To find the formula of a compound composed of iron and carbon monoxide ${Fe}_{x} {(CO)}_{y}$ , the compound is burned in pure oxygen and the following reaction occurs :
${Fe}_{x} (CO)_{y} + O_{2} ⟶ {Fe}_{2} O_{3} + {CO}_{2}$
If 19.6 gm of ${Fe}_{x} (CO)_{y}$ is burnt and 8 gm ${Fe}_{2} O_{3}$ is formed, then the empirical formula of ${Fe}_{x} {(CO)}_{y}$ is:

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$Fe (CO)_{3}$

$Fe (CO)_{5}$

$Fe (CO)_{4}$

${Fe}_{2} (CO)_{5}$

answer is D.

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Detailed Solution

${Fe}_{x} (CO)_{y} + O_{2} ⟶ {Fe}_{2} O_{3} + {CO}_{2}$

$\begin{array}{l} \frac{19.6}{56 x + 28 y} = \frac{8}{160} \times 2 \end{array}$

$\Rightarrow 2 x + y = 7$

Thus, the empirical formula of ${Fe}_{x} {(CO)}_{y}$ is $Fe (CO)_{5}$

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