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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
-7.43
+3.72
-3.72
+7.43
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
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