Aqueous HCl reacts with MnO2(s) to form MnCl2(aq), Cl2(g), and H2O(l). What is the weight (in g) of Cl2 liberated when 8.7 g of MnO2(s) is reacted with excess aqueous HCl solution?
Q. Aqueous HCl reacts with MnO2(s) to form MnCl2(aq), Cl2(g), and H2O(l). What is the weight (in g) of Cl2 liberated when 8.7 g of MnO2(s) is reacted with excess aqueous HCl solution? (Given Molar mass in g mol⁻¹ Mn = 55, Cl = 35.5, O = 16, H = 1)
A. 14.2
B. 21.3
C. 7.1
D. 71
Correct Answer: C

Explanation

Balanced equation:

MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

Molar mass of MnO2:

= 55 + 2(16)

= 55 + 32

= 87 g mol⁻¹

Moles of MnO2 taken:

= 8.7 / 87

= 0.1 mol

From balanced equation:

1 mol MnO2 produces 1 mol Cl2

Therefore,

0.1 mol MnO2 produces 0.1 mol Cl2

Molar mass of Cl2:

= 2 × 35.5 = 71 g mol⁻¹

Mass of Cl2 formed:

= 0.1 × 71

= 7.1 g

Correct Option: C

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