1m^(3) of C_(2) H_(4) at STP is burnt in oxygen, according to the thermochemical reaction : C_(2)H_(4)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(l) , Delta H = -1410 kJ mol^(-1). Assuming 70% efficients, determine how much of useful heat is evolved in the reaction.

1m^(3) of C_(2) H_(4) at STP is burnt in oxygen, according to the ther

1.	1m^(3) of C_(2) H_(4) at STP is burnt in oxygen, according to the thermochemical reaction : C_(2)H_(4)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(l) , Delta H = -1410 kJ mol^(-1). Assuming 70% efficients, determine how much of useful heat is evolved in the reaction.
Answer» Solution :22.4 L of `C_(2)H_(4)` at STP produces 1410 kJ of energy 1000 L of `C_(2)H_(4)` at STP produces `(1410)/(22.4) xx 1000` (FULL efficiency) At 70% efficiency `= (1410)/(22.4)xx 1000 xx (70)/(100) = 44.02 xx 10^(3) kJ`.