Two moles of helium are initially at a temperature of 21.0 ∘Cand occupy a volume of 3.30*10-2 m3. The helium first expands at constant pressure until its volume has doubled. Then it expands adiabatically until the temperature returns to its initial value. Assume that the helium can be treated as an ideal gas. B) What is the total change in internal energy of the helium? C) What is the total work done by the helium? D) What is the final volume of the helium?

(B) The total internal energy of the helium is 4888.6 Joules

(C) The total work done by the helium is 2959.25 Joules

(D) The final volume of the helium is 0.066 cubic meter

Explanation:

(B) ∆U = P (V2 - V1)

From ideal gas equation, PV = nRT

T1 = 21°C = 294K, V1 = 0.033m^3, n = 2moles, V2 = 2 * 0.033=0.066m^3

P = nRT : V = (2*8.314*294) : 0.033 = 148140.4 Pascal

∆U = 148140.4 (0.066 - 0.033) = 4888.6 Joules

(C) P2 = P1 (V1:V2) ^1.4 = 148140.4 (0.033:0.066) ^1.4 = 148140.4*0.379=56134.7 Pascal

Assuming a closed system

(C) Wc = (P1V1 - P2V2) : 0.4 = (148140.4*0.033 - 56134.7*0.066) : 0.4 = (4888.6 - 3704.9) : 0.4 = 1183.7 : 0.4 = 2959.25 Joules

(C) Final volume = 2*initial volume = 2*0.033 = 0.066 cubic meter