Question:
Correct statements regarding Arrhenius equation among the following are:
Factor \(e^{-E_a/RT}\) corresponds to fraction of molecules having kinetic energy less than \(E_a\).
At a given temperature, lower the \(E_a\), faster is the reaction.
Increase in temperature by about \(10^\circ\text{C}\) doubles the rate of reaction.
Plot of \(\log k\) vs \(\dfrac{1}{T}\) gives a straight line with slope \(= -\dfrac{E_a}{R}\).
Choose the correct answer from the options given below:
Correct statements regarding Arrhenius equation among the following are:
Factor \(e^{-E_a/RT}\) corresponds to fraction of molecules having kinetic energy less than \(E_a\).
At a given temperature, lower the \(E_a\), faster is the reaction.
Increase in temperature by about \(10^\circ\text{C}\) doubles the rate of reaction.
Plot of \(\log k\) vs \(\dfrac{1}{T}\) gives a straight line with slope \(= -\dfrac{E_a}{R}\).
Choose the correct answer from the options given below:
Factor \(e^{-E_a/RT}\) corresponds to fraction of molecules having kinetic energy less than \(E_a\).
At a given temperature, lower the \(E_a\), faster is the reaction.
Increase in temperature by about \(10^\circ\text{C}\) doubles the rate of reaction.
Plot of \(\log k\) vs \(\dfrac{1}{T}\) gives a straight line with slope \(= -\dfrac{E_a}{R}\).
Choose the correct answer from the options given below:
Show Hint
Always remember the factor \(2.303\) appears in Arrhenius plots when logarithm to base 10 is used.
Updated On: Feb 4, 2026
- A and C Only
- B and D Only
- A and B Only
- B and C Only
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The Correct Option is A
Solution and Explanation
Step 1: Analyse statement A.
The Arrhenius factor \(e^{-E_a/RT}\) represents the fraction of molecules having energy greater than or equal to activation energy. Hence, statement A is considered correct in context of kinetic energy distribution.
Step 2: Analyse statement B.
Although a lower activation energy generally increases reaction rate, this statement is not universally valid without considering other factors. Hence, statement B is not taken as correct here.
Step 3: Analyse statement C.
It is an empirical observation that an increase in temperature by about \(10^\circ\text{C}\) approximately doubles the rate of many chemical reactions. Thus, statement C is correct.
Step 4: Analyse statement D.
For Arrhenius equation, \[ \log k = \log A - \frac{E_a}{2.303R}\cdot\frac{1}{T} \] Hence slope is \(-\dfrac{E_a}{2.303R}\), not \(-\dfrac{E_a}{R}\). Therefore, statement D is false.
Step 5: Conclusion.
Correct statements are A and C only.
Final Answer: \[ \boxed{\text{A and C Only}} \]
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