(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 →

For the reaction $A + B \rightarrow C + D$,$\Delta H = -20 \ kJ \ mol^{-1}$. The activation energy for the forward reaction is $85 \ kJ \ mol^{-1}$. The activation energy for the reverse reaction is ......... $kJ \ mol^{-1}$.

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For an elementary chemical reaction, the Arrhenius plot is given below. If the energy of activation is $6.64 \ kJ \ mol^{-1}$ and $R = 8.3 \ J \ K^{-1} \ mol^{-1}$, the temperature at which the rate constant becomes $e^2 \ min^{-1}$, is (in $K$)

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When the temperature changes from $300 \ K$ to $310 \ K$,the rate of the reaction doubles. The activation energy of the reaction is ..... $kJ \ mol^{-1}$. $(R = 8.314 \ J \ K^{-1} \ mol^{-1} \text{ and } \log 2 = 0.301)$

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Oxygen is available in plenty in air,yet fuels do not burn by themselves at room temperature. Explain.

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The half-life of a first order reaction varies with temperature according to

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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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For the reaction $A + B \rightarrow C + D$,$\Delta H = -20 \ kJ \ mol^{-1}$. The activation energy for the forward reaction is $85 \ kJ \ mol^{-1}$. The activation energy for the reverse reaction is ......... $kJ \ mol^{-1}$.

For an elementary chemical reaction, the Arrhenius plot is given below. If the energy of activation is $6.64 \ kJ \ mol^{-1}$ and $R = 8.3 \ J \ K^{-1} \ mol^{-1}$, the temperature at which the rate constant becomes $e^2 \ min^{-1}$, is (in $K$)

When the temperature changes from $300 \ K$ to $310 \ K$,the rate of the reaction doubles. The activation energy of the reaction is ..... $kJ \ mol^{-1}$. $(R = 8.314 \ J \ K^{-1} \ mol^{-1} \text{ and } \log 2 = 0.301)$

Oxygen is available in plenty in air,yet fuels do not burn by themselves at room temperature. Explain.

The half-life of a first order reaction varies with temperature according to

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