Join Our JEE Preparation Group
Prep with like-minded aspirants; Get access to free daily tests and study material.
Sign in
Please select an account to continue using cracku.in
↓ →
Join Our JEE Preparation Group
Prep with like-minded aspirants; Get access to free daily tests and study material.
A current of 10 A flows for 2 hours through an electrolytic cell containing a molten salt of metal X and results in the deposition of 0.25 moles of metal X at cathode. The oxidation state X in the electrolysed salt is ____ .
Correct Answer: 3
The charge passed is $$10 \times 7200 = 72000\text{ C}$$, which is $$\frac{72000}{96500} \approx 0.75$$ faraday. Depositing 0.25 mol of X needs $$\frac{0.75}{0.25} = 3$$ mol of electrons per mole of X. So the oxidation state of X is $$+3$$.
Was this solution helpful?
Predict your JEE Main percentile, rank & performance in seconds
Educational materials for JEE preparation
Ask our AI anything
AI can make mistakes. Please verify important information.
AI can make mistakes. Please verify important information.