Calculate the mass and volume of oxygen at STP, which will be evolved on electrolysis of 1 mole (18g) of water.

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Solution

Electrolysis of water will break it down in its component as Hydrogen and Oxygen
Balanced chemical reaction:
$2 H_{2} O ⟶ 2 H_{2} + O_{2}$
From the above equation,2 moles of water will evolve 1 mole of oxygen gas upon electrolysis. Therefore 1 mole of water will produce mole of Oxygen.
Mass of Oxygen evolved = number of moles of Oxygen evolved $\times$ Molecular wt. of Oxygen
= $\times$ 32 = 16 g
At STP 1 mole of any gas will occupy 22.4L volume.
Volume of Oxygen evolved = no.of moles $\times$ 22.4L
= $\times$ 22.4L = 11.2L

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