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

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

(C) The Arrhenius equation is given by $k = A e^{-\frac{E_a}{RT}}$.Taking the natural logarithm on both sides,we get $\ln k = \ln A - \frac{E_a}{RT}$.Comparing this with the equation of a straight line $y = mx + c$,where $y = \ln k$ and $x = \frac{1}{T}$,the slope $m = -\frac{E_a}{R}$.Option $C$ is correct because the slope of the plot of $\ln k$ versus $\frac{1}{T}$ is $-\frac{E_a}{R}$.Note: If the plot is $\log_{10} k$ versus $\frac{1}{T}$,the slope is $-\frac{E_a}{2.303R}$.

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

Medium

Which of the following statements is correct regarding the Arrhenius equation and reaction kinetics?

A
Larger the activation energy,higher will be the value of temperature coefficient of reaction.
B
With an increase in temperature,in the high-temperature range,the rate constant increases more as compared to the low-temperature range.
C
The graph of $\ln k$ vs $\frac{1}{T}$ is a straight line with a slope of $-\frac{E_a}{R}$.
D
Chemical reactions with low activation energy always occur at a faster rate compared to reactions with higher activation energy.

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Class 12 Questions

Class 12

Chemistry Questions

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

When the temperature of a reaction is increased from $300 \ K$ to $310 \ K$,the rate of the reaction increases by $2.5$ times. If the rate constant of the reaction at $300 \ K$ is $K$,what will be the rate constant at $310 \ K$?

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The activation energy of a first-order reaction at $25\,^{\circ}C$ is $30\,kJ/mol$. In the presence of a catalyst,the activation energy of the same reaction at $25\,^{\circ}C$ becomes $24\,kJ/mol$. The rate of the reaction in the presence of the catalyst will be how many times the original rate?

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What happens to the most probable kinetic energy and the energy of activation with an increase in temperature?

Difficult

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Which of the following graphs of $\log \, K \rightarrow 1/T$ can be used to calculate the activation energy?

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The activation energy for the reaction $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$ is $209.5 \ kJ \ mol^{-1}$ at $581 \ K$. Calculate the fraction of molecules of reactants having energy equal to or greater than activation energy?

Difficult

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Which of the following statements is correct regarding the Arrhenius equation and reaction kinetics?

Similar Questions

When the temperature of a reaction is increased from $300 \ K$ to $310 \ K$,the rate of the reaction increases by $2.5$ times. If the rate constant of the reaction at $300 \ K$ is $K$,what will be the rate constant at $310 \ K$?

The activation energy of a first-order reaction at $25\,^{\circ}C$ is $30\,kJ/mol$. In the presence of a catalyst,the activation energy of the same reaction at $25\,^{\circ}C$ becomes $24\,kJ/mol$. The rate of the reaction in the presence of the catalyst will be how many times the original rate?

What happens to the most probable kinetic energy and the energy of activation with an increase in temperature?

Which of the following graphs of $\log \, K \rightarrow 1/T$ can be used to calculate the activation energy?

The activation energy for the reaction $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$ is $209.5 \ kJ \ mol^{-1}$ at $581 \ K$. Calculate the fraction of molecules of reactants having energy equal to or greater than activation energy?

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