Answer to Question #275411 in Physical Chemistry for NORAMIRA

Question

n moles of N2 gas (T1, V1) obey a van der Waals equation of state are contained in an insulated piston-cylinder arrangement. A reversible expansion of the gas is carried out until the volume become 2V1.

[CV.m = 28.80 J mol−1K−1, a = 1.37 L2.bar.mol-2, b = 0.0387 L. mol−1]

(a) Find the final temperature of gas as a function of n, 𝐂𝐂𝐕𝐕.𝐦𝐦 , T1, V1 and the van der Waals parameter a and b.

(b) If two moles of N2 gas involved and T1 = 350K, V1 = 40L, compute final temperature of the gas.

(c) Find work done and internal energy of the gas.

Answer 1

a)Temperature of gas =53.6°C

b)Final Temperature =42.6°C

c)Work Done =280kW

Internal Energy =-479kJ