For the following galvanic cell, represented in line notation, determine what balanced half-reactions occur at each electrode. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) Cr (s) | Cr3 + (aq) || Ag + (aq) | Ag (s) anode half-reaction:cathode half-reaction:

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Chemistry

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10 November, 20:48

For the following galvanic cell, represented in line notation, determine what balanced half-reactions occur at each electrode. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) Cr (s) | Cr3 + (aq) || Ag + (aq) | Ag (s) anode half-reaction:cathode half-reaction:

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Doyle · Answer 1

Anode (oxidation) : Cr (s) ⇒ Cr³⁺ (aq) + 3 e⁻

Cathode (reduction) : Ag⁺ (aq) + 1 e⁻ ⇒ Ag (s)

Explanation:

Let's consider the notation of a galvanic cell.

Cr (s) | Cr³⁺ (aq) || Ag⁺ (aq) | Ag (s)

On the left, it is represented the anode (oxidation) and on the right, it is represented the cathode (reduction).

The half-reactions are:

Anode (oxidation) : Cr (s) ⇒ Cr³⁺ (aq) + 3 e⁻

Cathode (reduction) : Ag⁺ (aq) + 1 e⁻ ⇒ Ag (s)

To have the global reaction, we have to multiply the reduction by 3 (so the number of electrons gained and lost are the same) and add both half-reactions.

Global reaction: Cr (s) + 3 Ag⁺ (aq) ⇒ Cr³⁺ (aq) + 3 Ag (s)