Calculate the maximum work done (in cal) when pressure on 10 gram of hydrogen is reduced from 20 to 1atm at a constant temperature of 273K. the gas behave Ideally
A
8192.6cal
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B
9258.3cal
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C
5924.2cal
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D
2896.4cal
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Solution
The correct option is A8192.6cal work done in isothermal reversible process is given as: W=−2.303nRTlogP1P2
n = number of moles of hydrogen n=given weightmolar mass = 102=5mol
Given : P1=20atm P2=1atm T=273K R=2cal/K.mol
so, w=−2.303×5×2×273×log201
= −8192.6Cal