Oxidizing Agents and Reducing Agents
Chemistry ⇒ Redox Reactions and Electrochemistry
Oxidizing Agents and Reducing Agents starts at 10 and continues till grade 12.
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Describe the role of hydrogen peroxide (H2O2) in redox reactions.
Explain why fluorine (F2) is the strongest oxidizing agent among the halogens.
Explain why potassium permanganate (KMnO4) is considered a strong oxidizing agent.
Identify the reducing agent in the following reaction: 2Na + Cl2 → 2NaCl
In the reaction 2H2 + O2 → 2H2O, identify the oxidizing agent.
In the reaction Fe2+ + Cl2 → Fe3+ + 2Cl-, which species is reduced?
In the reaction: 2Al + 3CuSO4 → Al2(SO4)3 + 3Cu, which element is reduced?
In the reaction: 2K + Br2 → 2KBr, which element is oxidized?
In the reaction: 2Na + 2H2O → 2NaOH + H2, which substance is the oxidizing agent?
Arrange the following species in order of increasing oxidizing strength: Br2, Cl2, I2.
Consider the following redox reaction: Cr2O72- + 6Fe2+ + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O. Identify the oxidizing agent and justify your answer based on changes in oxidation states.
Explain, with reference to electron transfer, why a reducing agent is itself oxidized in a redox reaction.
Given the standard reduction potentials: Ag+/Ag = +0.80 V, Cu2+/Cu = +0.34 V, Zn2+/Zn = -0.76 V, which metal is the strongest reducing agent?
In the reaction between hydrogen sulfide (H2S) and chlorine gas (Cl2): H2S + Cl2 → 2HCl + S, which substance is oxidized and which is reduced?
