Open Question
Balance the following redox reaction in an acidic solution.
Cl2 (g) + S2O32- (aq) → Cl- (aq) + SO42- (aq)
5. Classification & Balancing of Chemical Reactions
Balancing Redox Reactions: Acidic Solutions
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is the coefficient of Fe3+ when the following reaction is balanced?
Bi3+ (aq) + Fe3+ (aq) + H2O (l) → BiO3- (aq) + Fe2+ (aq) + H+ (aq)
A
1
B
2
C
3
D
4
E
6
Verified step by step guidance1
Identify the oxidation states of each element in the reaction. Bi3+ is in the +3 oxidation state, Fe3+ is in the +3 oxidation state, and Fe2+ is in the +2 oxidation state.
Determine the changes in oxidation states. Bi3+ is reduced to BiO3-, and Fe3+ is reduced to Fe2+. This indicates that electrons are transferred in the reaction.
Write the half-reactions for the oxidation and reduction processes. The reduction half-reaction involves Bi3+ gaining electrons to form BiO3-. The oxidation half-reaction involves Fe3+ losing electrons to form Fe2+.
Balance the electrons transferred in the 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.
Combine the balanced half-reactions to form the overall balanced equation. Adjust the coefficients of each species to ensure mass and charge balance, focusing on the coefficient of Fe3+.
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