Question

Which of the following statement is incorrect about activation energy? Higher the activation energy slower is the rate of reaction.

• A. Higher the activation energy slower is the rate of reaction.
• B. Catalyst decreases the activation energy.
• C. SI unit of activation energy is J/mol/K.
• D. Activation energy depends upon the rate of reaction.

Hint:

Remember that the SI unit for activation energy is \text{J/mol}, and not \text{J/mol/K}. The temperature dependence of the reaction rate is described by the Arrhenius equation.

Answer 1

The Correct Option is C

Activation energy is the minimum energy required for a reaction to occur. The rate of reaction is inversely proportional to the activation energy. - Option (A) is true because higher activation energy does indeed slow down the reaction rate.
- Option (B) is true since catalysts lower the activation energy required for a reaction to proceed.
- Option (C) is incorrect. The SI unit for activation energy is J/mol, not J/mol/K.
- Option (D) is true because activation energy is a property of the reaction itself, not directly related to the rate. Thus, the incorrect statement is option C.