Multiple Choice
Which of the following is the correctly balanced redox reaction for MnO4⁻(aq) + Br⁻(aq) → MnO2(s) + BrO3⁻(aq) in a basic solution?
6. Chemical Quantities & Aqueous Reactions
Balancing Redox Reactions: Basic Solutions
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What is the balanced equation for the redox reaction in a basic solution: Fe^{2+}(aq) + N_2(g) -> Fe^{3+}(aq) + N_2H_4(aq)?
A
3 Fe^{2+}(aq) + N_2(g) + 6 OH^-(aq) -> 3 Fe^{3+}(aq) + N_2H_4(aq) + 3 H_2O(l)
B
2 Fe^{2+}(aq) + N_2(g) + 4 OH^-(aq) -> 2 Fe^{3+}(aq) + N_2H_4(aq) + 2 H_2O(l)
C
Fe^{2+}(aq) + N_2(g) + 2 OH^-(aq) -> Fe^{3+}(aq) + N_2H_4(aq) + H_2O(l)
D
Fe^{2+}(aq) + N_2(g) + 4 OH^-(aq) -> Fe^{3+}(aq) + N_2H_4(aq) + 2 H_2O(l)
Verified step by step guidance1
Identify the oxidation and reduction half-reactions. In this case, Fe^{2+} is oxidized to Fe^{3+}, and N_2 is reduced to N_2H_4.
Write the oxidation half-reaction: Fe^{2+} -> Fe^{3+} + e^-. Balance the charge by adding one electron to the right side.
Write the reduction half-reaction: N_2 + 4 e^- + 4 H_2O -> N_2H_4 + 4 OH^-. Balance the atoms and charges by adding electrons, water, and hydroxide ions.
Combine the balanced half-reactions. Ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.
Add the half-reactions together and simplify to get the balanced redox equation in a basic solution: 2 Fe^{2+}(aq) + N_2(g) + 4 OH^-(aq) -> 2 Fe^{3+}(aq) + N_2H_4(aq) + 2 H_2O(l).
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