JEE Mains · Chemistry · STD 12 - 2. Electrochemistry
A current of \(10.0\, A\) flows for \(2 .00\, h\) through an electrolytic cell containing a molten salt of metal \(X\). This results in the decomposition of \(0 .250\, mol\) of metal \(X\) at the cathode. The oxidation state of \(X\) in the molten salt is \((F = 96,500\, C\))
- A \(1+\)
- B \(2+\)
- C \(3+\)
- D \(4+\)
Answer & Solution
Correct Answer
(C) \(3+\)
Step-by-step Solution
Detailed explanation
According to Faraday's first law of electrolysis \(W\,=\,\frac {E\times i\times t}{96500}\) Where \(E\,=\) equivqlent weight \(=\,\frac {mol.\,mass\,of\,metal\,(M)}{oxidation\,state\,of\,metal(x)}\) Substituting the value in the formula \(W\,=\,\frac {M}{x}\) \(\times \)…
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