n = 3.74 mol of Hydrogen gas is initially at T = 303 K temperature and p i = 3.3
ID: 1565116 • Letter: N
Question
n = 3.74 mol of Hydrogen gas is initially at T = 303 K temperature and pi = 3.33×105 Pa pressure. The gas is then reversibly and isothermally compressed until its pressure reaches pf = 7.21×105 Pa. What is the volume of the gas at the end of the compression process?
How much work did the external force perform?
7.27×103 J
How much heat did the gas emit?
7.27×103 J
How much entropy did the gas emit?
What would be the temperature of the gas, if the gas was allowed to adiabatically expand back to its original pressure?
2.43×102 K
** just need parts 1 and 4! Thank you please include units.
Incompatible units. No conversion found between "atm" and the required units. Tries 0/12 Previous TriesExplanation / Answer
1.
Using ideal gas law:
PV = nRT
when the temperature is constant
P1V1 = P2V2
V2 = P1V1/P2
P1 = 3.33*10^5 Pa
P2 = 7.21*10^5 Pa
V1 = nRT1/P1
V1 = 3.74*8.314*303/(3.33*10^5) = 0.0282 m^3
V2 = 3.33*10^5*0.0282/(7.21*10^5) = 0.013 m^3
4.
dS = Q/T
dS = 7.27*10^3/303 = 23.99 J/K
dS = 24 J/K
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