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Aqueous HCl reacts with MnO ₂( ~s ) to form MnCl ₂( aq ), Cl ₂( ~g ) and H ₂ O (l) . What is the weight (in g) of Cl ₂ liberated when 8.7 g of MnO ₂( ~s ) is reacted with excess aqueous HCl solution? (Given Molar mass in g mol ⁻¹ Mn =55, Cl =35.5, O =16, H =1 )

Options

  1. A21.3
  2. B71
  3. C14.2
  4. D7.1

Correct answer

D. 7.1

Step-by-step solution

The balanced redox equation is: MnO ₂ + 4 HCl MnCl ₂ + Cl ₂ + 2 H ₂ O . Molar mass of MnO₂ = 55 + 32 = 87 g/mol. Moles of MnO₂ = 8.7 87 = 0.1 mol. From stoichiometry, 1 mol MnO₂ produces 1 mol Cl₂, so 0.1 mol produces 0.1 mol Cl₂. Mass of Cl₂ = 0.1 71 = 7.1 g.

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