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 difference between an oxidizing agent and a reducing agent.
Explain why chlorine gas acts as an oxidizing agent when it reacts with sodium.
Explain why metals are often good reducing agents.
Explain why potassium permanganate is considered a strong oxidizing agent.
Identify the oxidizing agent in the following reaction: 2Na + Cl2 → 2NaCl
In the reaction 2Al + 3CuSO4 → Al2(SO4)3 + 3Cu, identify the oxidizing agent.
In the reaction 2H2O2 → 2H2O + O2, what role does H2O2 play?
In the reaction 2K + Br2 → 2KBr, which substance is oxidized?
In the reaction 2Mg + O2 → 2MgO, which element is reduced?
In the reaction Fe2+ + Cl2 → Fe3+ + 2Cl-, which species is the reducing agent?
A student mixes zinc metal with a solution of copper(II) sulfate. After some time, copper metal is deposited and the blue color of the solution fades. Explain which substance acts as the reducing agent and why.
Consider the following reaction:
MnO4- + 8H+ + 5Fe2+ → Mn2+ + 5Fe3+ + 4H2O
Calculate the change in oxidation state for manganese and iron, and identify which is oxidized and which is reduced.
Consider the following redox reaction:
Cr2O72- + 6Fe2+ + 14H+ → 2Cr3+ + 6Fe3+ + 7H2O
Identify the oxidizing agent in this reaction and explain your reasoning.
In the reaction between hydrogen sulfide (H2S) and chlorine gas (Cl2):
H2S + Cl2 → 2HCl + S
Which substance is reduced, and which is oxidized?
