Entropy – How do I proceed?
Hi everyone,
I'm faced with the problem that I don't know how to solve this problem:
Can anyone help me?
Thanks in advance to everyone who tries it 🙂
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Can someone explain task 2 to me?
Can someone explain task 2 to me?
Before I find the wheel again, I prefer to refer to the following Link, where the subject is precisely described. I think that should help.
But how do I use the c,pm values? The formula would be deltaS = n*cp,m*ln(T2/T1) but why should I count on the enthalpy of evaporation?
(a)
First, the entropy increases with the temperature. This is only linear in good approximation, since the increase in entropy takes place with the logarithm, but it doesn’t matter in the small temperature range.
The water then evaporates at 100° C. whereby the entropy increases accordingly. When the steam is overheated, the entropy then again rises approximately linearly.
(b)
1) Water heating:
ΔS = n * c_p,m * ln(T2/T1)
n= 1 mol
c_p,m = 75,29 J/molK
T1 = 273,15 K
T2 = 373,15 K
ΔS = 1 mol * 75.29 J/molK * ln(373,15/273,15) = 23.49 J/K
2) Evaporating the water:
ΔS = dQ/T = 1 mol * 40.66 kJ/mol / 373,15 K = 108.96 J/K
3) Overheating steam is like 1)
Entropy for ideal liquid and ideal gas should be created.
The evaporation enthalpy is actually only the evaporation enthalpy divided by the temperature 😉
If necessary, you can derive this from the entropy balance for evaporation.