With respect to the equation, k = Ae^(-Ea/RT) in chemical kinetics, which one of the following statements is correct?

Options

A. R is Boltzmann constant
B. `E_a` is energy of activation
C. A is concentration of reactant molecule
D. k is equilibrium constant

Answer

To solve the question regarding the equation \( k = Ae^{-\frac{E_a}{RT}} \) in chemical kinetics, we need to analyze the components of the equation and the provided options.

### Step-by-Step Solution:

1. **Identify the Components of the Equation**:
- The equation \( k = Ae^{-\frac{E_a}{RT}} \) is known as the Arrhenius equation.
- Here, \( k \) represents the rate constant of a chemical reaction.
- \( A \) is known as the pre-exponential factor or frequency factor.
- \( E_a \) is the activation energy, which is the minimum energy required for a reaction to occur.
- \( R \) is the universal gas constant.
- \( T \) is the absolute temperature in Kelvin.

2. **Evaluate Each Option**:
- **Option 1**: "R is Boltzmann constant" - This is incorrect. \( R \) is the universal gas constant, not the Boltzmann constant.
- **Option 2**: "Ea is energy of activation" - This is correct. \( E_a \) indeed represents the activation energy.
- **Option 3**: "A is concentration of reactant molecules" - This is incorrect. \( A \) is the pre-exponential factor, not the concentration of reactants.
- **Option 4**: "k is equilibrium constant" - This is incorrect. \( k \) is the rate constant, not the equilibrium constant.

3. **Conclusion**:
- After evaluating all options, the only correct statement is **Option 2**: "Ea is energy of activation".

### Final Answer:
The correct statement is: **Ea is energy of activation**.

---