Question:
Identify correct statement for reaction stated below.
\[ \mathrm{Ag}_2 \mathrm{O}+\mathrm{H}_2 \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Ag}+2 \mathrm{OH}^{-} \]
Identify correct statement for reaction stated below.
\[ \mathrm{Ag}_2 \mathrm{O}+\mathrm{H}_2 \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Ag}+2 \mathrm{OH}^{-} \]
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Track the change in oxidation number of silver in the given reduction half reaction.
Updated On: Nov 13, 2026
- Water is oxidised.
- Hydrogen is oxidised.
- Silver is reduced.
- Hydrogen is reduced.
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The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept
Gain of electrons is reduction, and the oxidation number falls.
Step 2: Oxidation Numbers
In \(\text{Ag}_2\text{O}\) silver is \(+1\); in \(\text{Ag}\) it is \(0\).
So silver gains one electron per atom.
Step 3: Conclusion
Silver is reduced. Hydrogen and oxygen of water remain at \(+1\) and \(-2\) in \(\text{OH}^{-}\), so water is neither oxidised nor reduced.
Final Answer:
Silver is reduced. \[ \boxed{\text{(C) }\text{Silver is reduced.}} \]
Gain of electrons is reduction, and the oxidation number falls.
Step 2: Oxidation Numbers
In \(\text{Ag}_2\text{O}\) silver is \(+1\); in \(\text{Ag}\) it is \(0\).
So silver gains one electron per atom.
Step 3: Conclusion
Silver is reduced. Hydrogen and oxygen of water remain at \(+1\) and \(-2\) in \(\text{OH}^{-}\), so water is neither oxidised nor reduced.
Final Answer:
Silver is reduced. \[ \boxed{\text{(C) }\text{Silver is reduced.}} \]
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