Question:
A current of $2.0\, A$ passed for $5$ hours through a molten metal salt deposits $22.2\, g$ of metal (At wt. = $177$). The oxidation state of the metal in the metal salt is
A current of $2.0\, A$ passed for $5$ hours through a molten metal salt deposits $22.2\, g$ of metal (At wt. = $177$). The oxidation state of the metal in the metal salt is
Updated On: Jul 13, 2024
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The Correct Option is C
Solution and Explanation
Weight $=\frac{E \times i \times t}{F}=\frac{\text { M it }}{n-\text { factor } \times F} \mid E=\frac{M}{n-\text { factor }}$
$\Rightarrow 22.2=\frac{177 \times 5 \times 2 \times 60 \times 60}{ n -\text { factor } \times 96500}$
$\therefore n -$ factor $=2.97 \simeq 3$
Hence oxidation state of metal $=+3$
$\Rightarrow 22.2=\frac{177 \times 5 \times 2 \times 60 \times 60}{ n -\text { factor } \times 96500}$
$\therefore n -$ factor $=2.97 \simeq 3$
Hence oxidation state of metal $=+3$
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Concepts Used:
Electrolysis
Electrolysis:
Electrolysis is the process by which an element is decomposed and undergoes some chemical change under the influence of any electric current. The first-ever electrolysis was executed out by Sir Humphrey Davey in the year 1808. Electrolysis can occur in both Galvanic cells and Electrolytic cells.
Applications of Electrolysis:
- Electrolytic cells are used for the production of Hydrogen and Oxygen gas from water.
- They are used for the large-scale production of pure metals like sodium, copper, magnesium, etc.
- They are used to extract Aluminium from Bauxite.
- Electrolytic cells are used for electroplating, a process by which a thin protective layer of one metal is formed over another metal, mostly for protection.
- Electrolysis is used for the electrorefining of non-ferrous metals.
Read More: Products of Electrolysis