Redox Reactions in Aqueous Solutions
Chemistry ⇒ Redox Reactions and Electrochemistry
Redox Reactions in Aqueous Solutions starts at 10 and continues till grade 12.
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See sample questions for grade 11
Assign the oxidation number to sulfur in H2SO4.
Balance the following redox reaction in acidic solution: MnO4- + Fe2+ → Mn2+ + Fe3+
Balance the following redox reaction in basic solution: ClO- → Cl- + ClO3-
Calculate the change in oxidation number of nitrogen in the reaction: NO3- → NO.
Calculate the oxidation number of chromium in Cr2O72-.
Context: In an experiment, a student mixes potassium iodide (KI) solution with chlorine water (Cl2 in H2O) and observes a color change. Question: Which element is reduced in this reaction?
Describe the steps involved in balancing a redox reaction in basic solution.
Explain why the reaction between hydrogen and oxygen to form water is considered a redox reaction.
Explain why water can act as both an oxidizing and a reducing agent in redox reactions in aqueous solutions.
Given the reaction: 2H2O(l) → 2H2(g) + O2(g), what is the oxidizing agent?
In the context of redox reactions in aqueous solutions, what is meant by a disproportionation reaction?
In the reaction: 2Al(s) + 3CuSO4(aq) → Al2(SO4)3(aq) + 3Cu(s), how many electrons are transferred per formula unit of Al2(SO4)3 formed?
In the reaction: 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g), what is the change in oxidation number of sodium?
In the reaction: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s), which species is oxidized?
Balance the following redox reaction in acidic solution and identify the number of electrons transferred per mole of dichromate ion: Cr2O72- + C2O42- → Cr3+ + CO2
Calculate the number of moles of electrons transferred when 0.25 mol of I- is oxidized to I2 in aqueous solution.
Context: A solution contains both Fe2+ and Fe3+ ions. When potassium permanganate (KMnO4) is added in acidic medium, a color change is observed.
Question: Explain the redox changes that occur and identify which species is oxidized and which is reduced.
Determine the oxidation number of each element in the ion [Fe(CN)6]4-.
Explain why the addition of a strong acid can increase the rate of certain redox reactions in aqueous solution.
