On increasing the temperature by `10^(@)C`,

Options

A. number of collisions get doubled
B. value of rate constant does not change
C. energy of activation increases
D. pecific rate of the reaction gets doubled

Explanation

**Step-by-Step Solution:**

1. **Understanding the Effect of Temperature on Reaction Rate:**
- The rate of a chemical reaction is influenced by temperature. As the temperature increases, the kinetic energy of the molecules also increases, leading to more frequent and effective collisions between reactant molecules.

2. **Temperature Coefficient (μ):**
- The temperature coefficient (μ) is a measure of how much the rate of a reaction changes with a change in temperature. It is commonly observed that for many reactions, the rate approximately doubles with every 10°C increase in temperature.

3. **Mathematical Representation:**
- If we denote the rate constant at temperature \( T \) as \( k_T \), then the rate constant at \( T + 10°C \) can be represented as:
\[ k_{T + 10} \approx 2 \cdot k_T \]
- This indicates that the rate constant (and thus the reaction rate) doubles when the temperature is increased by 10°C.

4. **Graphical Representation:**
- A graphical representation can help visualize this effect. On a graph where the x-axis represents temperature and the y-axis represents the percentage of molecules with sufficient kinetic energy, we can see that at a higher temperature (e.g., 30°C compared to 20°C), a greater percentage of molecules have the energy required to overcome the activation energy barrier for the reaction.

5. **Conclusion:**
- Therefore, when the temperature is increased by 10°C, the rate of the reaction approximately doubles, which is a significant increase in the reaction rate.