Physics Question Two cylinders each contain 0.15 mol of a diatomic gas at 330 K
ID: 1441012 • Letter: P
Question
Physics Question
Two cylinders each contain 0.15 mol of a diatomic gas at 330 K and a pressure of 3.0 atm. Cylinder A expands isothermally and cylinder B expands adiabatically until the pressure of each is 1.0 atm.
What is the final temperature of the gas in the cylinder A?
Express your answer to two significant figures and include the appropriate units.
What are the final temperature of the gas in the cylinder B?
Express your answer to two significant figures and include the appropriate units.
What is the final volume of the gas in the cylinder A?
Express your answer to two significant figures and include the appropriate units.
What is the final volume of the gas in the cylinder B?
Express your answer to two significant figures and include the appropriate units.
Explanation / Answer
(A)
Final temperature of the gas in the cylinder A,
As the expansion is Isothermal, There is no change in Temperature.
T = 330 K
(B)
Final temperature of the gas in the cylinder B,
pv = nRT
3*101352* Vi = 0.15*8.314*330
Vi = 1.35 * 10^-3 m^3
For Adiabatic Process,
PV^ = constant
For Diatomic gas, = 1.4
p*v^1.4 = const
3.0 * ( 1.35 * 10^-3 )^1.4 = 1.0 * vf^(1.4)
vf = 2.96 * 10^-3 m^3
p*v = nRT
101325 * 2.96 * 10^-3 = 0.15*8.314*T
T = 240.5 K
(C)
Final volume of the gas in the cylinder A,
Using Ideal Gas Law,
pv = nRT
pv = 0.15*8.314*330
In Isothermal Expansion, T is constant,
So PV = Constant
101325 *v = 0.15*8.314*330
v = 4.06 * 10^-3 m^3
(D)
Final volume of the gas in the cylinder B,
vf = 2.96 * 10^-3 m^3