A 1.73 mole sample of Ar undergoes an isothermal reversible expansion from an in
ID: 1048945 • Letter: A
Question
A 1.73 mole sample of Ar undergoes an isothermal reversible expansion from an initial volume of 2.00 L to a final volume of 85.0 L at 311 K. Calculate the work done in this process using the ideal gas equation of state. Express your answer using three significant figures. Calculate the work done in this process using the van der Waals equation of state. Express your answer using three significant figures. What percentage of the work done by the van der Waals gas arises from the attractive potential? Express your answer using two significant figures.Explanation / Answer
c) What percentage of the work done by the van der Waals gas arises from the attractive potential?
Increase in work done by the van der waals gas = Work done using van der waals eq. Less Work done using ideal gas equation
% Work = Preal - Pideal
= -16,675.81 - (-1.68 x 104)
= 124.19J
=0.1249 kJ
% Increase = {(1.68 x 104 - (16,675.81 )/16,675.81 }*100 = 0.7447 %
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