Multiple Choice
Which of the following correctly balances the chemical equation for the reaction between Fe^{3+}(aq) and Sn(s) to produce Fe(s) and Sn^{2+}(aq)?
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3. Chemical Reactions
Balancing Chemical Equations
Multiple Choice
Which of the following is the correct balanced equation for the reaction: MnO4^-(aq) + Br^-(aq) → MnO2(s) + BrO3^-(aq)?
A
MnO4^-(aq) + Br^-(aq) → MnO2(s) + BrO3^-(aq)
B
2 MnO4^-(aq) + 6 Br^-(aq) + 4 H2O(l) → 2 MnO2(s) + 3 BrO3^-(aq) + 8 OH^-(aq)
C
2 MnO4^-(aq) + 3 Br^-(aq) + 4 H2O(l) → 2 MnO2(s) + 3 BrO3^-(aq) + 8 OH^-(aq)
D
MnO4^-(aq) + 6 Br^-(aq) + 4 H2O(l) → MnO2(s) + 3 BrO3^-(aq) + 8 OH^-(aq)
Verified step by step guidance1
Identify that this is a redox reaction occurring in a basic solution, involving permanganate ion (MnO4^-), bromide ion (Br^-), manganese dioxide (MnO2), and bromate ion (BrO3^-).
Write the half-reactions separately: the reduction half-reaction for MnO4^- to MnO2, and the oxidation half-reaction for Br^- to BrO3^-.
Balance each half-reaction for atoms other than O and H first, then balance oxygen atoms by adding H2O, and hydrogen atoms by adding OH^- (since the solution is basic).
Balance the charges in each half-reaction by adding electrons (e^-), ensuring that the total charge is the same on both sides of each half-reaction.
Multiply the half-reactions by appropriate coefficients so that the number of electrons lost in oxidation equals the number gained in reduction, then add the half-reactions together and simplify to get the balanced overall equation.
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