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Question
One mole of a gas is expanded from (1 L, 10 atm,300K) to (4 L, 5 atm,600K) against a constant external pressure of 1 atm. The heat capacity of gas is 50 J/K.Then the enthalpy change during the process is (1 L atm ≃ 100 J)
One mole of a gas is expanded from (1 L, 10 atm,300K) to (4 L, 5 atm,600K) against a constant external pressure of 1 atm. The heat capacity of gas is 50 J/K.Then the enthalpy change during the process is (1 L atm ≃ 100 J)
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Solution
The correct option is B △H=15.7 kJ
State 1 → State 2
(1 L, 10 atm, 300K) (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
△E=q+W=15000−300=14700 J
△H=△E+P2V2−P1V1=14700 J+(20−10)×100 J=15.7 kJ
State 1 → State 2
(1 L, 10 atm, 300K) (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
△E=q+W=15000−300=14700 J
△H=△E+P2V2−P1V1=14700 J+(20−10)×100 J=15.7 kJ
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