Which of the following statements is correct?

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(C) According to the Arrhenius equation,$\ln K = \ln A - \frac{E_a}{RT}$,which can be written as $\log K = \log A - \frac{E_a}{2.303RT}$.Comparing thi

Vedclass · Accepted Answer

The graph of $\log K$ vs $\frac{1}{T}$ is a straight line with a slope of $-\frac{E_a}{2.303R}$.

Vedclass · Answer

(C) According to the Arrhenius equation,$\ln K = \ln A - \frac{E_a}{RT}$,which can be written as $\log K = \log A - \frac{E_a}{2.303RT}$.Comparing this with the equation of a straight line $y = mx + c$,we get the slope $m = -\frac{E_a}{2.303R}$.Therefore,the graph of $\log K$ vs $\frac{1}{T}$ is a straight line with a slope of $-\frac{E_a}{2.303R}$.Option $A$ is incorrect because the temperature coefficient depends on $E_a$,but the relationship is not simply 'larger $E_a$ means higher coefficient'.Option $B$ is incorrect because $K$ increases more significantly at lower temperatures for a given $\Delta T$.Option $D$ is incorrect because the rate of reaction also depends on the frequency factor $A$ and the concentration of reactants,not just $E_a$.

Step	Rate constant and Activation energy
$Step \ 1$	$k_1, E_{a_1} = 180 \ kJ \ mol^{-1}$
$Step \ 2$	$k_2, E_{a_2} = 80 \ kJ \ mol^{-1}$
$Step \ 3$	$k_3, E_{a_3} = 50 \ kJ \ mol^{-1}$

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