Thermal (Entropy / Enthalpy)

1. The problem statement, all variables and given/known data
Gas has a heat capacity of (C_v = (3/2)nR), intial temp of T_o, pressure P_o and volume V_o.

Process a to b is a quasistatic isobaric expansion to twice the intial volume

Find
a) work done,
b) heat transfer,
c) change in internal energy,
d) change in enthalpy
e) change in entropy
In terms of n(moles), R, T₀

2. Relevant equations

W = -P(delta)V
(delta)U = Q + W = (f/2)nR(delta)T
PV = nrT
H = U + PV


3. The attempt at a solution
Now this is what ive come up with but im unsure about enthalpy and entropy (this mostly), they seem ok but look wrong. I dont have any answer or similar questions to check it againt first and only isobaric cycle. Looking on the net ive found mostly constant U, while V changes which isnt helpful.

Attached is my attemp if any1 can shine any light on the last two points or anything else



Thanks Trent

 

Im basing this [tex]\Delta S = \int_{T_i}^{T_f} \frac{C_P}{T}\mathrm{d}T[/tex], from this

"When T is changing, it's usually more convenient to write the relation in terms of the heat capacipty at constant volume: dS = (C_VdT)/T."
Now we dont have constant volume so ive discarded that

Over the page than it says,
"constant pressure processes in which the temperature changes, we can write Q = C_PdT, than integrate to obtain,

[tex]\Delta S_P= \int_{T_i}^{T_f} \frac{C_P}{T}\mathrm{d}T[/tex]

This correct or i may have read misunderstood something, i agree it should be C_V rather than C_P, but from my understanding thats for constant volume??

If any1 can shine some light thanks heeps

Cheers Trent