In respect of the equation `k=Ae^(-E_(a)//RT)` in chemical kinetics, which one of the following statement is correct

Options

A. k is equilibrium constant
B. A is adsorption factor
C. `E_(a)` is energy of activation
D. R is Rydberg’s constant

Explanation

To solve the question regarding the equation \( k = A e^{-\frac{E_a}{RT}} \) in chemical kinetics, we need to analyze the components of the equation and determine which statement is correct.

### Step-by-Step Solution:

1. **Identify the components of the equation**:
- \( k \): This represents the rate constant of a reaction.
- \( A \): This is known as the pre-exponential factor or frequency factor.
- \( E_a \): This is the activation energy, which is the minimum energy required for a reaction to occur.
- \( R \): This is the universal gas constant.
- \( T \): This is the temperature in Kelvin.

2. **Understand the context of the equation**:
- The equation \( k = A e^{-\frac{E_a}{RT}} \) is known as the Arrhenius equation. It describes how the rate constant \( k \) of a reaction depends on temperature and activation energy.

3. **Analyze the statements**:
- If one of the statements claims that \( k \) is the equilibrium constant, this is incorrect. \( k \) refers to the rate constant, not the equilibrium constant.
- If another statement claims that \( A \) is the adsorption factor, this is also incorrect. \( A \) is the pre-exponential factor.
- A statement that correctly identifies \( E_a \) as the activation energy is accurate.
- Lastly, if a statement claims that \( R \) is the red word constant, this is incorrect. \( R \) is the universal gas constant.

4. **Conclusion**:
- The correct statement among the options provided is that \( E_a \) is the activation energy.

### Final Answer:
The correct statement is that \( E_a \) is the activation energy.

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