A solution of Fe_(2)(SO_(4))_(3) is electrolyzed for 'x' min with a current of 1.5 A to deposit 0.3482 g of Fe. The value of x is ___________. [nearest integer] Given : 1 F = 96500 C mol^(-1) Atomic mass of Fe = 56 g mol^(-1)

Fe^3++3 e^- -> Fe Moles of Fe deposited =(0.3482 / 56)=6.2 x 10^-3 For 1 mole Fe, charge required is 3 F For 6.2 x 10^-3 mole Fe, charge required is 3 x 6.2 x 10^-3 F Since, charge required =18.6 x 10^-3 x 96500 C =1794.9 C And, 1.5 x t=1794.9 t=(1794.9 / 1.5 x 60) min t = 20 min

A solution of Fe2SO43 is electrolyzed for x min with a ... | null (Chemistry)

\mathrm{Fe}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe}

\text {Moles of Fe deposited }=\frac{0.3482}{56}=6.2 \times 10^{-3}

For 1 mole

\mathrm{Fe}

, charge required is

3 \mathrm{~F}

For

6.2 \times 10^{-3}

mole

\mathrm{Fe}

, charge required is

3 \times 6.2 \times 10^{-3} \mathrm{~F}

Since, charge required

=18.6 \times 10^{-3} \times 96500 \mathrm{C}

=1794.9 \mathrm{C}

And,

1.5 \times \mathrm{t}=1794.9

t=\frac{1794.9}{1.5 \times 60} \min

\mathrm{t} \simeq 20 \mathrm{~min}

Explanation

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