So the full equation is...
2Cl- + Zn2+ ---> Zn + Cl2
I'm just going to confirm if I'm right.
I said that Cl- is the oxidant that loses the electron to oxidise Zn. And Zn is the reductant that gains the electron lost by the Cl?
Am I right, if I'm not please point it out and tell me the correct answer in detail
Thank you
Chemistry question on half equations and oxidant and reductant?
2017-02-08 1:42 pm
回答 (3)
2017-02-08 2:33 pm
There is no reaction between Cl⁻ ion and Zn²⁺ ion. In contrast, ZnCl₂ is a stable compound. This is because Cl⁻ is a weaker reducing agent than Zn metal, and Zn²⁺ is a weaker oxidizing agent than Cl₂.
Actually, the backward reaction occurs, i.e.
Zn + Cl₂ → Zn²⁺ + 2Cl⁻
Zn acts as a reducing agent, which is oxidized to Zn²⁺ ion. The half equation is :
Zn → Zn²⁺ + 2e⁻
Cl₂ acts as an oxidizing agent, which is reduced to Cl⁻ ion. The half equation is :
Cl₂ + 2e⁻ → 2Cl⁻
Actually, the backward reaction occurs, i.e.
Zn + Cl₂ → Zn²⁺ + 2Cl⁻
Zn acts as a reducing agent, which is oxidized to Zn²⁺ ion. The half equation is :
Zn → Zn²⁺ + 2e⁻
Cl₂ acts as an oxidizing agent, which is reduced to Cl⁻ ion. The half equation is :
Cl₂ + 2e⁻ → 2Cl⁻
2017-02-08 2:05 pm
Oxidant = Oxidising agent
Reductant = Reducing agent
Cl⁻ is oxidised to Cl₂ so it is a reducing AGENT / reductant
Zn²⁺ is reduced to Zn ; so it is an oxidising AGENT / oxidant
So, Cl⁻ is reductant which reduces Zn²⁺ to Zn
Reductant = Reducing agent
Cl⁻ is oxidised to Cl₂ so it is a reducing AGENT / reductant
Zn²⁺ is reduced to Zn ; so it is an oxidising AGENT / oxidant
So, Cl⁻ is reductant which reduces Zn²⁺ to Zn
2017-02-08 1:49 pm
2Cl- oxidizes Cl2
Zn2+ reduces Zn
Zn2+ reduces Zn
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