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: \mathrm{Cr_2O_7^{2-}} + \mathrm{Fe^{2+}} \rightarrow \mathrm{Cr^{3+}} + \mathrm{Fe^{3+}}
Calculate the change in oxidation number of Fe in the reaction: \mathrm{Fe^{2+}} \rightarrow \mathrm{Fe^{3+}} + 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 \mathrm{OH^-} ions.
Explain why redox reactions are important in biological systems.
Identify the oxidizing agent in the following reaction: \mathrm{Fe^{2+}}(aq) + \mathrm{Cl_2}(g) \rightarrow \mathrm{Fe^{3+}}(aq) + 2\mathrm{Cl^-}(aq)
In the reaction \mathrm{MnO_4^-}(aq) + 8\mathrm{H^+}(aq) + 5\mathrm{Fe^{2+}}(aq) \rightarrow \mathrm{Mn^{2+}}(aq) + 5\mathrm{Fe^{3+}}(aq) + 4\mathrm{H_2O}(l), how many electrons are transferred per \mathrm{MnO_4^-} ion?
In the reaction \mathrm{Zn}(s) + \mathrm{CuSO_4}(aq) \rightarrow \mathrm{ZnSO_4}(aq) + \mathrm{Cu}(s), which species is oxidized?
In the reaction: 2\mathrm{Fe^{3+}}(aq) + 2\mathrm{I^-}(aq) \rightarrow 2\mathrm{Fe^{2+}}(aq) + \mathrm{I_2}(s), which species is reduced?
In the reaction: 2\mathrm{I^-}(aq) + \mathrm{Cl_2}(aq) \rightarrow 2\mathrm{Cl^-}(aq) + \mathrm{I_2}(s), which species is oxidized?
What is the oxidation state of carbon in \mathrm{CO_2}?
What is the oxidation state of chlorine in \mathrm{Cl_2O_7}?
What is the oxidation state of nitrogen in \mathrm{NO_3^-}?
What is the oxidation state of oxygen in \mathrm{H_2O_2}?
What is the oxidation state of sulfur in \mathrm{H_2SO_4}?
Which ion is reduced in the reaction: 2\mathrm{MnO_4^-} + 5\mathrm{C_2O_4^{2-}} + 16\mathrm{H^+} \rightarrow 2\mathrm{Mn^{2+}} + 10\mathrm{CO_2} + 8\mathrm{H_2O}?
