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Charge and Current

Calculate the...

Question

Calculate the number of coulombs required to deposit $5.4 g$ of $A l$ , when the electrode reaction is ${A l}^{3 +} + 3 e^{-} \to A l$
(At.mass of $A l = 27, F = 96500$ coulomb per mole)

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Solution

${A l}^{3 +} + 3 e^{-} \to A l$
$3 m o l e^{-} \to 27 g$ of $A l$
$5.4 g \to \frac{3}{27} \times 5.4 = 0.6 m o l o f e^{-}$
no. of $F = \frac{Q}{96500} = 0.6$
$Q = 0.6 \times 96500 = 57900 C$

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