1.4 g of N2 are placed in a cylinder at an initial volume of 3.8 L and allowed to expand isothermally to a final volume of 10.8 liters against a constant external pressure of 0.8 bar.
(A) Treating N2 as a perfect gas, find q, w, ΔU, ΔH, and ΔS for this process.
(B) Now assume that the same process occurs, but that N2 can be assumed to have attractive forces between the molecules. In this case, how would q differ from the answer given in (A)? Specifically, would the value be larger, smaller, or unchanged? Explain your answer in 10 words or less.
Can you please explain part a and b?
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Ne has a mass of 20.18 amu, N2 has a mass of 28.01 amu, H2 has a mass of 1.01 amu, Ar has a mass of 39.95 amu, and He has a mass of 4.00 amu.
N2 gas has =1.4/28 mol
= 0.05 mol constant pressure =0.8 bar
Expand isothermally
N2 as ideal gas
Vi=3.8 L
Vf = 10.8 L
q=? ; w=? ;
For isothermal process : T = 0 ( temperature constant)
ΔU = ΔH = 0
w= -(0.8*100000)*(10.8-3.8)*(0.001) *(0.05) J
= -28J
q=(-w)
= 28J
S 0 ( Entropy increased)
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