Question

If 10g of V₂O₅ is dissolved in acid and is reduced to V²⁺ by zinc metal, how many mole I₂ could be reduced by the resulting solution if it is further oxidised to VO²⁺ions?

A. 0.11 mole of I₂
B. 0.22 mole of I₂
C. 0.055 mole of I₂
D. 0.44 mole of I₂

Answer 1

10 grams of V2O5 equates to 0.055 moles, which upon reduction yield 0.110 moles of V2+. These moles of V2+ can further reduce an equal number of moles of I2 upon oxidation to VO2+, resulting in 0.22 moles of I2 being reduced. Option B is the correct answer.

Step-by-step explanation:

The question concerns the redox reaction involving the reduction of V2O5 by zinc metal and the subsequent oxidation reaction where V2+ is further oxidized to VO2+ ions. To answer this, we must first understand the stoichiometry of these reactions and determine the molar amounts involved.

Using the molecular weight of V2O5 (181.88 g/mol), we find that 10 g of V2O5 corresponds to 0.055 mol of V2O5. Each mole of V2O5 reduces to 2 moles of V2+, hence 0.055 mol of V2O5 gives 0.110 mol V2+. Each mole of V2+ can reduce one mole of I2 when oxidized to VO2+. As a result, 0.110 mol of V2+ can reduce 0.110 mol of I2.

The correct answer to the question is B. 0.22 mole of I2 could be reduced by the resulting solution if it is further oxidised to VO2+ ions.