Question

H2O2 is oxidised by MnO4- in acidic medium
to form O2 and Mn2+. How many grams of O2
are produced from 1.5 x 10-3 moles of MnO4-
and 1.2 milligrams of H2O2 :-
​

Answer 1

hence , mass of O2 is 1.1294 miligrams.

balanced chemical reaction is

2MnO4^- + 5H2O2 + 6H^+ ⇔ 2Mn^2+ + 8H2O + 5O2

here it is clear that, 2 moles of MnO4^- is reacting with 5 moles of H2O2.

or, 1.5 × 10^-4 mol of MnO4^- will react with (5/2) × 1.5 × 10^-3 = 3.75 × 10^-3 mol of H2O2.

but given mass of H2O2 = 1.2 × 10^-3 g

molecular mass of H2O2 = 34g

so, mol of H2O2 = 1.2 × 10^-3/34 < 3.75 × 10^-3

hence, H2O2 is limiting reagent.

now, from equation,

5 moles of H2O2 is producing 5 moles of O2.

so, 1.2 × 10^-3/34 mol of H2O2 will produce 1.2 × 10^-3/34 mol of O2.

so, mass of O2 = 1.2 × 10^-3/34 × molecular mass of O2

= 1.2 × 10^-3/34 × 32

= 1.1294 miligrams

hence , mass of O2 is 1.1294 miligrams.

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