Physical Chemistry: Gibbs Free Energy?
Upon expanding two moles of an ideal gas fourfold at 400K, the Gibbs free energy of the gas has...
a)increased by 9.2 kJ
b)decreased by 9.2 kJ
c)increased by 4.6 kJ
d)decreased by 4.6 kJ
If someone can offer an explanation of how to do this problem that would be great! Thank you so much!
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Verified answer
dG = V*dP - S*dT
Since T is constant, dT = 0
dG = V*dP = (nRT/P)*dP
deltaG = nRT * ln(P/Po)
According to Boyle's law, P/Po = Vo/V.
deltaG = nRT * ln(Vo/V)
deltaG = (2 mol)*(8.314 J*K^-1*mol^-1)*(400K)*ln(1/4)
deltaG = -9220 J = -9.22 kJ
Thus, the Gibbs free energy of the gas has decreased by 9.2 kJ.
specific, fee of Gibbs loose ability (delta G) and Gibbs loose ability below huge-unfold circumstances (delta G knot) is comparable in the event that they're the two calculated below the comparable temperature (298K) inspite of the undeniable fact that it is going to additionally be reported to maintain a million atm stress additionally.