Graph plotted between $\log {\mathrm{t}}_{1/2}$ versus log concentration $\left(\mathrm{a}\right)$ is a straight line. What conclusion can you draw from the graph?

$\mathrm{n}=$ order of reaction

Consider the following reaction

$\mathrm{A} \underset{{\mathrm{k}}_{-1}}{\overset{{\mathrm{k}}_1}{\rightleftharpoons }} \mathrm{M}+\mathrm{C} ; \mathrm{M}+\mathrm{B} \stackrel{{\mathrm{k}}_2}{\to } \mathrm{Products} (\mathrm{Slow} \mathrm{step})$

The rate can be expressed as

If ${\mathrm{E}}_{\mathrm{a}} =30 \mathrm{kcal} {\mathrm{mol}}^{-1}$, what is the effect on rate constant of a reaction for $10°\mathrm{C}$ rise in temperature?

It will increase

For gaseous reaction, the following data is given $\mathrm{A}\to \mathrm{B}, {\mathrm{k}}_1={10}^{15}{\mathrm{e}}^{-2000/\mathrm{T}}$

$\mathrm{C}\to \mathrm{D}, {\mathrm{k}}_2={10}^{14}{\mathrm{e}}^{-1000/\mathrm{T}}$

 The temperature at which ${\mathrm{k}}_1={\mathrm{k}}_2$ is