One mole of a Vanderwaals gas at 300 K expands isothermally and reversibly from volume 10.064 L to 50.064 L. Vanderwaals constant a = 5 lit 2 atm mol –2 and b = 0.064 L/mole log 3 = 0.48 ; log 2 = 0.3 ; log 5 = 0.7 Determine the work done by the system in J/mole in nearest possible integers.
Text Solution
Verified by ExpertsCHECK THE SOLUTION.
3981
Sol. Δ W = – 
dV
or Δ W = – RT ln 
– a 
or Δ W = – 0.082 × 300 × 2.303 × log 
– 5 
or Δ W = – 0.082 × 300 × 2.303 × 0.7
+ 
or Δ W = – 39.66 + 0.3969 = – 39.2631 L atm.
or Δ W = – 39.2631 × 
J
= – 3980.89 ~ –3981 J/mole
work done by the system = 3981 J
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