When ethanol (grain alcohol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) ) is
burned in oxygen, approximately \(1360 \mathrm{~kJ}\) of heat energy is released
per mole of ethanol.$$\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+3
\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2}
\mathrm{O}(g)$$
a. What quantity of heat is released for each gram of ethanol burned?
b. What is \(\Delta H\) for the reaction as written?
c. How much heat is released when sufficient ethanol is burned so as to
produce 1 mole of water vapor?