A cell can be prepared from copper and tin.What is the E°_cell for the cell that forms from the following half-reactions?
Cu²⁺(aq) + 2e^-
Cu(s) ;E° = 0.34 V
Sn⁴⁺(aq) + 2e^-
Sn²⁺(aq) ;E° = 0.13 V

Question

A cell can be prepared from copper and tin.What is the E°_cell for the cell that forms from the following half-reactions?
Cu²⁺(aq) + 2e^-

A cell can be prepared from copper and tin.What is the E°<sub>cell</sub> for the cell that forms from the following half-reactions? Cu<sup>2+</sup>(aq) + 2e<sup>-</sup> Cu(s) ;E° = 0.34 V Sn<sup>4+</sup>(aq) + 2e<sup>-</sup> Sn<sup>2+</sup>(aq) ;E° = 0.13 V A) 0.47 V B) 0.21 V C) -0.21 V D) -0.47 V E) 0.42 V

Cu(s) ;E° = 0.34 V
Sn⁴⁺(aq) + 2e^- A cell can be prepared from copper and tin.What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq) + 2e- Cu(s) ;E° = 0.34 V Sn4+(aq) + 2e- Sn2+(aq) ;E° = 0.13 V A) 0.47 V B) 0.21 V C) -0.21 V D) -0.47 V E) 0.42 V

Sn²⁺(aq) ;E° = 0.13 V

Quizplus · Accepted Answer

The standard cell potential, E°cell, is calculated by subtracting the reduction potential of the anode from the reduction potential of the cathode:
E°cell = E°cathode - E°anode

In this case, the cathode is Cu and the anode is Sn:
E°cell = E°Cu - E°Sn
E°cell = 0.34 V - 0.13 V
E°cell = 0.21 V

Note that the given half-reactions are reduction reactions, so we need to flip the sign of the standard reduction potential for the anode (Sn) to use it in the E°cell calculation. The correct answer is B.

A Cell Can Be Prepared from Copper and Tin