mass of $CO _{2}( g )=330\, g$
mass of $H _{2} O (\ell)=270\, g$
mass of carbon $= n _{ CO _{2}} \times 12$
$=\frac{330}{44} \times 12=90 \,g$
$\,\%$ of carbon $=\frac{90}{120} \times 100=75 \,\%$
mass of hydrogen $= n _{ H _{2} O } \times 2$
$=\frac{270}{18} \times 2=30 \,g$
$\,\%$ of hydrogen $=\frac{30}{120} \times 100=25 \,\%$
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
$\begin{array}{*{20}{c}}
{C{H_3} - C = CH - C{H_2}C{H_3}} \\
{|\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \\
{CH{{(C{H_3})}_2}\,\,\,\,\,\,\,\,\,\,}
\end{array}\xrightarrow[{(ii)\,{H_2}{O_2},O{H^ - }}]{{(i)\,{B_2}{H_6}}}[A]$$\xrightarrow[\Delta ]{{dil.\,{H_2}S{O_4}}}[B]$
......$kJ/mole$