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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Balance the following redox reaction in acidic solution: Cr2O72- + Fe2+ → Cr3+ + Fe3+
Calculate the change in oxidation number of Fe in the reaction: Fe2+ → Fe3+ + e-
Describe the role of water in redox reactions in aqueous solutions.
Describe the steps to balance a redox reaction in acidic aqueous solution using the ion-electron method.
Explain why balancing redox reactions in basic solutions requires adding OH- ions.
Explain why redox reactions are important in biological systems.
Identify the oxidizing agent in the following reaction: Fe2+(aq) + Cl2(g) → Fe3+(aq) + 2Cl-(aq)
In the reaction MnO4-(aq) + 8H+(aq) + 5Fe2+(aq) → Mn2+(aq) + 5Fe3+(aq) + 4H2O(l), how many electrons are transferred per MnO4- ion?
In the reaction Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s), which species is oxidized?
In the reaction: 2Fe3+(aq) + 2I-(aq) → 2Fe2+(aq) + I2(s), which species is reduced?
In the reaction: 2I-(aq) + Cl2(aq) → 2Cl-(aq) + I2(s), which species is oxidized?
What is the oxidation state of carbon in CO2?
What is the oxidation state of chlorine in Cl2O7?
What is the oxidation state of nitrogen in NO3-?
What is the oxidation state of oxygen in H2O2?
What is the oxidation state of sulfur in H2SO4?
Which ion is reduced in the reaction: 2MnO4- + 5C2O42- + 16H+ → 2Mn2+ + 10CO2 + 8H2O?
