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When one mole of gaseous methane s burnt...

When one mole of gaseous methane s burnt in excess of gaseous oxygen, 890 kJ of heat is evolved in addition to the formation of gaseous `CO_(2)` and liquid water. (a) Write the thermochemical equation for this reaction. (b) Calculate the amount of heat evolved when 10 grams of methane is burnt.

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(a) `CH_(4)(g) + 2O_(2)(g) rarr CO_(2)(g) + 2H_(2)O(l) Delta H = -890 kJ`
(b) From the equation
`1 " mole of "CH_(4) = 16g = 890 kJ " heat"`
`16g CH_(4)` releases `= 890 kJ` heat
`10 g CH_(4)` releases `= (890 kJ xx 10 g)/(16g) = 556 kJ`
Amount of heat liberated for the combustion of 10 g `CH_(4) = 556 kJ`.
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