(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

C02 from a can of soda expands irreversibly against the atmospher. Assume the process is adiabatic and Pi = 3 bar. Assume C02 to be an ideal gas with Cp = 37 j/mol*K. Find the final temperature of CO2 after it has reached atmospheric pressure.

Thats all I get...

2. Relevant equations

Adiabatic implies dq = 0

constant Pext implies dw = -Pext dV

Ideal gas implies dU = CvdT

1st Law gives dU = -Pext dV

we go from here

3. The attempt at a solution

nCvdT = -Pext dV

integrating

nCv(T2-T1) = -Pext (V2-V1)

using PV=nRT the above equation reduces

nT2(Cv+R) = nT1(Cv+Pext*R/P1)

we can take Pext/T2 = P1/T1 ?? but this system does not yield a solution for T1, T2

here is were I am stuck seeing as how I dont know T1 or T2 (obviously n's cancel out)

If we take the can as the system

the first law energy balance gives

dU/dt = -dn_out/dt * H

this reduces to the standard adiabatic equation

(T2/T1)^Cp/R = Pext/P1

an attempt with the concervation of mass yields

dn/dt = -dn_out/dt we can sub in the ideal gas equation for n and get

d(p/T)/dt = -dn_out/dt * R/nV but I dont think we know anything about n or dn_out/dt

so I am stuck, help please!!

Thanks

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# Homework Help: Thermodynamics of open soda can

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