Multiple Choice
Which of the following statements is true for a salt bridge?
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5. Classification & Balancing of Chemical Reactions
Galvanic Cell (Simplified)
Multiple Choice
What is the balanced half reaction that occurs at the anode in the overall cell reaction of a voltaic cell?
3 MnO4–(aq) + 5 Fe(s) → 3 Mn2+(aq) + 5 Fe3+(aq)
A
MnO4–(aq) + 8 H+(aq) + 5 e– → Mn2+(aq) + 4 H2O(l)
B
2 MnO4–(aq) + 12 H+(aq) + 6 e– → 2 Mn2+(aq) + 3 H2O(l)
C
Fe(s) →Fe3+(aq) + 3 e–
D
Fe(s) →Fe2+(aq) + 2 e–
E
Fe2+(aq) → Fe3+(aq) + e–
Verified step by step guidance1
Identify the overall cell reaction given: 3 MnO4–(aq) + 5 Fe(s) → 3 Mn2+(aq) + 5 Fe3+(aq). This reaction involves both oxidation and reduction processes.
Determine the oxidation process occurring at the anode. In a voltaic cell, oxidation occurs at the anode, where electrons are lost.
Examine the species involved in the oxidation process. Here, Fe(s) is oxidized to Fe3+(aq), indicating that iron is losing electrons.
Write the half-reaction for the oxidation of iron. Start with the reactant Fe(s) and show the loss of electrons to form Fe3+(aq).
Balance the half-reaction for charge and mass. Ensure that the number of electrons lost equals the change in oxidation state from Fe(s) to Fe3+(aq), which is 3 electrons.
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