As the temperature increases, average kinetic energy of molecules increases. What would be the effect of increase of temperature on pressure provided the volume is constant ?

Options

A. Increases
B. Decreases
C. Remains same
D. Becomes half

Explanation

To solve the question regarding the effect of temperature on pressure when the volume is constant, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Relationship**: We need to establish the relationship between temperature and pressure when the volume is constant. This is described by Gay-Lussac's Law.

2. **State Gay-Lussac's Law**: Gay-Lussac's Law states that for a given mass of gas at constant volume, the pressure of the gas is directly proportional to its absolute temperature. Mathematically, this can be expressed as:
\[ P \propto T \]
or
\[ \frac{P_1}{T_1} = \frac{P_2}{T_2} \]
where \(P\) is pressure and \(T\) is temperature in Kelvin.

3. **Analyze the Effect of Temperature Increase**: If the temperature of the gas increases (while keeping the volume constant), the average kinetic energy of the gas molecules also increases. This increase in kinetic energy leads to more frequent and forceful collisions of the gas molecules with the walls of the container.

4. **Conclude the Effect on Pressure**: As a result of these more frequent and forceful collisions, the pressure exerted by the gas on the walls of the container will increase.

5. **Final Answer**: Therefore, when the temperature increases at constant volume, the pressure also increases.

### Summary of the Solution:
- As temperature increases, the average kinetic energy of molecules increases.
- According to Gay-Lussac's Law, pressure is directly proportional to temperature at constant volume.
- Hence, an increase in temperature results in an increase in pressure.