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NEET Chemistry Electrochemistry / विद्युत् रसायन Question Bank Self Evaluation Test - Electrochemistry

  • question_answer
    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 \[0.250\text{ }mol\] of metal X at the cathode. The oxidation state of X in the molten salt is: \[\left( F=96,500C \right)\]

    A) \[{{1}^{+}}\]                         

    B) \[{{2}^{+}}\]

    C) \[{{3}^{+}}\]                         

    D) \[{{4}^{+}}\]

    Correct Answer: C

    Solution :

    [c] According to Faraday's first law of electrolysis \[W=\frac{E\times i\times t}{96500}\] Where E = equivalent weight \[=\frac{mol.mass\,of\,metal(M)}{oxidation\text{ }state\text{ }of\text{ }metal\text{ }\left( x \right)}\] Substituting the value in the formula \[W=\frac{M}{x}\times \frac{i\times t}{96500}\] or \[x=\frac{M}{W}\times \frac{i\times t}{96500}=\frac{10\times 2\times 60\times 60}{96500\times 0.250}=3\]             \[\left[ Given:no.\text{ }of\text{ }moles=\frac{M}{W}=0.250 \right]\] Hence oxidation state of metal is (+3)


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