Question

Increasing the temperature of a gas filled in a container would lead to:
A. Increase in its mass
B. Increase in its kinetic energy
C. Decrease in pressure
D. Decrease in intermolecular distance

Answer 1

When we increase the temperature of a gas then the motion of the molecules of a gas increase which means that the energy carried by the molecules increases. By using this knowledge and its relation to thermodynamic quantities, we can obtain the required answer.

Complete step by step answer:
According to the kinetic theory of gases, the kinetic energy of a gas is directly related to the temperature of a gas. When the temperature of a gas is increased then the vibrations or motion of the gas molecules increases, as a result, the kinetic energy carried by the molecules of the gas increases. Mathematically, for a gas, the kinetic energy of the gas molecules is related to the temperature of the gas by the following relation.
$K.E. = \dfrac{1}{2}{K_B}T$
Here T is the temperature of the gas while ${K_B}$ is known as the Boltzmann constant. Its value is given as
${K_B} = 1.38 \times {10^{ - 23}}J{K^{ - 1}}$
So, based on the above discussion, increasing the temperature of a gas filled in a container would lead to increase in its kinetic energy.

So, the correct answer is “Option B”.

Note:
1. It should be noted that the pressure of a gas increases with the increase in the temperature of the gas because with increase in kinetic energy, the force with which molecules strike the wall increases, hence, pressure increases.
2. With increase in temperature of a gas, the intermolecular distance will increase because with increase in energy of particles, they hit each other with greater force and force each other away from each other.
3. The mass of a gas is fixed if the volume of the gas is fixed and it will remain unaffected by the change in temperature of the gas.