100 cc. each of water gas and oxygen are ignited and the resultant mixture of gases cooled to room temp. Calculate the composition of the resultant mixture. [Water gas contains CO and H₂ in equal ratio]

Given,

Vol of CO = 50 cc and H₂ = 50 cc [As Water gas contains CO and H₂ in equal ratio] and O₂ = 100 cc

[By Lussac's law]

$\begin{matrix} \text{CO}& + & \text{H}$2 & + & \text{O}2 & \longrightarrow & \text{CO}2 & + & \text{H}2 \text{O} \ 1 \text{ vol.} & : & 1 \text{ vol.} & : & 1 \text{ vol.} & \longrightarrow & 1 \text{ vol.} & : & 1 \text{ vol.} & \ \end{matrix}

To calculate the amount of O₂ used,

$\begin{matrix} \text{CO}& : & \text{O}_2 & \ 1 \text{ vol.} & : & 1 \text{ vol.} & \ 50 \text{ cc} & : & x \text{ cc} & \ \end{matrix}$

As ratio between CO and O₂ is same so, O₂ used is 50 cc.

Hence, remaining O₂ = 100 - 50 = 50 cc.

To calculate the amount of CO₂ produced,

$\begin{matrix} \text{CO}& : & \text{CO}_2 & \ 1 \text{ vol.} & : & 1 \text{ vol.} & \ 50 \text{ cc} & : & y \text{ cc} & \ \end{matrix}$

1 vol of CO produces 1 vol. of CO₂
Hence, CO₂ produced = 50 cc.

Therefore, the resultant mixture has 50 cc of O₂ + 50 cc of CO₂