An ideal gas, initially at P1 = 0.75 bar, undergoes an adiabatic expansion from V1 =...
An ideal gas, initially at P1 = 0.75 bar, undergoes an adiabatic expansion from V1 = 10.0 L to V2 = 30.0 L. What is the final pressure and temperature of this gas? Explain how you got this.
Homework Answers
Here we are assuming that the ideal gas is monoatomic,
gamma = 5/3
For adiabatic expansion,
PV^gamma = constant
0.75*10^(5/3) = P2 *30^(5/3)
P2 = 0.12 bar answer
Now assuming that number of moles taken was 1 mol (this will be needed as initial temperature was not given). Now using ideal gas equation,
T2 = P2V2/nR = 0.12*10^5*30*10^-3/[1*8.3]
= 43.37 K
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