Question

Identify the substance oxidised and substance reduced in the following reactions-

(i) ZnO(s) + C(s) ---> Zn(s) + CO (g)

(ii) 2Na(s) + O2(g) ---> 2Na2O (s)

(iii) CuO(s) + H2(g) ---> Cu(s) + H2O (l)​

Answer 1

i)ZnO is reduced to Zn and C is oxidised to CO.
ii)Na is oxidised to Na2O and O2 is reduced.
iii) CuO is reduced to Cu and H2 is oxidised to H2O.

Answer 2

Oxidizing and reducing agents

Explanation:

ZnO(s)+C(s) → Zn(s)+CO(g)

Zinc oxide is reduced to zinc.

Carbon is oxidized to Carbon mono-oxide.

Cuo(s)+H₂(g) → Cu(s)+H₂O(l)

Copper oxide is reduced to Copper.

Hydrogen is oxidized to water.

2H₂S+SO₂ → 2H₂O+3S+

SO2 oxidizes hydrogen to water. SO2 is the oxidizing agent.

H2S reduces SO2 to S. So H2S is the reducing agent.

An oxidizing agent is a reactant that removes electrons from other reactants during a redox reaction; a reducing agent is an element that loses an electron to an electron recipient in a redox chemical reaction.

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