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kalbuskj31
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Homework Statement
An Ideal Gas at 300K has a volume of 15L and a pressure of 15 atm. Calculate the change when the system goes under a reversible adiabatic expansion to a pressure of 10 atm. Gamma = 5/3. Cv = 1.5R. q = 0(definition of adiabatic processes).
Homework Equations
dw = P DV (lowercase means squiggly d and uppercase means straight d)
P = nRT/V
The Attempt at a Solution
The answer in the book says w = 5130 J, which is the opposite of what I got for the internal energy.
First, I calculated n: n = PV/RT = 15 atm * 15 L / .08206 (L*atm / K * mole) * 300K
n = 9.14 moles
Then, I calculated Vf: Vf = [(Pf * Vi ^ (5/3)) / (Pf)] ^ 3/5
Vf = 19.13 L
dW = P DV
dw = NRT (dw = P DV so then work = NRT * Integral [DV/V]) ****This is wrong since T changes temperature between states*****
w = nRT ln(Vf/Vi)
Plugged in everything and the answer didn't turn out.
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