In a chemical reaction, rate of a chemical reaction increases with temperature. The reason is due to

Options

A. number of collisions between molecules increases
B. decreases in activation energy
C. increase in the number of the molecules with activation energy
D. kinetic energy of reactants increases

Explanation

To understand why the rate of a chemical reaction increases with temperature, we can break down the explanation into several key steps:

### Step-by-Step Solution:

1. **Understanding Kinetic Energy and Temperature**:
- Temperature is a measure of the average kinetic energy of the molecules in a substance. As temperature increases, the average kinetic energy of the molecules also increases.

2. **Effect of Temperature on Molecular Motion**:
- With an increase in temperature, molecules move faster. This increased motion leads to more frequent collisions between the reacting molecules.

3. **Collision Theory**:
- According to collision theory, for a reaction to occur, reactant molecules must collide with sufficient energy and proper orientation. The frequency of these effective collisions increases with temperature.

4. **Activation Energy**:
- Activation energy is the minimum energy required for a chemical reaction to occur. At higher temperatures, a greater proportion of the molecules have kinetic energy that exceeds this activation energy.

5. **Increase in Effective Collisions**:
- As more molecules have energy greater than the activation energy, the number of effective collisions increases. This means that more collisions will lead to product formation.

6. **Conclusion**:
- Therefore, the rate of the chemical reaction increases with temperature due to an increase in the number of molecules with energy equal to or greater than the activation energy, leading to more effective collisions.

### Final Answer:
The rate of a chemical reaction increases with temperature due to an increase in the number of molecules with activation energy, resulting in more effective collisions.