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RJWills
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Homework Statement
"In the following a<b<c are finite positive constants. One mole of an ideal monoatomic gas, initially at volume Vi and temperature 1000K, expands to a final volume cVi in 3 reversible steps: (1) isothermal expansion from Vi to aVi (2) adiabatic expansion from aVi to bVi (3) isothermal expansion from bVi to cVi.
b)a) Make careful sketches, approximately to scale, of how i) the pressure ii) the temperature and iii) the entropy evolve with volume.
Homework Equations
pV=nRT,
W = ∫pdV
ΔU= Q-W
W=nRTlnVf/Vi
The Attempt at a Solution
I've come up with these after quite a bit of thinking:
a) i)pV:
ii)Temp v pressure.This doesn't look right to me, but my reasoning is, first step temp stays the same, reversible adiabatic expansion has no ΔQ and again isothermal keeps it the same. Right? The only thing I can think is there's a problem in my understanding of a adiabatic reversible expansion- how does the temp change?!
Entropy vs Volume
*Just realized I should have arrows an all isotherms because it's reversible