Physical Chemistry - Redox Reactions

⏱ Time: 0s

Q1. In the reaction 2Fe²⁺ + Cl2 → 2Fe³⁺ + 2Cl⁻, which element is oxidized? (2021)

Solution:

Iron (Fe) is oxidized from +2 to +3 oxidation state in this reaction.

⏱ Time: 0s

Q2. In the electrochemical series, which element is the best reducing agent? (2022)

Solution:

Li is the best reducing agent among the given alkali metals due to its low ionization energy.

⏱ Time: 0s

Q3. What is the product of the reduction of Cr2O7²⁻ in acidic medium? (2019)

Solution:

In acidic medium, Cr2O7²⁻ is reduced to Cr³⁺.

⏱ Time: 0s

Q4. In the reaction 2Fe2O3 + 3C → 4Fe + 3CO2, which species is oxidized? (2019)

Solution:

In this reaction, carbon (C) is oxidized as it loses electrons to form CO2.

⏱ Time: 0s

Q5. In a redox reaction, if the oxidation state of an element increases, what happens to that element? (2021)

Solution:

An increase in the oxidation state of an element indicates that it has lost electrons, which means it is oxidized.

⏱ Time: 0s

Q6. Which of the following species can act as an oxidizing agent? (2023)

Solution:

MnO4- is a strong oxidizing agent because it can gain electrons and be reduced to Mn2+.

⏱ Time: 0s

Q7. In the electrochemical series, which of the following has the highest reduction potential? (2022)

Solution:

Fluorine (F+) has the highest reduction potential in the electrochemical series, indicating it is a strong oxidizing agent.

⏱ Time: 0s

Q8. Which of the following is the oxidizing agent in the reaction: 2MnO4⁻ + 5C2O4²⁻ + 6H⁺ → 2Mn²⁺ + 10CO2 + 3H2O? (2022)

Solution:

In this reaction, MnO4⁻ is reduced to Mn²⁺, thus it acts as the oxidizing agent.

⏱ Time: 0s

Q9. Which of the following reactions is an example of a disproportionation reaction? (2023)

Solution:

In the reaction 2H2O2 → 2H2O + O2, the oxidation state of oxygen changes from -1 in H2O2 to 0 in O2, indicating that it is both oxidized and reduced.

⏱ Time: 0s

Q10. In a redox reaction, what happens to the oxidation state of the reducing agent? (2021)

Solution:

The oxidation state of the reducing agent decreases as it loses electrons during the reaction.