A 50.0 L sealed cylinder contains 100.0 moles of helium gas. Its pressure at 273.0 K is 44.8 atm. What is the pressure when the gas is heated to 500.0 K.

Question

A 50.0 L sealed cylinder contains 100.0 moles of helium gas. Its pressure at 273.0 K is 44.8 atm. What is the pressure when the gas is heated to 500.0 K.

Answer 1

Given:

Initial volume = V1 = 50.0L

Initial moles = n1 = 100.0 moles

Initial pressure = P1 = 44.8 atm

Initial temperature = T1 = 273.0K

Final temperature = 500.0K

Asked to find:

Final pressure = P2 = ?

Since the only variables that change are the temperature and the pressure (moles and volume are constant), we will use P1/T1 = P2/T2 and solve for P2:

44.8 atm / 273K = P2 / 500K

P2 = 82.1 atm