Which is the weight of A1 deposited at cathode when 1 ampere current is passed through molten…

Which is the weight of A1 deposited at cathode when 1 ampere current is passed through molten $\mathrm{AlCl}_3$ for 9650 seconds? (At mass of $\mathrm{Al}=27$ )
  1. 3.0 g
  2. 9.0 g
  3. 13.6 g
  4. 0.9 g

Solution

$\begin{aligned} & \text { Number of equivalents of } \mathrm{Al} \text { deposited }=\frac{\mathrm{I} . \mathrm{t}}{\mathrm{F}} \\ & =\frac{1 \times 9650}{96500}=0.1 \\ & \text { Number. Of equivalents }=\text { moles } \times \mathrm{n}_{\text {factor }} \\ & \stackrel{+3}{\mathrm{AlCl}_3 \longrightarrow \mathrm{Al}_{\text {factor }}=3} \\ & 0.1=\text { moles } \times 3 \\ & \text { moles of } \mathrm{Al}=0.1 / 3 \\ & \text { mass of } \mathrm{Al}=\frac{0.1}{3} \times 27=0.9 \mathrm{~g}\end{aligned}$

Asked in: MHT CET 2021 (24 Sep Shift 1)

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