Introduction
When the number of molecules in a container is doubled but the kinetic energy remains the same, it affects the absolute temperature of the gas. In this explanation, we will explore how the absolute temperature changes in such a scenario.

Understanding the Concept
To understand this scenario, it is important to have a clear understanding of the relationship between temperature, kinetic energy, and the number of molecules.

Temperature and Kinetic Energy
The temperature of a gas is directly related to the average kinetic energy of its molecules. According to the kinetic theory of gases, the average kinetic energy of a gas is proportional to its absolute temperature. This means that as the temperature increases, so does the average kinetic energy of the gas molecules.

Number of Molecules and Kinetic Energy
The total kinetic energy of a gas is directly proportional to the number of molecules present. When the number of molecules in a gas is doubled while the total kinetic energy remains the same, it means that each molecule must have half the kinetic energy compared to the previous scenario. This is because the total kinetic energy is distributed among a larger number of molecules.

Understanding the Relationship
To understand how the absolute temperature changes in this scenario, we need to consider the relationship between temperature, kinetic energy, and the number of molecules.

Relationship between Temperature, Kinetic Energy, and Number of Molecules
The relationship between temperature, kinetic energy, and the number of molecules can be expressed using the equation:

Temperature ∝ (Kinetic Energy / Number of Molecules)

Explanation
In the given scenario, the number of molecules is doubled while the kinetic energy remains the same. This means that the numerator of the equation (Kinetic Energy) remains constant, while the denominator (Number of Molecules) is doubled.

Effect on Absolute Temperature
As the number of molecules doubles while the kinetic energy remains constant, the denominator of the equation doubles. According to the relationship between temperature, kinetic energy, and the number of molecules, this would cause the absolute temperature to decrease by half. Therefore, the absolute temperature of the gas would be halved in this scenario.

Conclusion
When the number of molecules in a container is doubled while the kinetic energy remains the same, the absolute temperature of the gas is halved. This is because the total kinetic energy is distributed among a larger number of molecules, resulting in each molecule having half the kinetic energy compared to the previous scenario.