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Determine the Cell Notation for the Redox Reaction Given Below

Question 16

Multiple Choice

Determine the cell notation for the redox reaction given below:
3Cl2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)


A) Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s) Determine the cell notation for the redox reaction given below: 3Cl<sub>2</sub>(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe<sup>3+</sup>(aq) A) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe(s) ∣ Fe<sup>3+</sup>(aq) B) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) Fe<sup>3+</sup>(aq) <sup> </sup>∣<sup> </sup>Fe(s) C) Fe<sup>3+</sup>(aq) ∣ Fe(s) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) D) Fe(s) ∣ Cl<sub>2</sub>(g) Fe<sup>3+</sup>(aq) ∣ Cl⁻(aq) ∣ Pt(s) E) Fe(s) ∣ Fe<sup>3+</sup>(aq) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe(s) ∣ Fe3+(aq)
B) Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s) Determine the cell notation for the redox reaction given below: 3Cl<sub>2</sub>(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe<sup>3+</sup>(aq) A) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe(s) ∣ Fe<sup>3+</sup>(aq) B) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) Fe<sup>3+</sup>(aq) <sup> </sup>∣<sup> </sup>Fe(s) C) Fe<sup>3+</sup>(aq) ∣ Fe(s) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) D) Fe(s) ∣ Cl<sub>2</sub>(g) Fe<sup>3+</sup>(aq) ∣ Cl⁻(aq) ∣ Pt(s) E) Fe(s) ∣ Fe<sup>3+</sup>(aq) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe3+(aq) ∣ Fe(s)
C) Fe3+(aq) ∣ Fe(s) Determine the cell notation for the redox reaction given below: 3Cl<sub>2</sub>(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe<sup>3+</sup>(aq) A) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe(s) ∣ Fe<sup>3+</sup>(aq) B) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) Fe<sup>3+</sup>(aq) <sup> </sup>∣<sup> </sup>Fe(s) C) Fe<sup>3+</sup>(aq) ∣ Fe(s) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) D) Fe(s) ∣ Cl<sub>2</sub>(g) Fe<sup>3+</sup>(aq) ∣ Cl⁻(aq) ∣ Pt(s) E) Fe(s) ∣ Fe<sup>3+</sup>(aq) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)
D) Fe(s) ∣ Cl2(g) Determine the cell notation for the redox reaction given below: 3Cl<sub>2</sub>(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe<sup>3+</sup>(aq) A) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe(s) ∣ Fe<sup>3+</sup>(aq) B) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) Fe<sup>3+</sup>(aq) <sup> </sup>∣<sup> </sup>Fe(s) C) Fe<sup>3+</sup>(aq) ∣ Fe(s) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) D) Fe(s) ∣ Cl<sub>2</sub>(g) Fe<sup>3+</sup>(aq) ∣ Cl⁻(aq) ∣ Pt(s) E) Fe(s) ∣ Fe<sup>3+</sup>(aq) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt(s)
E) Fe(s) ∣ Fe3+(aq) Determine the cell notation for the redox reaction given below: 3Cl<sub>2</sub>(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe<sup>3+</sup>(aq) A) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Fe(s) ∣ Fe<sup>3+</sup>(aq) B) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) Fe<sup>3+</sup>(aq) <sup> </sup>∣<sup> </sup>Fe(s) C) Fe<sup>3+</sup>(aq) ∣ Fe(s) Cl⁻(aq) ∣ Cl<sub>2</sub>(g) ∣ Pt(s) D) Fe(s) ∣ Cl<sub>2</sub>(g) Fe<sup>3+</sup>(aq) ∣ Cl⁻(aq) ∣ Pt(s) E) Fe(s) ∣ Fe<sup>3+</sup>(aq) Cl<sub>2</sub>(g) ∣ Cl⁻(aq) ∣ Pt(s) Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)

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