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

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Slope = $-\frac{E_a}{R}$,Intercept = $\ln A$

(A) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.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 $y = \ln k$,$x = \frac{1}{T}$,$m$ is the slope,and $c$ is the intercept:Slope $(m)$ = $-\frac{E_a}{R}$Intercept $(c)$ = $\ln A$.

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

Easy

In the plot of $\ln k$ versus $\frac{1}{T}$,what do the slope and intercept represent?

A
Slope = $-\frac{E_a}{R}$,Intercept = $\ln A$
B
Slope = $\frac{E_a}{R}$,Intercept = $\ln A$
C
Slope = $-\frac{E_a}{R}$,Intercept = $-\ln A$
D
Slope = $\frac{E_a}{R}$,Intercept = $-\ln A$

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

The decomposition of $N_2O$ into $N_2$ and $O_2$ in the presence of argon follows first-order kinetics. If the rate constant is given by $K = 5.0 \times 10^{11} \, e^{-2000/T}$,what is the activation energy of the reaction?

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For two reactions,the values of the pre-exponential factor are the same. However,the difference between their activation energy values is $24.9 \, kJ \, mol^{-1}$. The ratio of their rate constants at $300 \, K$ is ....

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Explain the effect of an increase in temperature on the rate of reaction and the rate constant.

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For a reaction,given below is the graph of $\ln k$ vs $\frac{1}{T}$. The activation energy for the reaction is equal to $...... \ cal \ mol^{-1}$. (Nearest integer). (Given : $R = 2 \ cal \ K^{-1} \ mol^{-1}$)

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Which graph shows zero activation energy?

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In the plot of $\ln k$ versus $\frac{1}{T}$,what do the slope and intercept represent?

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The decomposition of $N_2O$ into $N_2$ and $O_2$ in the presence of argon follows first-order kinetics. If the rate constant is given by $K = 5.0 \times 10^{11} \, e^{-2000/T}$,what is the activation energy of the reaction?

For two reactions,the values of the pre-exponential factor are the same. However,the difference between their activation energy values is $24.9 \, kJ \, mol^{-1}$. The ratio of their rate constants at $300 \, K$ is ....

Explain the effect of an increase in temperature on the rate of reaction and the rate constant.

For a reaction,given below is the graph of $\ln k$ vs $\frac{1}{T}$. The activation energy for the reaction is equal to $...... \ cal \ mol^{-1}$. (Nearest integer). (Given : $R = 2 \ cal \ K^{-1} \ mol^{-1}$)

Which graph shows zero activation energy?

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