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Ch.15 - Chemical Equilibrium
All textbooksTro 4th EditionCh.15 - Chemical EquilibriumProblem 43
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Chapter 15, Problem 43

Consider the reaction: Fe3+ (aq) + SCN- (aq) ⇌ FeSCN2+ (aq). A solution is made containing an initial [Fe3+] of 1.0*10^-3 M and an initial [SCN-] of 8.0*10^-4 M. At equilibrium, [FeSCN2+] = 1.7*10^-4 M. Calculate the value of the equilibrium constant (Kc).

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Identify the initial concentrations of the reactants: [Fe^{3+}]_0 = 1.0 \times 10^{-3} \text{ M} and [SCN^-]_0 = 8.0 \times 10^{-4} \text{ M}.
Determine the change in concentration for the formation of FeSCN^{2+} at equilibrium, which is given as [FeSCN^{2+}] = 1.7 \times 10^{-4} \text{ M}.
Calculate the equilibrium concentrations of the reactants: [Fe^{3+}]_{eq} = [Fe^{3+}]_0 - [FeSCN^{2+}] and [SCN^-]_{eq} = [SCN^-]_0 - [FeSCN^{2+}].
Write the expression for the equilibrium constant K_c: K_c = \frac{[FeSCN^{2+}]_{eq}}{[Fe^{3+}]_{eq} \times [SCN^-]_{eq}}.
Substitute the equilibrium concentrations into the K_c expression to find the value of the equilibrium constant.
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Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kp = 2.91⨉103 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of Cl2 is 285 torr. What is the partial pressure of SO2Cl2in this mixture?

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