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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Assign oxidation numbers to all elements in the compound H2SO4.
Balance the following redox reaction in acidic solution: Fe2+ + Cr2O72- → Fe3+ + Cr3+
Calculate the change in oxidation number of sulfur in the reaction: SO2 + 2H2O2 → H2SO4 + H2O
Calculate the number of electrons transferred when 2 moles of Fe2+ are oxidized to Fe3+.
Calculate the number of moles of electrons required to reduce 1 mole of MnO4- to Mn2+ in acidic solution.
Describe the role of water as a reactant or product in redox reactions in aqueous solutions.
Describe the steps involved in balancing a redox reaction in basic aqueous solution.
Explain why potassium permanganate (KMnO4) is a strong oxidizing agent in acidic aqueous solution.
Explain why the oxidation number of chlorine in ClO4- is +7.
In the context of redox reactions in aqueous solutions, what is meant by a disproportionation reaction?
In the reaction: 2H2O2(aq) → 2H2O(l) + O2(g), which element undergoes both oxidation and reduction?
In the reaction: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s), which species is oxidized?
State the oxidation number of chromium in Cr2O72-.
State the oxidation number of nitrogen in NO3-.
Write the balanced half-reaction for the oxidation of Fe2+ to Fe3+ in aqueous solution.
