Open Question
In the equation PbO2 + 4 HCl → 2 H2O + PbCl2 + Cl2, how many electrons are transferred?
6. Chemical Quantities & Aqueous Reactions
Balancing Redox Reactions: Acidic Solutions
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Which of the following is the correctly balanced redox reaction for S2O3^2- (aq) + Cl2(g) → SO4^2- (aq) + Cl^- (aq) in acidic solution?
A
S2O3^2- + Cl2 + 2H2O → 2SO4^2- + 2Cl^- + 4H^+
B
S2O3^2- + Cl2 + 4H2O → 2SO4^2- + 2Cl^- + 8H^+
C
S2O3^2- + Cl2 + 6H2O → 2SO4^2- + 2Cl^- + 12H^+
D
S2O3^2- + Cl2 + 5H2O → 2SO4^2- + 2Cl^- + 10H^+
Verified step by step guidance1
Identify the oxidation and reduction half-reactions. In this case, S2O3^2- is oxidized to SO4^2-, and Cl2 is reduced to Cl^-.
Write the oxidation half-reaction: S2O3^2- → SO4^2-. Balance the sulfur atoms first, then add water molecules to balance the oxygen atoms, and finally add H^+ ions to balance the hydrogen atoms.
Write the reduction half-reaction: Cl2 → Cl^-. Balance the chlorine atoms first, then add electrons to balance the charge.
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 H^+ ions to balance the charge in the acidic solution. Verify that the atoms and charges are balanced in the final equation.
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