In arrhenius equation, the fraction of effective collisions is given by

Options

A. `K = Ae^((-Ea)/(RT))`
B. A
C. `e^((-Ea)/(RT))`
D. RT

Answer

To solve the question regarding the fraction of effective collisions in the Arrhenius equation, we will break it down step by step.

### Step-by-Step Solution:

1. **Understand the Arrhenius Equation**:
The Arrhenius equation is given by:
\[ k = A \cdot e^{-\frac{E_a}{RT}} \]
where:
- \( k \) is the rate constant,
- \( A \) is the pre-exponential factor (also known as the frequency factor),
- \( E_a \) is the activation energy,
- \( R \) is the gas constant,
- \( T \) is the temperature in Kelvin.

2. **Identify the Components**:
- The term \( A \) represents the frequency of collisions between reactant molecules.
- The term \( e^{-\frac{E_a}{RT}} \) represents the fraction of molecules that have enough energy to overcome the activation energy barrier.

3. **Fraction of Effective Collisions**:
The fraction of effective collisions is determined by the exponential term:
\[ \text{Fraction of effective collisions} = e^{-\frac{E_a}{RT}} \]
This term indicates the proportion of molecules that possess sufficient energy to react when they collide.

4. **Conclusion**:
Therefore, the fraction of effective collisions in the Arrhenius equation is given by the term \( e^{-\frac{E_a}{RT}} \).

### Final Answer:
The fraction of effective collisions in the Arrhenius equation is \( e^{-\frac{E_a}{RT}} \).

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