(C) The activation energy $(E_a)$ is determined using the Arrhenius equation at two different temperatures ($T_1$ and $T_2$).According to the Arrheniu

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Evaluating rate constants at two different temperatures

(C) The activation energy $(E_a)$ is determined using the Arrhenius equation at two different temperatures ($T_1$ and $T_2$).According to the Arrhenius equation: $\log \frac{K_2}{K_1} = \frac{E_a}{2.303R} \left[ \frac{T_2 - T_1}{T_1 T_2} \right]$.By measuring the rate constants ($K_1$ and $K_2$) at two different temperatures,the activation energy can be calculated.

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

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Activation energy of a chemical reaction can be determined by

AIPMT 1998 All AIPMT

A
Changing concentration of reactants
B
Evaluating rate constant at standard temperature
C
Evaluating rate constants at two different temperatures
D
Evaluating velocities of reaction at two different temperatures

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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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AIPMT 1998 Paper All AIPMT years →

For a reaction,the temperature increases from $10\,^\circ\text{C}$ to $50\,^\circ\text{C}$. The rate of the reaction will increase by a factor of ........

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For a reversible reaction $A \rightleftharpoons B$,which one of the following statements is wrong from the given energy profile diagram?

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Which of the following statements is correct for the activation energy of a reaction?

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If the rate of a reaction doubles when the temperature increases from $298 \, K$ to $308 \, K$,the activation energy of the reaction is ........... $kJ \, mol^{-1}$.

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All energetically effective collisions do not result in a chemical change. Explain with the help of an example.

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Activation energy of a chemical reaction can be determined by

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For a reaction,the temperature increases from $10\,^\circ\text{C}$ to $50\,^\circ\text{C}$. The rate of the reaction will increase by a factor of ........

For a reversible reaction $A \rightleftharpoons B$,which one of the following statements is wrong from the given energy profile diagram?

Which of the following statements is correct for the activation energy of a reaction?

If the rate of a reaction doubles when the temperature increases from $298 \, K$ to $308 \, K$,the activation energy of the reaction is ........... $kJ \, mol^{-1}$.

All energetically effective collisions do not result in a chemical change. Explain with the help of an example.

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