Question

A sample of O2 gas has a volume of 19.0 L at a pressure of 1.50 atm and a temperature of 23 °C. What volume, in liters, will the gas occupy at 3.50 atm and 271 °C? Assume ideal behavior

Answer 1

From ideal gas equation PV = nRT

Where

T = Temperature

P = pressure

n = No . of moles

R = gas constant = 0.0821 L atm / mol - K

V= Volume of the gas

Since the mass of O2 gas should not change n remains same so PV / T = P'V'/T'

Where

P = initial pressure = 1.5 atm

P' = final pressure = 3.50 atm

V = initial volume = 19.0 L

V' = final volume = ?

T = initial temperature = 23 ^oC = 23+273 = 296 K

T' = final temperature = 271 ^oC = 271+273 = 544 K

Plug the values we get V' = PVT' / TP'

                                          = ( 1.50 x 19.0 x 544 ) / ( 296 x 3.50 )

                                          = 14.96 L

                                          ~ 15.0 L

Therefore the required volume is 15.0 L