In the electrolysis of aqueous of NaOH, 2.8 litres of oxygen was liberated at the anode at NTP. How much hydrogen was liberated at the cathode?

5.6

litre

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56

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560

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0.056

litre

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Solution

The correct option is A $5.6$ litre
In electrolysis of $N a O H$ , $H_{2}$ liberate at cathode and $O_{2}$ at anode.

Since, $H_{2} O \to H_{2} + 1 / 2 O_{2}$

If $2.8$ litre $O_{2}$ is liberated the volume of hydrogen will be twice (as seen from stoichiometric reaction).

So, $5.6$ litre $H_{2}$ is obtained.

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