20L of octane (Density =  $1.14g/m\mathcal{l}$) is burned in an engine in a test run. The total mass of  $CO,C{O}_2{\text{\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}\hspace{0.17em}and\hspace{0.17em}\hspace{0.17em}H}}_{2}O$ produced due to complete and incomplete combustion of octane is 87.44kg. The mole percentage of octane that is converted to CO is_________

 Mole of octane taken  $=\frac{20\times 1000\times 1.14}{114}=200$
 $$\begin{gathered} \underset{xmole}{C_8{H}_{18}}+\frac{25}{2}{O}_2\to \underset{8xmole}{8C{O}_2}+\underset{9xmole}{9H_{2}O} \\ {C}_8{H}_{18}+\frac{17}{2}{O}_2\to 8CO+9H_{2}O \\ (\text{ 2}00–x)mole 8(\text{ 2}00-x)mole 9(200-x)mole \end{gathered}$$
 From question:  $8x\times 44+8(200-x)\times 28+[9x+9(200-x\left)\right]\times 18=87440$

$\begin{array}{l}x=80\Rightarrow 200-x=120\\ \%\text{\hspace{0.17em}\hspace{0.17em}converted\hspace{0.17em}\hspace{0.17em}to\hspace{0.17em}\hspace{0.17em}}CO=\frac{120}{200}\times 100=60\end{array}$