Write the expression for \(K_{c}\) for the following reactions. \(\operatorname{In}\) each case indicate whether the reaction is homogeneous or heterogeneous. (a) \(\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g)\) (b) $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)$ (c) \(\mathrm{CO}_{2}(g)+\mathrm{C}(s) \rightleftharpoons 2 \mathrm{CO}(g)\) (d) $\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)$ (e) $\mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(I) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}^{+}(a q)$ (f) $\mathrm{Fe}^{2+}(a q)+\mathrm{Zn}(s) \rightleftharpoons \mathrm{Zn}^{2+}(a q)+\mathrm{Fe}(s)$ (g) $\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q)$

Step by step solution

01

(a) I2(g) 2 I(g)

For this reaction, the equilibrium constant Kc can be written as: \[K_c = \frac{[\mathrm{I}]^2}{[\mathrm{I}_2]}\] Since all the species involved in this reaction are in the gas phase, the reaction is homogeneous.

02

(b) 2 SO2(g) + O2(g) 2 SO3(g)

The equilibrium constant Kc for this reaction is: \[K_c = \frac{[\mathrm{SO}_3]^2}{[\mathrm{SO}_2]^2[\mathrm{O}_2]}\] All species in this reaction are in the gas phase, so this is a homogeneous reaction.

03

(c) CO2(g) + C(s) 2 CO(g)

The equilibrium constant Kc can be expressed as: \[K_c = \frac{[\mathrm{CO}]^2}{[\mathrm{CO}_2]}\] This reaction involves both gaseous and solid species, hence it is a heterogeneous reaction.

04

(d) H2O(g) + CO(g) CO2(g) + H2(g)

For this reaction, the equilibrium constant Kc is: \[K_c = \frac{[\mathrm{CO}_2][\mathrm{H}_2]}{[\mathrm{H}_2\mathrm{O}][\mathrm{CO}]}\] All species are in the gas phase, making this a homogeneous reaction.

05

(e) CO2(aq) + H2O(l) HCO3^-(aq) + H^(aq)

The equilibrium constant Kc for this reaction is: \[K_c = \frac{[\mathrm{HCO}_3^-][\mathrm{H}^+]}{[\mathrm{CO}_2][\mathrm{H}_2\mathrm{O}]}\] In this reaction, we have aqueous and liquid species involved, so it is a heterogeneous reaction.

06

(f) Fe^2+(aq) + Zn(s) Zn^2+(aq) + Fe(s)

The equilibrium constant Kc for this reaction can be expressed as: \[K_c = \frac{[\mathrm{Zn}^{2+}]}{[\mathrm{Fe}^{2+}]}\] This reaction involves both aqueous and solid species, so it is heterogeneous.

07

(g) CaCO3(s) Ca^2+(aq) + CO3^2-(aq)

The equilibrium constant Kc for this reaction is: \[K_c = [\mathrm{Ca}^{2+}][\mathrm{CO}_3^{2-}]\] Since this reaction involves solid and aqueous species, it is a heterogeneous reaction.

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