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» <html><body><p></p>Solution :22.<a href="https://interviewquestions.tuteehub.com/tag/4-311707" style="font-weight:bold;" target="_blank" title="Click to know more about 4">4</a> L of `C_(2)H_(4)` at STP produces 1410 kJ of energy <br/> 1000 L of `C_(2)H_(4)` at STP produces `(1410)/(22.4) xx 1000` (<a href="https://interviewquestions.tuteehub.com/tag/full-1001178" style="font-weight:bold;" target="_blank" title="Click to know more about FULL">FULL</a> efficiency) <br/> At 70% efficiency `= (1410)/(22.4)xx 1000 xx (70)/(100) = 44.02 xx 10^(<a href="https://interviewquestions.tuteehub.com/tag/3-301577" style="font-weight:bold;" target="_blank" title="Click to know more about 3">3</a>) kJ`.</body></html>