Calculate the volume of oxygen produced (measured at standard temperature and pressure - STP) at the...

Calculate the volume of oxygen produced (measured at standard temperature and pressure - STP) at the anode during the electrolysis of sodium sulfate solution, if the electrolytic cell is operated at a current of 2.50 amperes for 45 minutes.

F = 9.65 x 104 C mol-1 (or 96,500 C mol-1). The molar volume of a gas at STP = 22.4 L mol-1 the two possible reactions at the anode are;

O2(g) + 2H2O(l) + 4e- 4OH-(aq) E = 0.40V

SO42- (aq) + 4H+(aq) + 2e- 2H2SO3(aq) + H2O(l) E = 0.20V

Expert Solution

Using Faraday's law

Mass =ZQ

Mass = Mit/nF

Mole = it/nF

=2.5×45×60/4×96500

Mole = 0.0175 mol

Volume produced = 0.0175×22.4

= 0.392 L

queen_honey_blossom answered 2 years ago

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