At a temperature of 274 K, the gas in a cylinder has a volume of 2.0 liters. If the volume of the gas is increased to 4.0 liters, what must the temperature be for the gas pressure to remain constant?

Question

anonymous · Answer

We can use the ideal gas law! 

$$P V = nRT$$

We can relate the two states of the gas as$${P_1 V_1 \over nRT_1} = {P_2V_2 \over nRT_2}$$

The system is closed, therefore the amount of the gas remains constants so the n cancels out. Additionally, R is a constant and also cancels. $${P_1 V_1 \over T_1} = {P_2V_2 \over T_2}$$

The problems states that the pressure at both states should be constant, therefore $P_1 = P_2$

$${ V_1 \over T_1} = {V_2 \over T_2}$$

We can see from the below expression that if the volume is doubled, the temperature must be doubled as well $${V_2 \over V_1} = {T_2 \over T_1}$$

anonymous · Answer

ya i now how to set it up but i cant get the right answer

anonymous · Answer

Liters and Kelvin is a valid unit combination for Charles's Law and the Ideal Gas Law. 

You should be getting 548K.