Suppose you have a fixed amount of an ideal gas at a constant volume. If the pressure of the gas is doubled while the volume is held constant, what happens to its temperature? [Section 10.4]

Understanding the pressure-volume relationship in gases is essential to grasp the behavior of gases under various conditions. This relationship is commonly described by Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when the temperature and the amount of gas remain constant.

In mathematical terms, Boyle's Law can be expressed as: \[ P \times V = \text{constant} \] This means that if the volume of a gas is decreased, the pressure increases, assuming no change in the gas's temperature or the amount (moles) of gas. Conversely, if the volume is increased, the pressure decreases. This is crucial in understanding how pressure changes when we manipulate the volume of a gas within a closed system. Boyle's Law is a stepping stone towards understanding more complex gas behaviors described by the ideal gas law.

Temperature changes in gases are intimately linked with their pressure and volume changes, a concept incorporated in Charles's Law and Gay-Lussac's Law. Charles's Law states that the volume of a gas is directly proportional to its temperature when the pressure is kept constant. Gay-Lussac's Law, on the other hand, states that the pressure of a gas is directly proportional to its temperature when the volume is kept constant.

These laws imply that if you were to heat a gas, expecting its volume to remain unchanged, the gas's pressure must increase to accommodate the increased kinetic energy of the particles. This is exactly the scenario presented in the textbook exercise above. By doubling the pressure while maintaining constant volume, you are indirectly deducing that the temperature must also have doubled to maintain the equilibrium described by the ideal gas law, as long as the amount of the gas remains unchanged.

The ideal gas constant, denoted as 'R', is a fundamental parameter in the ideal gas law equation. It serves as a bridge linking pressure, volume, temperature, and the amount of a gas in moles. The value of R is the same for all gases, which is why it is termed a 'constant.'

Expressed in different units depending on the given pressure and volume units, the most common value used is approximately \(8.314 \text{J/(mol K)}\). The ideal gas constant helps to quantify the behavior of an ideal gas, allowing scientists and engineers to make predictions about the behavior of gases under different conditions. It is crucial to note that the ideal gas constant has different values depending on the units used for pressure, volume, and temperature. Ensuring that these units are consistent with those of 'R' is key to correctly using the ideal gas law and avoiding errors in calculations.