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

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Grade 12Physical Chemistry

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

Pratik Sharma

16 Years agoGrade 12

2 Answers

Askiitians Expert Sahil Arora - IITD

16 Years ago

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

Saurabh Kumawat

7 Years ago

2C6H6(l)+15O2(g) -> 12CO2(g)+6H2O(l) at 25℃ in KJ/mol

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∆ng=12-15=-3

∆ngRT=(-3)×(8.314×10^-3KJ/mol/K)×298=-7.43

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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 1) -7.43 2) +3.72 3) -3.72 4) +7.43

Pratik Sharma

2 Answers

Askiitians Expert Sahil Arora - IITD

Saurabh Kumawat

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

at 25?C in kJ mol^-1 is

1)

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2)

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3)

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electrolysis