In the cycle shown in the figure, (1) 1.00 mol of an ideal diatomic gas is initi
ID: 1618947 • Letter: I
Question
In the cycle shown in the figure, (1) 1.00 mol of an ideal diatomic gas is initially at a pressure of 1.00 atm and a temperature of 0.0 degree C. (2) The gas is heated at constant volume to T_2 = 160 degree C, and (3) is then expanded adiabatically until its pressure is again 1.00 atm. It is then compressed at constant pressure back to its original state. (a) Find the temperature after the adiabatic expansion. degree C (b) Find the heat absorbed or released by the system during each step. Q_1-2 = kJ Q_2-3 = kJ Q_3-1 = kJ (c) Find the efficiency of this cycle. % (d) Find the efficiency of a Carnot cycle operating between the temperature extremes of this cycle. %Explanation / Answer
P1/T1 = P2/T2 vol constant process
1/273 = P2/433
P2 = 1.586 atm
for the adiabatic process P^{(1-)/}T = constant
P3=1atm ;
a)T3 = 379.54 K
b) in volume const process Q = nCvT = 3328 J
in adiabatic processs Q = 0
const pressure Q = nCpT = -3102.45 J
c)W output
in volume const process W1 = 0
in adiabatic processs Q = 0 W2 = -nCvT = 1111.97 J
in constant pressure process W3 = nRT = -885.77J
= 6.78
d)1-Tlow/Thigh = 38.95%