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Question

What will be the amount of heat evolved by burning 10 L of methane under standard conditions?
(Given heats of formation of CH4,CO2 and H2O are -76.2, -398.8 and -241.6 kJmol1 respectively)

A
805.8 kJ
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B
398.8 kJ
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C
359.7 kJ
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D
640.4 kJ
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Solution

The correct option is A 359.7 kJ
CH4+2O2CO2+2H2O
ΔH=HPHR
=ΔHf(CO2)+2ΔHf(H2O)[Δf(CH4)+2ΔHf(CO2)]
=398.8(2×241.6)(76.2+2×0)
=805.8 kJ
22.4 L of CH4(1mole) gives 805.8 kJ
10 L of CH4 will give 805.822.4×10=359.73 kJ


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