Which of the following plots is in accordance | vedclass

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(A) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.Taking the logarithm on both sides,we get $\ln k = \ln A - \frac{E_a}{RT}$.Converting to

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(A) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.Taking the logarithm on both sides,we get $\ln k = \ln A - \frac{E_a}{RT}$.Converting to base $10$,we have $\log k = \log A - \frac{E_a}{2.303 R} 	imes \frac{1}{T}$.Comparing this with the equation of a straight line $y = mx + c$,where $y = \log k$,$x = \frac{1}{T}$,$m = -\frac{E_a}{2.303 R}$,and $c = \log A$.Therefore,a plot of $\log k$ versus $\frac{1}{T}$ yields a straight line with a negative slope of $-\frac{E_a}{2.303 R}$.

Which of the following plots is in accordance with the Arrhenius equation?

Similar Questions

At what temperature does the rate become double that at $300 \, K$ (in $, K$)? Given $\ln k = 10 - \frac{69 \, kJ}{RT}$.

What is the slope of the graph between $\ln K$ and $\frac{1}{T}$ according to the Arrhenius equation?

Choose the incorrect statement -

The temperature-dependent equation for the rate constant is written as:

The rate constant for a reaction can be increased by $\underline{a}$ the stability of the reactant or by $\underline{b}$ the stability of the transition state. Select the correct choice for $a$ and $b$.

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