Question

Chlorine is prepared in the laboratory by treating manganese dioxide (MnO2 ) with aqueous hydrochloric acid according to the reaction 4 HCl (aq) + MnO2 (s) → 2H2O (l) + MnCl2 (aq) + Cl2 (g) what mass of 95% pure MnO2 is required for the production 1kg of cl2

Answer 1

Answer:

Explanation:

The reaction for production of Chlorine is:

4 HCl (aq) + MnO2 (s) → 2H2O (l) + MnCl2 (aq) + Cl2 (g)

Molar mass of Cl₂ = 2 x 35.5 = 71 g/mol

Molar mass of MnO₂ = 55 + 2 x 16 = 87 g/mol

From the reaction,

1 mole of chlorine is produced by 1 mole of MnO₂

⇒71 g of chlorine is produced by 87 g of MnO₂

⇒0.071 kg of chlorine is produced by 0.087 kg of MnO₂

⇒1 Kg of chlorine is produced by 0.087/0.071 Kg of MnO₂

                                                    = 1.22 kg of MnO₂

Since the sample is 95% is pure,

Mass of MnO₂ required = 1.22/0.95 = 1.29 Kg