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Question
One mole of a gas is expanded from 1 L, 10 atm, 300 K to 4 L, 5 atm, 600 K against a constant external pressure of 1 atm. The heat capacity of gas is 50 J/K.Then the internal energy change during the process is: (1 L atm ≃100 J).
One mole of a gas is expanded from 1 L, 10 atm, 300 K to 4 L, 5 atm, 600 K against a constant external pressure of 1 atm. The heat capacity of gas is 50 J/K.Then the internal energy change during the process is: (1 L atm ≃100 J).
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Solution
The correct option is A △U=14.7 kJ
State 1State 2(1 L, 10 atm, 300 K)(4 L, 5 atm, 600 K)
Heat given, q=nC△T
where, C is the heat capacity and △T is the change in Temperature
Therefore,
q=50(600−300)=15000 J
And,
W=−Pext(V2−V1)=−1(4−1)=−3 L atm=−300 J
△U=q+W=15000−300=14700 J
State 1State 2(1 L, 10 atm, 300 K)(4 L, 5 atm, 600 K)
Heat given, q=nC△T
where, C is the heat capacity and △T is the change in Temperature
Therefore,
q=50(600−300)=15000 J
And,
W=−Pext(V2−V1)=−1(4−1)=−3 L atm=−300 J
△U=q+W=15000−300=14700 J
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