i) H2 + Cl2 ——> 2Hcl

ii) BaCl2 + NaSo4——->BaSo4 +2NaCl

iii) Zn + CuSo4——-> ZnSo4 + Cu

Vi) 2Kclo3I2——->2KIO3 + Cl2


BaCl2 + NaSo4——->BaSo4 +2NaCl


H2 + Cl2 → 2HCl is an oxidation-reduction (redox) reaction.

Oxidation: Hydrogen atoms in H2 lose electrons and become oxidized to H+
Reduction: Chlorine atoms in Cl2 gain electrons and become reduced to Cl-

(BaCl_{2}(aq)+Na_{2}SO_{4}(aq)\rightarrow BaSO_{4}(s)+2NaCl(aq)\) is not a redox reaction because there is no change in oxidation state. This is because there is no formal electron transfer. The reaction is driven by the insolubility of the barium sulfate salt

Reaction Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s) is a redox reaction. In a redox reaction, both oxidation and reduction occur at the same time. In this reaction, zinc is oxidized and copper is reduced.

2KClO3: The oxidizing agent, with an oxidation number of +5 for chlorine
I2: The reducing agent, as iodine is undergoing oxidation.

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