The difference between heats of reaction at constantpressure and constant volume for the reaction2C6H6 (I) + 1502(g) 12CO2 (g) + 6H2O(I)at25?C in kJmol-1 is1)-7.432)+3.723)-3.724)+7.43

Dear Student,

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

ΔH-ΔU=Δn_gRT

Δn_g=12-15=-3

Δn_gRT=(-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