(B) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.As $T \to \infty$,the term $\frac{E_a}{RT} \to 0$.Therefore,the rate constant $k$ approac

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(B) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.As $T \to \infty$,the term $\frac{E_a}{RT} \to 0$.Therefore,the rate constant $k$ approaches the pre-exponential factor $A$ (Arrhenius parameter).Given that the Arrhenius parameter $A = 6.0 \times 10^{14}\,s^{-1}$,the value of the rate constant as $T \to \infty$ is $6.0 \times 10^{14}\,s^{-1}$.

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

The rate constant,the activation energy and the Arrhenius parameter of a chemical reaction at $25\,^oC$ are $3.0 \times 10^{-4}\,s^{-1}$,$104.4\,kJ\,mol^{-1}$ and $6.0 \times 10^{14}\,s^{-1}$ respectively. The value of the rate constant as $T \to \infty$ is

IIT 1996 All IIT

A
$2.0 \times 10^{18}\,s^{-1}$
B
$6.0 \times 10^{14}\,s^{-1}$
C
Infinity
D
$3.6 \times 10^{30}\,s^{-1}$

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Class 12

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Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

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IIT 1996 Paper All IIT years →

$A$ chemical reaction was carried out at $300 \, K$ and $280 \, K$. The rate constants were found to be $K_1$ and $K_2$ respectively. The energy of activation is $1.157 \times 10^4 \, cal \, mol^{-1}$ and $R = 1.987 \, cal \, K^{-1} \, mol^{-1}$. Then:

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Fill in the blank :
$1.$ In collision theory the molecules are hard .........
$2.$ In a reality the molecules are hard ..........
$3.$ Collision take place with .......... species.

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Consider the following energy profile for the reaction $X + Y \rightarrow R + S$. Which of the following deductions about the reaction is not correct?

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The plot of $\log K$ vs $\frac{1}{T}$ helps to calculate

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What is the slope of the straight line for the graph drawn between $\ln k$ and $\frac{1}{T}$,where $k$ is the rate constant of a reaction at temperature $T$?

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The rate constant,the activation energy and the Arrhenius parameter of a chemical reaction at $25\,^oC$ are $3.0 \times 10^{-4}\,s^{-1}$,$104.4\,kJ\,mol^{-1}$ and $6.0 \times 10^{14}\,s^{-1}$ respectively. The value of the rate constant as $T \to \infty$ is

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$A$ chemical reaction was carried out at $300 \, K$ and $280 \, K$. The rate constants were found to be $K_1$ and $K_2$ respectively. The energy of activation is $1.157 \times 10^4 \, cal \, mol^{-1}$ and $R = 1.987 \, cal \, K^{-1} \, mol^{-1}$. Then:

Fill in the blank :$1.$ In collision theory the molecules are hard .........$2.$ In a reality the molecules are hard ..........$3.$ Collision take place with .......... species.

Consider the following energy profile for the reaction $X + Y \rightarrow R + S$. Which of the following deductions about the reaction is not correct?

The plot of $\log K$ vs $\frac{1}{T}$ helps to calculate

What is the slope of the straight line for the graph drawn between $\ln k$ and $\frac{1}{T}$,where $k$ is the rate constant of a reaction at temperature $T$?

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Fill in the blank :
$1.$ In collision theory the molecules are hard .........
$2.$ In a reality the molecules are hard ..........
$3.$ Collision take place with .......... species.