AP EAMCET · Chemistry · Electrochemistry

When a current of $10 A$ is passes through molten ${AlCl}_{3}$ for $1.608$ minutes. The mass of $Al$ deposited will be [Atomic mass of $Al = 27 g$ ]:-

A $0 .09 g$
B $0 .81 g$
C $1 .35 g$
D $0 .27 g$

Verified Solution

Answer & Solution

Correct Answer

(A) $0 .09 g$

Step-by-step Solution

Detailed explanation

Given data :- Current = 10 A. Time = 1.608 min=96.48 s Atomic mass of Al=27 g/mol Oxidation state of Al=+3 Mass of aluminium deposited = Atomic mass ×time×currentF×valency factor Mass of aluminium deposited =…

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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When a current of 10 A is passes through molten AlCl3 for 1.608 minutes. The mass of Al deposited will be [Atomic mass of Al=27 g]:-

Step-by-step Solution

When a current of $10 A$ is passes through molten ${AlCl}_{3}$ for $1.608$ minutes. The mass of $Al$ deposited will be [Atomic mass of $Al = 27 g$ ]:-