(D) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.As $T \to \infty$,the term $E_a / RT \to 0$.Therefore,$k = A e^0 = A \times 1 = A$.Thus,t

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The rate constant of a reaction becomes equal to the pre-exponential factor when the absolute temperature is infinity.

(D) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.As $T \to \infty$,the term $E_a / RT \to 0$.Therefore,$k = A e^0 = A \times 1 = A$.Thus,the rate constant $k$ becomes equal to the pre-exponential factor $A$ at infinite temperature.Molecularity is always a whole number (integer) and cannot be fractional or zero.Zero order reactions do stop when the reactant is completely consumed.First order reactions can be either homogeneous or heterogeneous.

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

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Which of the following statements is correct?

A
Molecularity of a reaction can be fractional.
B
Zero order reaction never stops.
C
$A$ first order reaction must be homogeneous.
D
The rate constant of a reaction becomes equal to the pre-exponential factor when the absolute temperature is infinity.

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

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Collision theory, Energy of activation and Arrhenius equation

The number of molecules with energy greater than the threshold energy for a reaction increases five-fold by a rise of temperature from $27^{\circ} C$ to $42^{\circ} C$. Its energy of activation in $J \ mol^{-1}$ is.............. (Take $\ln 5 = 1.6094$; $R = 8.314 \ J \ mol^{-1} K^{-1}$)

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The rate constant of a first order reaction was doubled when the temperature was increased from $300 \ K$ to $310 \ K$. What is its approximate activation energy (in $kJ \cdot mol^{-1}$)? ($R = 8.3 \ J \cdot mol^{-1} \cdot K^{-1}$; $\log 2 = 0.3$)

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Calculate the activation energy of a reaction,whose rate constant doubles on raising the temperature from $300 \ K$ to $600 \ K$.

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The rate constant $(k)$ of a reaction is measured at different temperatures $(T),$ and the data are plotted in the given figure. The activation energy of the reaction in $kJ\, mol^{-1}$ is :
($R$ is gas constant)

MediumJEE MAIN 2020

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According to the Arrhenius equation, in a graph of $\log k$ versus $\frac{1}{T}$, the slope will be . . . . . . .

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Which of the following statements is correct?

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The number of molecules with energy greater than the threshold energy for a reaction increases five-fold by a rise of temperature from $27^{\circ} C$ to $42^{\circ} C$. Its energy of activation in $J \ mol^{-1}$ is.............. (Take $\ln 5 = 1.6094$; $R = 8.314 \ J \ mol^{-1} K^{-1}$)

The rate constant of a first order reaction was doubled when the temperature was increased from $300 \ K$ to $310 \ K$. What is its approximate activation energy (in $kJ \cdot mol^{-1}$)? ($R = 8.3 \ J \cdot mol^{-1} \cdot K^{-1}$; $\log 2 = 0.3$)

Calculate the activation energy of a reaction,whose rate constant doubles on raising the temperature from $300 \ K$ to $600 \ K$.

The rate constant $(k)$ of a reaction is measured at different temperatures $(T),$ and the data are plotted in the given figure. The activation energy of the reaction in $kJ\, mol^{-1}$ is :($R$ is gas constant)

According to the Arrhenius equation, in a graph of $\log k$ versus $\frac{1}{T}$, the slope will be . . . . . . .

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The rate constant $(k)$ of a reaction is measured at different temperatures $(T),$ and the data are plotted in the given figure. The activation energy of the reaction in $kJ\, mol^{-1}$ is :
($R$ is gas constant)