ELECTROCHEMISTRY-HOMEWORK 7. Write down the cell notation for the redox reaction

Question

ELECTROCHEMISTRY-HOMEWORK 7. Write down the cell notation for the redox reaction given below Sn(s) 2 Ag-(aq) Sn2+(aq) + 2 Ag(s) A) Ag (ag)I Ag(s) II Sn(s)ISn2(aq)B) A C) Sn(s) I Sn2+(ag) Il Ag (ag) I Ag(s) E) Sn(s)I Ag(s) II Sn2+(aq)I Ag (aq) g(s) IAg (a)II Sn2(ag) I Sn(s) D) Sn2 (ag) I Sn(s) II Ag(s) I Ag (ag) 8. What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) I Sn2t(a) II Ag (ag) 1 Ag(s) A) Sn(s) B Agng)n2a) D) Ag(s) E) Pt 9. Which of the following is the strongest reducing agent? Mg2+(ag) +2e-Mg(s) Zn2+(aq) + 2e. Zn (s) E.--2.37V A) Al(s) B) Zn(s Mgs) D) AI3+(a)E) Mg2*(aq) 10. Which of the following is the strongest oxidizing agent? Ag+(aq) + e- Ag(s) Au3+(aq) +3e- Au(s) Br2+2 e- 2 Br-(aq) E"= 1.50V e-109v A) Br2) B) Au (s) Ags DB(a) E) Au3 (ag) 11. Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C·(The equation is balanced.) 3 Cl2(g) + 2 Fe(s) 6 a-(aq) + 2 Fe3+(aq) Fe3+(aq) + 3e. Fe(s) E°=-0.036 V A) 4.16 V B)-140 V C)-132 V D) 1.32 V E) 140 V

Explanation / Answer

7. C

8. B (Ag+ is the strong oxidising agent)

9. C (Mg is a strong reducing agent)

10. C (Ag+ is the strongest reducing agent)

11. E

Soln: 1.36 -(-0.036) = +1.40 V

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