ZnS NO3- -----> Zn2 S NO
Also...
Which element got oxidized and which got reduced?
Which species was the oxidizing agent and which was the reducing agent?
Complete and balance the equation for this reaction in acidic solution....?
2016-06-13 6:41 am
回答 (1)
2016-06-13 9:12 am
Oxidation half equation: ZnS(s) + 2e⁻ → Zn²⁺(aq) + S(s) ...... [1]
Reduction half equation: NO₃⁻(aq) + 4H⁺(aq) + 3e⁻ → NO(g) + 2H₂O(l) ...... [2]
[1]×3 + [2]×2, and cancel 6e⁻ on the both sides :
3ZnS(s) + 2NO₃⁻(aq) + 8H⁺(aq) → 3Zn²⁺(aq) + 3S(s) + 2NO(g) + 4H₂O(l)
The element S was oxidized as the oxidation number of S increases from -2 (in ZnS) to 0 (in S).
The element N was reduced as the oxidation number of N decreases from +5 (in NO₃⁻) to +2(in NO).
The reducing agent is oxidized, while the oxidizing agent is reduced.
Hence, the oxidizing agent is NO₃⁻, while the reducing agent is ZnS.
Reduction half equation: NO₃⁻(aq) + 4H⁺(aq) + 3e⁻ → NO(g) + 2H₂O(l) ...... [2]
[1]×3 + [2]×2, and cancel 6e⁻ on the both sides :
3ZnS(s) + 2NO₃⁻(aq) + 8H⁺(aq) → 3Zn²⁺(aq) + 3S(s) + 2NO(g) + 4H₂O(l)
The element S was oxidized as the oxidation number of S increases from -2 (in ZnS) to 0 (in S).
The element N was reduced as the oxidation number of N decreases from +5 (in NO₃⁻) to +2(in NO).
The reducing agent is oxidized, while the oxidizing agent is reduced.
Hence, the oxidizing agent is NO₃⁻, while the reducing agent is ZnS.
收錄日期: 2021-04-18 14:59:51
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