Question at position 8 Consider the balanced redox reaction: 2 Fe2+(aq) + Cl2(g) → 2 Fe3+(aq) + 2Cl– (aq) How many electrons are transferred in this reaction as written? 12634Single choice
A
1
B
2
C
6
D
3
E
4

Question

Question at position 8 Consider the balanced redox reaction: 2 Fe2+(aq) + Cl2(g) → 2 Fe3+(aq) + 2Cl– (aq) How many electrons are transferred in this reaction as written? 12634

BlackTom AI · Accepted Answer

Fe2+ is oxidized to Fe3+ (loses one electron) while Cl2 is reduced to 2 Cl– (gains electrons).

1. Relevant knowledge points and concepts
- Oxidation is loss of electrons; reduction is gain of electrons.
- In half-reactions, the number of electrons lost must equal electrons gained for the overall balanced redox equation.
- Stoichiometric coefficients in the balanced equation determine the total electrons transferred "as written."

2. Step-by-step reasoning
Write the half-reactions for the species involved:
- Oxidation half-reaction: Fe2+ → Fe3+ + e–
- Reduction half-reaction: Cl2 + 2 e– → 2 Cl–

3. Intermediate steps and electron accounting
- The balanced full equation shows 2 Fe2+ reacting with 1 Cl2. Apply stoichiometry to the oxidation half-reaction:
  For 1 Fe2+: Fe2+ → Fe3+ + e–
  For 2 Fe2+: 2 Fe2+ → 2 Fe3+ + 2 e–  (multiply oxidation half-reaction by 2)
- The reduction half-reaction as written already uses 2 electrons:
  Cl2 + 2 e– → 2 Cl–
- Combine the half-reactions: the 2 e– produced by oxidation are consumed by reduction, yielding the overall balanced reaction:
  2 Fe2+ + Cl2 → 2 Fe3+ + 2 Cl–

4. Why the correct answer is correct
- Total electrons transferred equals the number of electrons exchanged between half-reactions. From the balanced equation, oxidation of two Fe2+ ions produces 2 electrons, which are exactly the 2 electrons gained by Cl2. Therefore 2 electrons are transferred in the reaction as written.

5. Why other options are incorrect
- 1: Incorrect because each Fe2+ → Fe3+ involves one electron; with two Fe2+ the total is 2 electrons, not 1.
- 6 and 4: Incorrect because they imply multiple-electron changes per atom beyond the stoichiometry shown.
- 3: Incorrect because electron transfers must balance; there are exactly 2 electrons involved, not 3.

6. Conclusion
The total number of electrons transferred in the reaction as written is 2, which matches the provided correct answer.

Question at position 8 Consider the balanced redox reaction: 2 Fe2+(aq) + Cl2(g) → 2 Fe3+(aq) + 2Cl– (aq) How many electrons are transferred in this reaction as written? 12634Single choice

Similar Questions

Indicate whether the following reactions are oxidation reactions, reduction reactions or neither. 1: 2: 3:

Under acidic conditions the bromate ion (BrO3–) is reduced to the bromide ion. The balanced half-equation for this process is:

Balance the following redox equation which occurs in acidic solution. N2H4(g) + BrO3–(aq) → Br–(aq) + N2(g)

Iodide ion reacts with manganese(IV) oxide according to: MnO2(s) + 2 I– (aq) + 4 H+(aq) → I2(aq) + Mn2+(aq) + 2 H2O(l) Which statement correctly describes this reaction?

The only redox reaction among the following is:

Question at position 16 Which substance serves as the oxidizing agent in the following reaction? I2(s) + 2Fe2+(aq) → 2I−(aq) + 2Fe3+(aq) Fe3+(aq) Fe2+(aq)I2(s)I−(aq)

More Practical Tools for Students Powered by AI Study Helper

Homework AI Solver

Stylized AI Paper Writer

Plagiarism Checker Assistant

Citation AI Academic Writing Tool

In-Class Translation Assistant

AI Note Generator

AI Quiz Answers

Past Exam Questions from University Test Bank

Smart Practice Assistant

Adaptive Practice

Making Your Study Simpler