InterviewSolution
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InterviewSolution
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During complete combustion of one mole of butane ,2658Kj of heat is released. The thermochemical reaction for above change isA. `2C_(4)H_(10(g))+130_(2(g)) rarr 8CO_(2(g))+10H_(2)O_((l)) Delta H_(c) = -2658.0 kJ mol^(-1)`B. `C_(4)H_(10(g))+(13)/(2)O_(2(g)) rarr4CO_(2(g))+5H_(2)O_(l) Delta H_(c) = -1329.0 kJ mol^(-1)`C. `C_(4)H_(10(g))+(13)/(2)O_(2(g)) rarr 4CO_(2(g))+5H_(2)O_((l)) DeltaH_(c) = -2659.0kJ mol^(-1)`D. `C_(4)H_(10(g))+(13)/(2)O_(2(g)) rarr4CO_(2(g))+5H_(2)O_((l)) Delta H_(c) = +2658.0 kJ mol^(-1)` |
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Answer» Correct Answer - C Exothermic reaction for combustion of one mole of butane is represented as : `C_(4)H_(10(g))+(13)/(2)O_(2(g)) rarr 4CO_(2(g))+5H_(2)O_((l))` `Delta H_(c) = -2658.0 kJ mol^(-1)` |
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