What is the empirical formula of vanadium oxide, if $2.74 \mathrm{~g}$ of the metal oxide contains $1.53…

What is the empirical formula of vanadium oxide, if $2.74 \mathrm{~g}$ of the metal oxide contains $1.53 \mathrm{~g}$ of metal?
  1. $\mathrm{V}_{2} \mathrm{O}_{3}$
  2. $\mathrm{VO}$
  3. $\mathrm{V}_{2} \mathrm{O}_{5}$
  4. $\mathrm{V}_{2} \mathrm{O}_{7}$

Solution

Mass of oxide $=$ Mass of metal $+$ Mass of oxygen
$2.74=1.53+\mathrm{W}_{\text {Oxygen }} \Rightarrow \mathrm{W}_{\text {Oxygen }}=1.21 \mathrm{~g}$
Moles of $\mathrm{V}=\frac{1.53}{51}=0.03$
Moles of $\mathrm{O}=\frac{1.21}{16}=0.075$
$\mathrm{V}_{0.03} \mathrm{O}_{0.075}$
$\mathrm{V} \mathrm{O}_{2,5} \Rightarrow \mathrm{V}_{2} \mathrm{O}_{5}$

Asked in: JEE-TOPICTESTS-CHEMISTRY

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