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ipitydatfu
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i was given this test problem a couple of days ago, that ha2 parts:
1 mol of ideal
a) isothermal reversible at a Ti, Pi = 3 atm, Pf= 1 atm
b)irreversible isothermal expansion under constant pressure (1 atm) .
find the heat/work/internal energy, delta(H), entropy for both.
attempt:
part a is easy, that was well covered over the lecture/internets/various physics book
but for part b, i wasnt so sure
for my answers i put something in the lines of:
U = q + w, deltaU = 0
therefore
q = -w
H = 0 (not too sure)
i guess since its under constant pressure
q = -w, and w = -p (delta v)
q = (1 atm)(Vf - Vi) (volumes were found from ideal gas law)
and Entropy
S = Ssys + Ssur
S = q/t + Ssur
how do i get the entropy surroundings? and how far off am i?
edit: bump no love for this thread?
1 mol of ideal
a) isothermal reversible at a Ti, Pi = 3 atm, Pf= 1 atm
b)irreversible isothermal expansion under constant pressure (1 atm) .
find the heat/work/internal energy, delta(H), entropy for both.
attempt:
part a is easy, that was well covered over the lecture/internets/various physics book
but for part b, i wasnt so sure
for my answers i put something in the lines of:
U = q + w, deltaU = 0
therefore
q = -w
H = 0 (not too sure)
i guess since its under constant pressure
q = -w, and w = -p (delta v)
q = (1 atm)(Vf - Vi) (volumes were found from ideal gas law)
and Entropy
S = Ssys + Ssur
S = q/t + Ssur
how do i get the entropy surroundings? and how far off am i?
edit: bump no love for this thread?
Last edited: