X litre of carbon monoxide is present at STP. | vedclass

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(B) The balanced chemical equation for the oxidation of carbon monoxide is:$CO(g) + \frac{1}{2} O_2(g) \longrightarrow CO_2(g)$According to the stoich

Vedclass · Accepted Answer

$11.207$

Vedclass · Answer

(B) The balanced chemical equation for the oxidation of carbon monoxide is:$CO(g) + \frac{1}{2} O_2(g) \longrightarrow CO_2(g)$According to the stoichiometry of the reaction,$1 	ext{ mole}$ of $CO$ produces $1 	ext{ mole}$ of $CO_2$.At $STP$,$1 	ext{ mole}$ of any ideal gas occupies $22.414 \ L$.Therefore,$22.414 \ L$ of $CO$ produces $22.414 \ L$ of $CO_2$.Since the volume of $CO_2$ formed is $11.207 \ L$,the volume of $CO$ $(X)$ required is also $11.207 \ L$ because the molar ratio is $1:1$.

$X$ litre of carbon monoxide is present at $STP$. It is completely oxidized to $CO_2$. The volume of $CO_2$ formed is $11.207 \ L$. What is the value of $X$ in litres?

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