The heats of combustion of ethane (C2H6) and butane (C4H10) are 52 kJ/g and 49 k

Question

The heats of combustion of ethane (C2H6) and butane (C4H10) are 52 kJ/g and 49 kJ/g, respectively, I want to produce 1000 kJ by burning one of the fuels. Which fuel will emit the least amount of CO2? Please show work!

Explanation / Answer

C2H6 + 7/2 02 ---> 2C02 + 3H2O , delta H = -1560 kJ / mole... (bcoz 52 kJ/g) to get 1000 kJ, no of moles of C2H6 to be burnt = 1000/1560 x 1 = 0.641 moles of ethane... This reaction liberates 2 x 0.641 moles = 1.282 moles of CO2... C4H10 + 13/2 02 ---> 4C02 + 5H2O , delta H = -2842 kJ / mole... (bcoz 49 kJ/g) to get 1000 kJ, no of moles of C4H10 to be burnt = 1000/2842 x 1 = 0.352 moles of ethane... This reaction liberates 4 x 0.352 moles = 1.408 moles of CO2... To get 1000kJ, C2H6 should be burnt, to liberate minimum CO2...

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