The absolute temperature of a gas is increased four times while maintaining a constant volume. what happens to the pressure of the gas?

Explanation:

The expression that rules the change of temperature of ideal gases at constant volume is the Law of Gay-Lussac: pressure and temperature of gases are directly related. In the form of equations that is:

The question states that the absolute temperature is increased four times, the you can write that as T₂ = 4 × T₁, and substitute in the equation 1 to obtain:

Simplify:

That proves that the pressure also increases four times, when the absolute temperature is increased four times, while maintaining the volume constant.

The pressure will also increase 4 times.

Explanation:

To calculate the final temperature of the system, we use the equation given by Gay-Lussac Law. This law states that pressure of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

where,

are the initial pressure and temperature of the gas.

are the final pressure and temperature of the gas.

We are given:

Putting values in above equation, we get:

Hence, the pressure will also increase 4 times.

it is a good conductor

explanation: