n = 3.76 mol of Hydrogen gas is initially at T = 302 K temperature and p i = 2.2
ID: 1483265 • Letter: N
Question
n = 3.76 mol of Hydrogen gas is initially at T = 302 K temperature and pi = 2.22×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 7.42×105Pa.
A) What is the volume of the gas at the end of the compression process?
B)How much work did the external force perform?
C )How much heat did the gas emit?
D) How much entropy did the gas emit?
E) What would be the temperature of the gas, if the gas was allowed to adiabatically expand back to its original pressure?
Explanation / Answer
Here , T = 302 K
Pi = 2.22 *10^5 Pa
Pf = 7.42 *10^5 Pa
A) for the final volume V2
P2 * V2 = n * R * T
7.42 *10^5 * V2 = 3.76 * 302 * 8.314
V2 = 0.0126 m^3
the final volume is 0.0126 m^3
B)
work done by platform = n * R * T ln(Pf/Pi)
work done by platform = 3.76 * 8.314 * 302 * ln(7.42/2.22)
work done by platform = 11391.8 J
the work done by platform is 11391.8 J
C)
as the change in internal energy is zero (isothermal process)
heat emitted by gas = - work done by platform
heat emitted by gas = - 11391.8 J
D)
entropy emitted = delta H/T
entropy emitted = 11391.8/302
entropy emitted = 37.7 J/K
the entropy emitted by gas is 37.7 J/K
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