- #1
Rocalvic
- 1
- 0
Homework Statement
Suppose 100g of ethane (C2H6) expands isothermally at 350C from 50ml to 2L. Calculate the heat and work done by the system and the change in entropy if:
i)The process is via a reversible path.
ii)The process is non-reversible.
I don't know how to answer ii)
Homework Equations
w=-nRTln(v2/v1)
The Attempt at a Solution
I have managed to answer i)
Work = -NRTln (v2/v1) = (0.30026)(8.315)(623.15)ln(2/0.050)
Work = -5738.79 J.
Entropy change = nRln (v2/v1) = (0.30026)(8.3145)ln(2/0.050)
Entropy Change = 9.209 J.K
Heat: Q=-w, so Heat = 5738.79.
ii) I am unsure how to answer this question, do I apply the same principle? Or is this a result of free expansion and therefore the work done is 0?
Thanks