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1. The problem statement, all variables and given/known data

One mole of monoatomic ideal gas initially at a pressure of 2.00 bar and temperature of 273 K is taken to a final pressure of 4.00 bar by the reversible path defined by P/V = constant. Calculate the values of Delta(H)(change in enthalpy), Delta(U)(potential energy), q(heat) and w(work). Cv = 12.5 kj*mol^-1*K^-1

2. Relevant equations

Delta(U) = q + w

Delta(U)= Cv*delta(t)

Delta(H)= Cp*delta(t)

Cv = 12.5 kj*mol^-1*K^-1

Cp = Cv - R

w = -Pext*delta(V)

q = Delta(U) - w

R = .08314 dm^3*bar*mol^-1*K^-1

I'm missing the equation for work in this situation as the reversible path is defined by P/V = constant.

3. The attempt at a solution

I found the change in enthalpy and the potential energy. They are correct, the textbook lists quantitative answers. However, the work is proving difficult as I don't understand the reversible path condition(P/V = constant) and how to relate that the energy of work. I know that it relates in some way to the ideal gas equation of state, but I cannot figure out that way. Thank you, I'm not sure if this should be introductory physics or advanced forum, so i've placed it in both.

What i've calculated so far, all are correct according to the text:

Delta(U) = 10.23 KJ*mol^-1

Delta(H) = 17.01 KJ*mol^-1

V1 = 11.35 dm^3

V2 = 22.7 dm^3

T1 = 273 K

T2 = 1092 K

thanks again

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# Homework Help: Expansion of an Ideal gas(molecular thermodyanmics)

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