Question

aqueous iron(iii) and hydroxide ions combine to form solid iron(iii) hydroxide. fe3 (aq) 3 oh– (aq) ⇌ fe(oh)3 (s) when equilibrium is reached at a certain temperature, there is 3.6 g fe(oh)3 (s) and the concentrations of iron(iii) and hydroxide are 0.555 m and 0.750 m, respectively. what is the value of kc for this reaction?

Answer 1

The value of Kc for this reaction is 4.27.

Balanced chemical reaction: Fe3+(aq) + 3OH–(aq) ⇌ Fe(OH)3

c(Fe3+) = 0.555 M; concentration of iron ions

c(OH-) = 0.750 M; concentration of hydroxide ions

m(Fe(OH)3) = 3.6 g; mass of iron(III) hydroxide

The equilibrium constant (Kc) is a ratio of the concentration of the products  to the concentration of the reactants (in this reaction iron and hydroxide ions). Concentration of the product is 1, because it is in the solid state.

Kc = 1 / c(Fe3+) x c(OH-)³

Kc = 1 / (0.555 M x (0.750 M)³

Kc = 4.27; equilibrium constant for this reaction.

More info about Kc: brainly.com/question/15115430

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