Consider a galvanic cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a silver electrode immersed in 1.0 M Ag⁺.
Zn²⁺ + 2e^- $\to$ Zn
$\varepsilon$ ° = -0.76 V
Ag⁺ + e^- $\to$ Ag
$\varepsilon$ ° = 0.80 V
Which of the electrodes is the anode?

Question

Consider a galvanic cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a silver electrode immersed in 1.0 M Ag⁺.
Zn²⁺ + 2e^-

\to

Zn

\varepsilon

° = -0.76 V
Ag⁺ + e^-

\to

Ag

\varepsilon

° = 0.80 V
Which of the electrodes is the anode?

Quizplus · Accepted Answer

The Answer of Consider a galvanic cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a silver electrode immersed in 1.0 M Ag⁺. Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$° = -0.76 V Ag⁺ + e^- $\to$ Ag $\varepsilon$° = 0.80 V Which of the electrodes is the anode?

Consider a Galvanic Cell with a Zinc Electrode Immersed in 1.0