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## Homework Statement

One mole of a monatomic ideal gas is transformed from 0.00°C and 2.00 atm to

-40.0°C and 0.400 atm. Show that this is NOT an adiabatic reversible expansion and

calculate ΔS for the change. (Hint: you will need to consider a reversible path that

includes a constant pressure step and a constant temperature step.)

## Homework Equations

ΔU=q+w

pV=nRT

ΔS=nC(p,m)ln(V

_{f}/V

_{i})

## The Attempt at a Solution

For adiabatic reversible expansion, q=0, so i have to show that q= a number.

Found V

_{i}= 11.2L and V

_{f}=47.8L via ideal gas law

ΔS=(1mol)(5/2(8.314J/Kmol)ln(47.2/11.2)

=30.15J/K

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