(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

Which scientist explained that all the species taking part in a reaction do not possess the same kinetic energy?

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For a hypothetical reaction $A \to B$,the activation energies for forward and backward reactions are $19 \ kJ/mol$ and $9 \ kJ/mol$ respectively. The heat of reaction is $.... \ kJ$.

MediumAIPMT 2000

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The relation between the rate constant and temperature according to the Arrhenius equation is:

Easy

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For a reaction,the activation energy $E_{a} = 0$ and the rate constant at $200 \ K$ is $1.6 \times 10^{6} \ s^{-1}$. The rate constant at $400 \ K$ will be (given $R = 8.314 \ J \ K^{-1} \ mol^{-1}$):

DifficultNEET 2019

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Define the following terms:
$1.$ Collision
$2.$ Frequency of collision

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

Similar Questions

Which scientist explained that all the species taking part in a reaction do not possess the same kinetic energy?

For a hypothetical reaction $A \to B$,the activation energies for forward and backward reactions are $19 \ kJ/mol$ and $9 \ kJ/mol$ respectively. The heat of reaction is $.... \ kJ$.

The relation between the rate constant and temperature according to the Arrhenius equation is:

For a reaction,the activation energy $E_{a} = 0$ and the rate constant at $200 \ K$ is $1.6 \times 10^{6} \ s^{-1}$. The rate constant at $400 \ K$ will be (given $R = 8.314 \ J \ K^{-1} \ mol^{-1}$):

Define the following terms:$1.$ Collision$2.$ Frequency of collision

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Define the following terms:
$1.$ Collision
$2.$ Frequency of collision