In general, how does increasing temperature affect the pressure of a fixed amount of refrigerant vapor in a sealed cylinder?

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Multiple Choice

In general, how does increasing temperature affect the pressure of a fixed amount of refrigerant vapor in a sealed cylinder?

When a fixed amount of refrigerant vapor is in a sealed cylinder, the volume is constant, so raising temperature makes the gas molecules move faster and collide with the cylinder walls more forcefully. That increased molecular activity pushes the walls harder, raising the pressure. This follows the gas law P = nRT / V, where with n and V fixed, pressure is directly proportional to temperature (in kelvin). So, higher temperature leads to higher pressure. The other ideas—pressure decreasing, no effect, or remaining constant—don’t align with how gases behave in a closed volume. In real refrigerants, very high pressures can show non-ideal behavior, but the general trend remains: temperature up means pressure up.

When a fixed amount of refrigerant vapor is in a sealed cylinder, the volume is constant, so raising temperature makes the gas molecules move faster and collide with the cylinder walls more forcefully. That increased molecular activity pushes the walls harder, raising the pressure. This follows the gas law P = nRT / V, where with n and V fixed, pressure is directly proportional to temperature (in kelvin). So, higher temperature leads to higher pressure. The other ideas—pressure decreasing, no effect, or remaining constant—don’t align with how gases behave in a closed volume. In real refrigerants, very high pressures can show non-ideal behavior, but the general trend remains: temperature up means pressure up.

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