Background info: Evaporation of NH3(l) at its boiling point of -33.4degrees celcius and at a pressure of 100kPa requires heat absorption of 23.3x10^3 J mol-1.
Question: NH3(g) is condensed at its boiling point at a pressure that is infinitesimally greater than 100kPa. Calculate..
a) w per mole (J mol-1)
b) q per mole (J mol-1)
c) change in molar internal energy U (J mol -1)
d) change in molar enthalpy H (J mol-1)
Thanks for your help.
ΔU = q + w
ΔU = q - pextΔV
ΔH = ΔU +p ΔV
ΔH = ΔU + ΔngasRT
The Attempt at a Solution
[/B]P is also constant? because it's a condensation process?
(a) irreversible work?
(b) I would know when I figure out what w is.. (reverse)
(c) zero because T stayed the same
(d) isn't this already given in the question? (23.3 x 103)?