If both the volume and absolute temperature of a confined gas are doubled, what will happen to the pressure?

When considering the behavior of a confined gas, we can refer to the ideal gas law, which is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is the absolute temperature.

In this scenario, if both the volume and absolute temperature of the gas are doubled, we can analyze what happens to the pressure. By substituting the new values into the equation, we have:

• New volume (V'): 2V
• New temperature (T'): 2T

Substituting into the ideal gas law gives us:

P' (2V) = nR(2T)

From this equation, we can simplify it to determine the new pressure (P'). Thus, it becomes:

P' = (nRT) / (2V)

This shows that the new pressure is actually half of the original pressure because while the volume and temperature both increased, the increase in volume (which generally would decrease pressure) effectively countered the increase in temperature (which would generally increase pressure).

Therefore, when both the volume and the absolute temperature are doubled, the pressure remains unchanged because the effects of both physical changes offset