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Chemistry

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

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Answer

2H2O⟶2H2 +O22(2+16)2(16)36g32g\begin{matrix} 2\text{H}2\text{O} & \longrightarrow 2\text{H}2 \space + & \text{O}_2 \ 2(2 + 16) & & 2(16) \ 36 \text{g} & & 32 \text{g} \ \end{matrix}

36 g of water produces 32 g of O2

∴ 18 g of water will produced

= 3236\dfrac{32}{36} x 18 = 16 g of O2

2H2O⟶2H2 +O22 mole1 mole\begin{matrix} 2\text{H}2\text{O} & \longrightarrow 2\text{H}2 \space + & \text{O}_2 \ 2\text{ mole} & & 1\text{ mole} \ \end{matrix}

2 moles of water produces 1 mole of oxygen

∴ 1 mole of water will produce 12×1\dfrac{1}{2} \times 1 = 0.5 moles of O2

1 mole of O2 occupies 22.4 L volume

∴ 0.5 moles will occupy = 22.4 × 0.5

= 11.2 L

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