At constant pressure, the ideal gas was heated from zero degrees Celsius

At constant pressure, the ideal gas was heated from zero degrees Celsius and the volume increased by 3 times. How many degrees Celsius was the gas heated?

Given:

T1 = 0 degrees Celsius = 273 degrees Kelvin – the initial gas temperature;

V1 = V – initial gas volume;

V2 = 3 * V – final gas volume;

P1 = P2 = const – gas pressure.

It is required to determine the final gas temperature T2 (Kelvin).

Since the process took place at constant pressure, then:

V1 / T1 = V2 / T2, hence:

T2 = V2 * T1 / V1 = 3 * V * 273 / V = 3 * 273 = 819 degrees Kelvin = 546 degrees Celsius.

Answer: the gas was heated to a temperature of 546 degrees Celsius.