Question

What volume of gases at STP will evolve if 1 L of
0.01 M solution of H2SO4 is electrolysed?
(1) 33.6 L
(2) 336 ml
(3) 3.36 ml
(4) 3.36 L
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Answer 1

The solution is in the pic attached above.

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Answer 2

Answer: The volume of gases evolved at STP is 33.6 L

Explanation:

The half reactions for the electrolysis of $H_2SO_4$ follows:

Oxidation half reaction:  $H_2O\rightarrow 2H^++\frac{1}{2}O_2+2e^-$  

Reduction half reaction:  $2H^++2e^-\rightarrow H_2$

The gases that are formed by the electrolysis of sulfuric acid are hydrogen and oxygen gas

Moles of hydrogen gas produced = 1 mole

Moles of oxygen gas produced = 0.5 mole

Total moles of gases produced = 1 + 0.5 = 1.5 moles

When 2 Faradays of charge (this means that 2 electrons are exchanged) is passed, the moles of gases produced are 1.5 moles.

STP conditions:

1 mole of a gas occupies 22.4 L of volume  

So, 1.5 moles of gas will occupy = $\frac{22.4}{1}\times 1.5=33.6L$ of volume  

Hence, the volume of gases evolved at STP is 33.6 L