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Pratik Sharma Grade: 12
        



The difference between heats of reaction at constant pressure and constant volume for the reaction


2C6H6 (I) + 1502(g) "12CO2 (g) + 6H2O (I)


at 25?C in kJ mol-1 is




1)


 -7.43 





2)


 +3.72





3)


-3.72    





4)


+7.43




7 years ago

Answers : (1)

Askiitians Expert Sahil Arora - IITD
19 Points
										

Dear Student,


Heat of reaction at constant pressure is ΔH and at constant volume is ΔU.


ΔH-ΔU=ΔngRT


Δng=12-15=-3


ΔngRT=(-3)*(8.314*10-3KJ/mol/K)*(298 K)=-7.43


one more thing,someone may think of dividing the reaction by 2..but that will be wrong.


On multiplying by a factor,ΔH and ΔU also get multiplied by the factor..


All the best Pratik !!!





Regards,

Askiitians Experts

Sahil Arora
7 years ago
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