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Oxidizing and reducing agents

Chemistry • Oxidation–Reduction Reactions • Knowledge-Based • 5 questions

Oxidizing and reducing agents Knowledge-Based Download PDF

Chemistry · Redox & Electrochemistry · Chemistry · Oxidation–Reduction Reactions

5 Chemistry practice questions on Oxidizing and reducing agents. Questions that assess core concepts and understanding.

Questions

  1. 1.

    Which statement correctly describes the function of an oxidizing agent in an oxidation–reduction reaction?

    • A) It gains electrons from another substance, causing that substance to be oxidized while its own oxidation state decreases.
    • B) It loses electrons to another substance, causing that substance to be oxidized while its own oxidation state increases.
    • C) It donates electrons to another substance, causing that substance to be reduced while its own oxidation state decreases.
    • D) It accepts electrons from another substance, causing that substance to be reduced while its own oxidation state increases.
  2. 2.

    In the redox reaction represented by the equation CuO(s)+H2(g)→Cu(s)+H2O(l)\text{CuO}(s) + \text{H}_2(g) \rightarrow \text{Cu}(s) + \text{H}_2\text{O}(l), which substance acts as the oxidizing agent?

    • A) H2(g)\text{H}_2(g)
    • B) Cu(s)\text{Cu}(s)
    • C) CuO(s)\text{CuO}(s)
    • D) H2O(l)\text{H}_2\text{O}(l)
  3. 3.

    In the redox reaction represented by the equation MnO2(s)+4HCl(aq)→MnCl2(aq)+Cl2(g)+2H2O(l)\text{MnO}_2(s) + 4\text{HCl}(aq) \rightarrow \text{MnCl}_2(aq) + \text{Cl}_2(g) + 2\text{H}_2\text{O}(l), which substance acts as the reducing agent?

    • A) MnO2\text{MnO}_2
    • B) HCl\text{HCl}
    • C) MnCl2\text{MnCl}_2
    • D) Cl2\text{Cl}_2
  4. 4.

    In the redox reaction represented by the equation Cl2(g)+2Br−(aq)→2Cl−(aq)+Br2(aq)\text{Cl}_2(g) + 2\text{Br}^-(aq) \rightarrow 2\text{Cl}^-(aq) + \text{Br}_2(aq), which species acts as the oxidizing agent?

    • A) Br−(aq)\text{Br}^-(aq)
    • B) Cl2(g)\text{Cl}_2(g)
    • C) Cl−(aq)\text{Cl}^-(aq)
    • D) Br2(aq)\text{Br}_2(aq)
  5. 5.

    In the redox reaction represented by the equation 2Fe3+(aq)+Sn2+(aq)→2Fe2+(aq)+Sn4+(aq)2\text{Fe}^{3+}(aq) + \text{Sn}^{2+}(aq) \rightarrow 2\text{Fe}^{2+}(aq) + \text{Sn}^{4+}(aq), which species acts as the reducing agent, and what change does it undergo?

    • A) Fe3+\text{Fe}^{3+}, because it undergoes reduction
    • B) Fe3+\text{Fe}^{3+}, because it undergoes oxidation
    • C) Sn2+\text{Sn}^{2+}, because it undergoes oxidation
    • D) Sn2+\text{Sn}^{2+}, because it undergoes reduction