The heat evolved in the combustion of methane is given by the equation `:` `CH_(4)(s) + 2O_(2)(g) rarr CO_(2)(g) + 2H_(2)O(l), DeltaH = - 890 .3 kJ mol^(-1)` (a ) How manygrams of methane would be required to produce 445.15 kJ of heat of combustion ? (b ) How many grams of carbon dioxide would beformed when 445.15 kJ of heat is evolved ? (c ) What volume of oxygen at STP would be used in the combustion process (a ) or (b) ?

The heat evolved in the combustion of methane is given by the equation

1.	The heat evolved in the combustion of methane is given by the equation `:` `CH_(4)(s) + 2O_(2)(g) rarr CO_(2)(g) + 2H_(2)O(l), DeltaH = - 890 .3 kJ mol^(-1)` (a ) How manygrams of methane would be required to produce 445.15 kJ of heat of combustion ? (b ) How many grams of carbon dioxide would beformed when 445.15 kJ of heat is evolved ? (c ) What volume of oxygen at STP would be used in the combustion process (a ) or (b) ?
Answer» (a) From the given equation , 890.3 kJ of heat is produced from 1 mole of`CH_(4), i.e., 12+4 = 16 g ` of `CH_(4)` (b ) `:. 445.15kJ` of heat is produced from 8g of `CH_(4)` (b) From the given equation, when 890.3 kJ of heat is evolved , `CO_(2)` formed `=1` mole `=44 g ` `:. `When 445.15 kJ of heat is evolved , `CO_(2)` formed `= 22g` (c ) From the equation , `O_(2)` used in the production of 890.3 kJ of heat `=2` moles `= 2 xx 22.4 ` litres at STP `= 44.8` litres at STP Hene, `O_(2)` used in the production of 445.1 5 kJ of heat = 2 22.4 litres at STP.

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