Redox reaction is also known as an oxidation-reduction reaction. It involves the transfer of electrons between two species. The loss of electrons is called oxidation and the gain of electrons is called reduction. There are mainly three types of redox reactions, combustion, disproportionation and single replacement. Redox reactions are widely used in the industries, e.g. pharmaceutical, metallurgical, agricultural, etc.
1. Which of the compounds can exist together?
(a) HgCl2, SnCl2
(b) FeCl3, KI
(c) FeCl3, SnCl2
(d) FeCl2, SnCl2
2. One mole of ferrous oxalate requires____ moles of MnO4– to get oxidised completely in an acidic medium
(a) 0.6 moles
(b) 0.4 moles
(c) 0.2 moles
(d) 7.5 moles
3. H2O2 changes Cr2O72- ion to CrO5 in an acidic medium, oxidation state of Cr in CrO5 is
4. H2SO4 acts as a strong oxidising agent. In which of the reaction, is it not acting as an oxidising agent?
(a) C + 2H2SO4 → CO2 + 2SO2 + 2H2O
(b) CaF2 + 2H2SO4 → CaSO4 + 2HF
(c) S + 2H2SO4 → 3SO2 + H2O
(d) Cu + 2H2SO4 → CuSO4 + SO2 + 2H2O
5. During a reaction of oxalic acid, potassium chlorate and sulphuric acid, the oxidation number of which of the element undergoes a maximum change
6. Find the redox reaction
(a) In atmosphere, O3 from O2 by lighting
(b) Reaction of H2SO4 with NaOH
(c) Both oxidation and reduction reaction
(d) Evaporation of water
7. Find the oxidation state of I in H4IO6–
8. In which of the following complex, the oxidation number of Fe is +1?
9. Which among the following compounds is the most reducing compound?
10. Which among the following is the strongest oxidising agent?