Ethane $($C$2$H$6)$ burns completely with $110\%$ of theoretical air entering at $74$F$,1$ atm, $50\%$ relative humidity. The dry air component can be modeled as $21\%$O$2$ and $79\%$N$2$ on a molar basis. The combustion products leave at $1$atm$.$ Step $1$ Your answer is correct. For complete combustion of ethane $($C$2$H$6)$ with the theoretical amount of air, what is the number of moles of oxygen $($O$2)$ per mole of fuel? Determine the mole fraction of water in the products, in Ibmol$($water$)/$lbmol$($products$).$ yv$=$ Determine the dew point temperature of the products, in $$F$.$