Q. 5

# During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change isA. 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l)ΔcH = –2658.0 kJ mol–1B. C4 H10(g) + O2 (g) → 4CO2 (g) + 5H2 O (g) Δc H = –1329.0 kJ mol–1C. C4H10(g) + O2 (g) → 4CO2 (g) + 5H2O (l) ΔcH = –2658.0 kJ mol–1D. C4H10 (g) + O2 (g) → 4CO2 (g) + 5H2O (l) ΔcH = +2658.0 kJ mol–1

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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