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Chapter 14: Problem 6

Write the equilibrium constant expression for the reaction \(\mathrm{Fe}^{3+}(a q)+\mathrm{SCN}^{-}(a q) \rightleftarrows \mathrm{Fe}(\mathrm{SCN})^{2+}(a q)\)

Short Answer

Expert verified
The equilibrium constant expression for the reaction \(\mathrm{Fe}^{3+}(aq) + \mathrm{SCN}^{-}(aq) \rightleftarrows \mathrm{Fe}(\mathrm{SCN})^{2+}(aq)\) is given by: \[K_c = \frac{[\mathrm{Fe}(\mathrm{SCN})^{2+}]}{[\mathrm{Fe}^{3+}] [\mathrm{SCN}^{-}]}\]

Step by step solution

01

Write the balanced chemical equation

For this reaction, the balanced chemical equation is: \[\mathrm{Fe}^{3+}(aq) + \mathrm{SCN}^{-}(aq) \rightleftarrows \mathrm{Fe}(\mathrm{SCN})^{2+}(aq)\]
02

Identify the species in the reaction

In this reaction, we have the following species: - Reactants: \(\mathrm{Fe}^{3+}(aq)\) and \(\mathrm{SCN}^{-}(aq)\) - Product: \(\mathrm{Fe}(\mathrm{SCN})^{2+}(aq)\)
03

Write the Equilibrium Constant Expression

The equilibrium constant, denoted as \(K_c\), can be defined as the ratio of concentrations of products to reactants raised to their stoichiometric coefficients. In this case, we have: \[K_c = \frac{[\mathrm{Fe}(\mathrm{SCN})^{2+}]}{[\mathrm{Fe}^{3+}] [\mathrm{SCN}^{-}]}\] Here, \([\mathrm{Fe}^{3+}]\), \([\mathrm{SCN}^{-}]\), and \([\mathrm{Fe}(\mathrm{SCN})^{2+}]\) represent the equilibrium concentrations of the respective species in the reaction.

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Most popular questions from this chapter

The process of photosynthesis in plants converts carbon dioxide and water to glucose and oxygen: \(6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \quad \Delta E_{\mathrm{rxn}}=2801 \mathrm{~kJ}\) (a) Write the equilibrium constant expression for this conversion. (b) How would the equilibrium be affected if \(\mathrm{CO}_{2}(g)\) were added? (c) How would the equilibrium be affected if \(\mathrm{H}_{2} \mathrm{O}(l)\) were added? (d) How would the equilibrium be affected if the reaction vessel were warmed? (e) How would the equilibrium be affected if a catalyst were added?

One way of preparing hydrogen is by decomposition of water: \(2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftarrows 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \quad \Delta E_{\mathrm{rxn}}=484 \mathrm{~kJ}\) (a) Would you expect the decomposition to be more complete at equilibrium when it is run at high temperature or when it is run at low temperature? Explain. (b) According to your answer to (a), would the reaction speed up, slow down, or occur at the same rate as before the temperature was changed? Explain.

Suppose we have an equilibrium mixture of reactants and products for the reaction \(\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftarrows \mathrm{PCl}_{5}(g)\) Predict the direction in which the reaction will shift when: (a) Chlorine \(\left(\mathrm{Cl}_{2}\right)\) gas is added. (b) Chlorine gas is removed. (c) \(\mathrm{PCl}_{5}\) is added. (d) \(\mathrm{PCl}_{3}\) is removed. (e) \(\mathrm{H}_{2}\) gas is added. (Assume the \(\mathrm{H}_{2}\) does not react with any reactant or product.)

Suppose the reaction \(\mathrm{A}_{2}+\mathrm{B}_{2} \rightleftarrows 2 \mathrm{AB}\) proceeds via a one-step mechanism involving a collision between one \(\mathrm{A}_{2}\) molecule and one \(\mathrm{B}_{2}\) molecule. Suppose also that this reaction is reversible, and that the forward reaction is inherently much faster than the reverse reaction. (a) Does the equilibrium lie to the left or to the right? Explain your choice in terms of the reactant and product concentrations necessary to establish equal forward and reverse rates. (b) Does an analysis in terms of the relationship \(K_{\mathrm{eq}}=k_{\mathrm{f}} / k_{\mathrm{r}}\) yield the same answer as in (a)? Explain.

Will \(K_{\text {eq }}\) for an exothermic reaction increase or decrease when the reaction mixture is (a) heated and (b) cooled? Explain your answer.
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