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 salt is
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- +1
- +2
- +3
- +4
The Correct Option is C
Solution and Explanation
Step 1: Use the formula for electrolysis.
The number of moles of metal deposited is \( \text{moles} = \frac{\text{mass}}{\text{atomic weight}} \). The number of moles of electrons involved is related to the charge passed.
Step 2: Calculate the oxidation state.
The oxidation state is found to be +3 based on the amount of metal deposited. Final Answer: \[ \boxed{+3} \]
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