The acid HOCI (hypochlorous acid) is produced by bubbling chlorine gas through a suspension of solid mercury(II) oxide particles in liquid water according to the equation 2HgO(s) + H₂O(1) + 2Cl₂(g)=2HOCl(aq) + HgO-HgCl₂ (s) What is the equilibrium-constant expression for this reaction?

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### The Equilibrium-Constant Expression for Heterogeneous Equilibria

**Introduction:**
Heterogeneous equilibria involve reactants and products that are not all in the same phase. For example, a solid may decompose, forming two gases. When writing equilibrium-constant expressions for heterogeneous reactions, generally the concentrations of pure solids and liquids are omitted. The composition of a pure solid or liquid does not change over the course of the reaction; only its quantity changes. Since its concentration isn’t changing, the values can usually be excluded.

**General Expression:**

Given the equation:  
\[ x \text{CD(s)} \rightleftharpoons c \text{C(g)} + d \text{D(g)} \]  

The equilibrium constant expression would be:  
\[ K = [\text{C}]^c[\text{D}]^d \]

---

### Example Reaction

**Problem:**
The acid \(\text{HOCl}\) (hypochlorous acid) is produced by bubbling chlorine gas through a suspension of solid mercury(II) oxide particles in liquid water according to the equation:  

\[ 2\text{HgO(s)} + \text{H}_2\text{O(l)} + 2\text{Cl}_2\text{(g)} \rightleftharpoons 2\text{HOCl(aq)} + \text{HgO}\cdot\text{HgCl}_2\text{(s)} \]

**Question:**
What is the equilibrium-constant expression for this reaction?

**Answer Options:**

- \((A)\) \[ K = \frac{[\text{HOCl}]^2[\text{H}_2\text{O}][\text{HgCl}_2]}{[\text{Cl}_2]^2[\text{H}_2\text{O}][\text{HgO}]^2} \]

- \((B)\) \[ K = \frac{[\text{HOCl}]^2}{[\text{Cl}_2]^2[\text{H}_2\text{O}]} \]

- \((C)\) \[ K = \frac{[\text{HOCl}]^2}{[\text{Cl}_2]^2} \]

- \((D)\) \[ K = \frac{[\text{Cl}_2]^2
Transcribed Image Text:### The Equilibrium-Constant Expression for Heterogeneous Equilibria **Introduction:** Heterogeneous equilibria involve reactants and products that are not all in the same phase. For example, a solid may decompose, forming two gases. When writing equilibrium-constant expressions for heterogeneous reactions, generally the concentrations of pure solids and liquids are omitted. The composition of a pure solid or liquid does not change over the course of the reaction; only its quantity changes. Since its concentration isn’t changing, the values can usually be excluded. **General Expression:** Given the equation: \[ x \text{CD(s)} \rightleftharpoons c \text{C(g)} + d \text{D(g)} \] The equilibrium constant expression would be: \[ K = [\text{C}]^c[\text{D}]^d \] --- ### Example Reaction **Problem:** The acid \(\text{HOCl}\) (hypochlorous acid) is produced by bubbling chlorine gas through a suspension of solid mercury(II) oxide particles in liquid water according to the equation: \[ 2\text{HgO(s)} + \text{H}_2\text{O(l)} + 2\text{Cl}_2\text{(g)} \rightleftharpoons 2\text{HOCl(aq)} + \text{HgO}\cdot\text{HgCl}_2\text{(s)} \] **Question:** What is the equilibrium-constant expression for this reaction? **Answer Options:** - \((A)\) \[ K = \frac{[\text{HOCl}]^2[\text{H}_2\text{O}][\text{HgCl}_2]}{[\text{Cl}_2]^2[\text{H}_2\text{O}][\text{HgO}]^2} \] - \((B)\) \[ K = \frac{[\text{HOCl}]^2}{[\text{Cl}_2]^2[\text{H}_2\text{O}]} \] - \((C)\) \[ K = \frac{[\text{HOCl}]^2}{[\text{Cl}_2]^2} \] - \((D)\) \[ K = \frac{[\text{Cl}_2]^2
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