## 14.33

$\Delta G^{\circ} = -nFE_{cell}^{\circ}$

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### 14.33

Can someone explain part B to me? What does it mean if an element will disproportionate in aqueous solution ?

Chem_Mod
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### Re: 14.33

Disproportionation is a type of redox reaction in which an element undergoes both oxidation and reduction to form two different products. In other words, part of the element oxidizes(or reduces) the other part of the element. This will give out two different product of the same element. This is common in multiple valence nonmetal element like Cl, Br, P etc. For example,$2H_{2}PO_{4}^{-}\rightarrow HPO_{4}^{2-} + H_{3}PO_{4}$

andrea_Disc3D
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### Re: 14.33

When the question asks to identify whether Tl^+ will disproportionate in an aqueous solution, the answer is no because Gibss free energy is positive (Given: +215kj/mol) and not spontaneous, but also K <1, right? Is this a right reasoning? I know that there is also an equation that related Gibbs Free energy and the equilibrium constant so would proving that K<1, also be a sufficient answer?

Kevin Pham 2G
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### Re: 14.33

andrea_Disc3D wrote:When the question asks to identify whether Tl^+ will disproportionate in an aqueous solution, the answer is no because Gibss free energy is positive (Given: +215kj/mol) and not spontaneous, but also K <1, right? Is this a right reasoning? I know that there is also an equation that related Gibbs Free energy and the equilibrium constant so would proving that K<1, also be a sufficient answer?

Proving that K<1 should also be a sufficient answer b/c K<1 means that reactants are more favored than products, just as a positive Gibbs free energy means that the forward reaction (formation of products) is not favored.