Which of the following plot represents the variation of $$\ln \mathrm{k}$$ versus $$\frac{1}{\mathrm{~T}}$$ in accordance with Arrhenius equation?

Rate constants of a reaction at $$500 \mathrm{~K}$$ and $$700 \mathrm{~K}$$ are $$0.04 \mathrm{~s}^{-1}$$ and $$0.14 \mathrm{~s}^{-1}$$, respectively; then, activation energy of the reaction is :

(Given: $$\log 3.5=0.5441, \mathrm{R}=8.31 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$$)

Activation energy of any chemical reaction can be calculated if one knows the value of

Which plot of $$\ln \mathrm{k}$$ vs $$\frac{1}{\mathrm{~T}}$$ is consistent with Arrhenius equation?