an endothermic reaction?

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 : $\mathrm{R}=8.31 \mathrm{J}{\mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$)

For a first order reaction, the time required for completion of $90\%$ reaction is '$\mathrm{x}$' times the half life of the reaction. The value of '$\mathrm{x}$' is

(Given: $\ln 10=2.303$ and $\log 2=0.3010$)

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 : $\mathrm{R}=8.3 \mathrm{J}{ \mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$)