Write the following ions in order of decreasing capacity to accept electrons.
$H^{+}, M g^{2 +}, K^{+}, A g^{+}, Z n^{2 +}$

A g^{+} > H^{+} > Z n^{2 +} > M g^{2 +} > K^{+}

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H^{+} > Z n^{2 +} > M g^{2 +} > K^{+} > A g^{+}

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K^{+} > M g^{2 +} > Z n^{2 +} > H^{+} > A g^{+}

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M g^{2 +} > Z n^{2 +} > K^{+} > A g^{+} > H^{+}

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Solution

The correct option is A $A g^{+} > H^{+} > Z n^{2 +} > M g^{2 +} > K^{+}$
Based on electrochemical series, elements can be arranged in order of decreasing capacity to accept electrons i.e decreasing reduction potentials.
$A g^{+} > H^{+} > Z n^{2 +} > M g^{2 +} > K^{+}$ where reduction potential of $A g^{+}$ is positive, for $H^{+}$ is zero and others have negative $E^{0}$
Alkali metals are most electropositive followed by alkaline earth metals, thus have most negative reduction potential and least capacity to accept electrons.

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O^{2 -}

The cell representation of the given reactions is:

Zn(s) + 2Ag⁺ → Zn²⁺ + 2Ag(s)

$E_{A g^{+} | A g}^{\circ} = 0.8$ volt and $E_{Z n^{2 +} | Z n}^{\circ} = - 0.76$ volt

Which of the following is correct?

F e^{2 +}, N i^{2 +}, C a^{2 +}, K^{+}, M g^{2 +}, N a^{+}, C u^{2 +}, Z n^{2 +}

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E_{C u^{2 +} / C u}^{\circ} = 0.34 v o l t; E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 v o l t

E_{A g^{+} / A g}^{\circ} = 0.8 v o l t; E_{M g^{2 +} / M g}^{\circ} = - 2.37 v o l t

Δ G^{\circ}

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