Ethene undergoes incomplete combustion to form carbon dioxide, carbon monoxide and water vapour. If the ratio of carbon dioxide to carbon monoxide formed is 9:1 when x cm^3 of ethene is burnt, what is the volume of oxygen gas consumed in the reaction?

Md Ariful Islam

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Ethene undergoes incomplete combustion to form carbon dioxide, carbon monoxide and water vapour. The balanced equation of this incomplete combustion reaction is as follows.

$C_2H_4(g)+5/2O_2(g)->CO_2(g)+CO(g)+2H_2O(g)$

But as per question the ratio of volumes of $CO_2(g):CO(g)$ produced is $9:1$. So this also represents ratio of
$CO_2(g):CO(g)$ produced.

Hence adjusting this ratio balanced equation may be written as follows
$10C_2H_4(g)+39/2O_2(g)->9CO_2(g)+CO(g)+20H_2O(g)$

Here we see $10cm^3$ $C_2H_4(g)$ will require $39/2=19.5cm^3"" ""O_2(g)$

So to burn $xcm^3$ ethene the required volume of oxygen will be $19.5/10xx xcm^3=1.95xcm^3$

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