(A) The temperature coefficient $\mu$ is defined as the ratio of rate constants at temperatures $(T + 10) \ K$ and $T \ K$.From the Arrhenius equation

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(A) The temperature coefficient $\mu$ is defined as the ratio of rate constants at temperatures $(T + 10) \ K$ and $T \ K$.From the Arrhenius equation,$k = Ae^{-E_a / RT}$,it can be derived that $\log \mu \propto E_a$.This implies that the temperature coefficient $\mu$ increases as the activation energy $E_a$ increases.Given $E_{a_1} > E_{a_2}$,it follows that $\mu_1 > \mu_2$.

Class 12 Chemistry Chemical Kinetics Collision theory, Energy of activation and Arrhenius equation

Medium

If for two reactions $E_{a_1} > E_{a_2}$ and $\mu_1$ and $\mu_2$ are their respective temperature coefficients,then which of the following is correct?

A
$\mu_1 > \mu_2$
B
$\mu_1 < \mu_2$
C
$\mu_1 = \mu_2$
D
$\text{None of these}$

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Collision theory, Energy of activation and Arrhenius equation

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If for two reactions $E_{a_1} > E_{a_2}$ and $\mu_1$ and $\mu_2$ are their respective temperature coefficients,then which of the following is correct?

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For $N_2 + 3H_2 \rightarrow 2NH_3$,$\Delta H = -22 \ kcal$,and $E_a = 70 \ kcal$. Hence $E_a$ for $2NH_3 \rightarrow N_2 + 3H_2$ is $.....$ $kcal$.

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