Answer :
The equilibrium constant (Kc) is 1.37 * 10² M⁻¹.
First, we write the reaction equation:
Fe³⁺ + SCN⁻ ↔ [FeSCN]²⁺
From this, we can see that the iron(III) cation (Fe³⁺) and the thiocyanate anion (SCN⁻) are the reactants, while the iron(III) thiocyanate ion ([FeSCN]²⁺) is the product. Based on this, we can write the expression for the equilibrium constant (Kc):
[tex]Kc = \frac{[[FeSCN]^{2+}]}{[Fe^{3+} ][SCN^{-} ] }[/tex]
[Fe³⁺] - equilibrium concentration of the iron(III) ion (1.32 * 10⁻³M)
[SCN⁻] - equilibrium concentration of the thiocyanate ion (1.02 * 10⁻³ M)
[[FeSCN]²⁺] - equilibrium concentration of the iron(III) thiocyanate ion (1.84 * 10⁻⁴ M)
Now we plug the known values into the expression:
Kc = 1.84 * 10⁻⁴ M / (1.32 * 10⁻³ M * 1.02 * 10⁻³M)
Kc = 1.37 * 10² M⁻¹
You can learn more about equilibrium constants here:
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