In view of the signs ΔrG∘ of for the following reactionsPbO2+Pb→2PbO; ΔtG∘<0SnO2+Sn→2SnO; ΔTG∘>0Which oxidation states are more characteristic for lead and tin?

In view of the signs $Δ_{r} G^{\circ}$ of for the following reactions
$\begin{array}{ll} {PbO}_{2} + Pb \to 2 PbO; Δ_{t} G^{\circ} < 0 \\ {SnO}_{2} + Sn \to 2 SnO; Δ_{T} G^{\circ} > 0 \end{array}$
Which oxidation states are more characteristic for lead and tin?

A
For lead +4, for tin +2
B
For lead +2, for tin +2
C
For lead +4, for tin +4
D
For lead +2, for tin +4

Solution:

$Δ_{r} G^{\circ} < 0$ implies that the reaction is feasible. Thus, the more characteristic oxidation state oflead is +2.

$Δ_{r} G^{\circ} > 0$ implies that the reaction is not feasible. Thus, the more characteristic oxidation state of tin is +4.

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