Q. 5

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
A. 2C4H10(g) + 13O2(g) 8CO2(g) + 10H2O(l)ΔcH = 2658.0 kJ mol1

B. C4 H10(g) + O2 (g) 4CO2 (g) + 5H2 O (g) Δc H = –1329.0 kJ mol–1

C. C4H10(g) + O2 (g) 4CO2 (g) + 5H2O (l) ΔcH = 2658.0 kJ mol–1

D. C4H10 (g) + O2 (g) 4CO2 (g) + 5H2O (l) ΔcH = +2658.0 kJ mol–1

Answer :

Reason: -

A. As it is provided that there is combustion of 1 mole of butane.


B. The heat released during the combustion of butane is 2658 kJ.


C. In this reaction, there is a combustion of 1 mole of butane and the energy released is 2658 kJ.


D. In this reaction, there is also combustion of 1 mole of butane but the sign of ΔcH is positive, which is indicating that we have given that much amount of energy.

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