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5 June, 18:01

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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  1. 5 June, 21:28
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    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)
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