Write the expressions for \(K_{c}\) for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. (a) \(\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{O}(g)\) (b) $\mathrm{Si}(s)+2 \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SiCl}_{4}(g)$ (c) $\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{HCl}(g)$ (d) $\mathrm{O}_{2}(g)+2 \mathrm{CO}(g) \rightleftharpoons 2 \mathrm{CO}_{2}(g)$ (e) $\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}^{+}(a q)$ (f) $\mathrm{Fe}^{2+}(a q)+\mathrm{Ce}^{4+}(a q) \rightleftharpoons \mathrm{Fe}^{3+}(a q)+\mathrm{Ce}^{3+}(a q)$ (g) $\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$

Step by step solution

01

(a) Reaction and Kc expression for O2(g) ⇌ 2 O(g) equilibrium

This is a homogeneous reaction since both species are in the gas phase. The equilibrium constant, Kc, can be expressed as follows: Kc = \(\frac{[\mathrm{O}]^2}{[\mathrm{O}_{2}]}\)

02

(b) Reaction and Kc expression for Si(s) + 2 Cl2(g) ⇌ SiCl4(g) equilibrium

This is a heterogeneous reaction, as there are solid and gas species involved. The equilibrium constant, Kc, can be expressed as follows: Kc = \(\frac{[\mathrm{SiCl}_{4}]}{[\mathrm{Cl}_{2}]^2}\) (Note: we don't include the solid Si in the expression)

03

(c) Reaction and Kc expression for H2(g) + Cl2(g) ⇌ 2 HCl(g) equilibrium

This is a homogeneous reaction since all species are in the gas phase. The equilibrium constant, Kc, can be expressed as follows: Kc = \(\frac{[\mathrm{HCl}]^2}{[\mathrm{H}_{2}][\mathrm{Cl}_{2}]}\)

04

(d) Reaction and Kc expression for O2(g) + 2 CO(g) ⇌ 2 CO2(g) equilibrium

This is a homogeneous reaction since all species are in the gas phase. The equilibrium constant, Kc, can be expressed as follows: Kc = \(\frac{[\mathrm{CO}_{2}]^2}{[\mathrm{O}_{2}][\mathrm{CO}]^2}\)

05

(e) Reaction and Kc expression for HCO3-(aq) ⇌ CO32-(aq) + H+(aq) equilibrium

This is a homogeneous reaction since all species are in the aqueous phase. The equilibrium constant, Kc, can be expressed as follows: Kc = \(\frac{[\mathrm{CO}_{3}^{2-}][\mathrm{H}^{+}]}{[\mathrm{HCO}_{3}^{-}]}\)

06

(f) Reaction and Kc expression for Fe2+(aq) + Ce4+(aq) ⇌ Fe3+(aq) + Ce3+(aq) equilibrium

This is a homogeneous reaction since all species are in the aqueous phase. The equilibrium constant, Kc, can be expressed as follows: Kc = \(\frac{[\mathrm{Fe}^{3+}][\mathrm{Ce}^{3+}]}{[\mathrm{Fe}^{2+}][\mathrm{Ce}^{4+}]}\)

07

(g) Reaction and Kc expression for CaCO3(s) ⇌ CaO(s) + CO2(g) equilibrium

This is a heterogeneous reaction, as there are solid and gas species involved. The equilibrium constant, Kc, can be expressed as follows: Kc = \([CO_2]\) (Note: we don't include the solid CaCO3 and CaO in the expression)

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