An oxide of an element contains 67.67% oxygen | vedclass

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(B) Calculation of equivalent weight:Weight of oxygen $= 67.67 	ext{ g}$Weight of element $= 100 - 67.67 = 32.33 	ext{ g}$$67.67 	ext{ g}$ of oxyge

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$15.28$

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(B) Calculation of equivalent weight:Weight of oxygen $= 67.67 	ext{ g}$Weight of element $= 100 - 67.67 = 32.33 	ext{ g}$$67.67 	ext{ g}$ of oxygen combines with $32.33 	ext{ g}$ of element.$8 	ext{ g}$ of oxygen combines with $\frac{32.33 	imes 8}{67.67} = 3.82 	ext{ g}$ of element.Equivalent weight of the element $= 3.82 	ext{ g}$.Let the valency of the element be $n$. The chloride is $MCl_n$.Equivalent weight of chloride $= 	ext{Equivalent weight of element} + 	ext{Equivalent weight of chlorine} = 3.82 + 35.5 = 39.32$.Molecular weight of chloride $= 2 	imes 	ext{Vapour density} = 2 	imes 79 = 158$.Valency $n = \frac{	ext{Molecular weight}}{	ext{Equivalent weight of chloride}} = \frac{158}{39.32} \approx 4$.Atomic weight $= 	ext{Equivalent weight} 	imes 	ext{Valency} = 3.82 	imes 4 = 15.28$.

An oxide of an element contains $67.67\%$ oxygen and the vapour density of its volatile chloride is $79$. What is the atomic weight of the element?

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