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Oxidizing Agents and Reducing Agents

Chemistry ⇒ Redox Reactions and Electrochemistry

Oxidizing Agents and Reducing Agents starts at 10 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Oxidizing Agents and Reducing Agents. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 12
Describe the change in oxidation number for the oxidizing agent during a redox reaction.
Describe the change in oxidation number for the reducing agent during a redox reaction.
Explain why alkali metals are good reducing agents.
Explain why halogens are good oxidizing agents.
Explain why hydrogen peroxide (H2O2) can act as both an oxidizing agent and a reducing agent.
Explain why transition metals can act as both oxidizing and reducing agents.
Identify the reducing agent in the following reaction: 2Na + Cl2 → 2NaCl
In the reaction: 2Al + 3CuSO4 → Al2(SO4)3 + 3Cu, which element is reduced?
In the reaction: 2H2O2 → 2H2O + O2, which species is reduced?
In the reaction: C + O2 → CO2, identify the oxidizing agent and the reducing agent.
Name one strong oxidizing agent commonly used in laboratory redox titrations.
A student mixes aqueous solutions of potassium permanganate (KMnO4) and hydrogen peroxide (H2O2) under acidic conditions. Identify which substance acts as the oxidizing agent and which acts as the reducing agent. Write the balanced redox equation for the reaction.
Arrange the following species in order of increasing reducing strength: Zn, Mg, Al, Na. Justify your answer based on their standard electrode potentials.
Consider the following redox reaction: Cr2O72- + 6Fe2+ + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O Which species is reduced and which is oxidized?
Explain, with reference to electron transfer, why a reducing agent is always found on the reactant side of a redox equation.
Given the following standard reduction potentials at 25 °C: Fe3+ + e- → Fe2+ E0 = +0.77 V Sn4+ + 2e- → Sn2+ E0 = +0.15 V Which ion, Fe3+ or Sn4+, is the stronger oxidizing agent? Justify your answer.
In the reaction between nitric acid (HNO3) and copper metal, copper is oxidized to Cu2+ and nitrogen is reduced to NO. Write the half-reactions for oxidation and reduction, and identify the oxidizing and reducing agents.