Depict the galvanic cell in which the reaction $Z n (s) + 2 A g^{+} (a q) ⟶ Z n^{2 +} (a q) + 2 A g (s)$ takes place, further show:
Which of the electrode is negatively charged,

The carriers of the current in the cell.

Individual reaction at each electrode.

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Solution

The galvanc cell corresponding to the given redox reaction can be represented as:
$Z n | Z n_{(a q)}^{2 +} | | A g_{(a q)}^{+} | A g$
Zn electrode is negatively charged because at this electrode, Zn oxidized to $Z n^{2 +}$ and the leaving electrons accumulate on this electrode.

Ions are the carriers of current in the cell.

$Z n | Z n_{(a q)}^{2 +} | | A g_{(a q)}^{+} | A g$
The Oxidation reaction taking place at Zn electrode (Anode) can be represented as:
$Z n_{(s)} ⟶ Z n_{(a q)}^{2 +} + 2 e^{-}$
And the Reduction reaction taking place at Ag electrode (Cathode) can be represented as:
$A g_{(a q)}^{+} + e^{-} ⟶ A g_{(s)}$

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Similar questions

Depict the galvanic cell in which the reaction, $Z n (s) + 2 A g^{+} (a q) \to Z n^{2 +} (a q) + 2 A g (s)$ takes place . Further show :

Which of the electrode is negatively charged

The carriers of the current in the cell

Individual reaction at each electrode

Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place, further show:

(i) which of the electrode is negatively charged,

(ii) the carriers of the current in the cell, and

(iii) individual reaction at each electrode.

Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:

(i) Which of the electrode is negatively charged?

(ii) The carriers of the current in the cell.

(iii) Individual reaction at each electrode.

Z n (s) + 2 A g^{+} (a q) \to Z n^{2 +} (a q) + 2 A g (s)

Z n (s) + 2 A g^{+} (a q) \to Z n^{2 +} (a q) + 2 A g (s)

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