Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Sn(s) ∣ Sn²⁺(aq, 0.022 mol L^-1) Ag⁺(aq, 2.7 mol L^-1) ∣ Ag(s)
E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Question

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Sn(s) ∣ Sn²⁺(aq, 0.022 mol L^-1)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn<sup>2+</sup>(aq, 0.022 mol L<sup>-1</sup>) Ag<sup>+</sup>(aq, 2.7 mol L<sup>-1</sup>) ∣ Ag(s) E°(Sn<sup>2+</sup>/Sn) = -0.14 V and E°(Ag<sup>+</sup>/Ag) = +0.80 V A) +1.01 V B) -0.83 V C) +1.31 V D) +0.01 V E) -0.66 V

Ag⁺(aq, 2.7 mol L^-1) ∣ Ag(s)
E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Quizplus · Accepted Answer

The Answer of Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s)∣ Sn²⁺(aq, 0.022 mol L^-1) Ag⁺(aq, 2.7 mol L^-1)∣ Ag(s) E°(Sn²⁺/Sn)= -0.14 V and E°(Ag⁺/Ag)= +0.80 V

Calculate the Cell Potential for the Following Reaction That Takes