A mixture of fuel containing $40\%$ mol CH$4,30\%$ mol C$2$H$6,$ and $30\%$ mol C$4$H$10$ initially at $300\mathrm{.}15$ K was burned in a furnace with $50\%$ excess air initially at $323\mathrm{.}15$ K$,$ at a pressure of $760$ mm Hg$,$ and with $80\%$ RH$.$ The fractional conversions of CH$4,$ C$2$H$6,$ and C$4$H$10$ were $0\mathrm{.}95,0\mathrm{.}90,$ and $0\mathrm{.}85,$ respectively. Of the fuel burned, $90\%$ of the total carbon content of the fuel was converted to CO$2$ and the balance to CO while $95\%$ of the total hydrogen $($H$2)$ content of the fuel was converted to water and the balance exited as H$2$ gas. Starting with a basis of $100$ moles of the fuel mixture,

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