MHT CET · Chemistry · Electrochemistry

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 \(\mathrm{Al}=27\) )

A 3.0 g
B 9.0 g
C 13.6 g
D 0.9 g

Verified Solution

Answer & Solution

Correct Answer

(D) 0.9 g

Step-by-step Solution

Detailed explanation

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

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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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 \(\mathrm{Al}=27\) )

Step-by-step Solution

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 \(\mathrm{Al}=27\) )