Consider the reactions- PbO2- PbO- - G298 - 0- SnO2- SnO- - G298 - 0The most probable oxidation state of Pb and Sn will be -

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Hydrogen Peroxide

Consider the ...

Question

Consider the reactions;
$P b O_{2} \to P b O, Δ G_{298} < 0;$
$S n O_{2} \to S n O, Δ G_{298} < 0$
The most probable oxidation state of $P b$ and $S n$ will be :

P b^{4 +}, S n^{2 +}

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P b^{4 +}, S n^{4 +}

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P b^{2 +}, S n^{3 +}

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P b^{2 +}, S n^{2 +}

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P b O_{2} \to P b O

Δ G_{298} < 0

S n O_{2} \to S n O

Δ G_{298} > 0

P b

S n

P b O_{2}

P b O Δ G_{298} < 0

S n O_{2}

S n O

Δ G_{298}

[1] P b^{2 +} > P b^{4}, S n^{2 +} > S n^{4 +}

[2] P b^{2 +} < P b^{4}, S n^{2 +} < S n^{4 +}

[3] P b^{2 +} > P b^{4}, S n^{2 +} < S n^{4 +}

[4] P b^{2 +} < P b^{4}, S n^{2 +} > S n^{4 +}

[5] S n^{2 +} < P b^{2 +}, S n^{4 +} > P b^{4 +}

[6] S n^{2 +} < P b^{2 +}, S n^{4 +} < P b^{4 +}

P b^{4 +} + S n^{2 +} \to S n^{4 +} + P b^{2 +}

S n^{4 +} + P b^{2 +} \to P b^{4 +} + S n^{2 +}

E_{P b^{4 +} / P b^{2 +}}^{o} = 1.69 V, E_{S n^{4 +} / S n^{2 +}}^{o} = 0.15 V

Stability of ions of $G e, S n, a n d P b$ will be in the order:

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