Which equation is a balanced thermochemical equation for a neutralization (acid-base) reaction? O A. KOH(aq) + HNO3(aq)→ KNO3(aq) + H20(1) O B. 2 HCI(aq) + Zn(s) → ZNCI2(aq) + H2(1) A,H° = –153.9 kJ/mol-reaction OC. KOH(aq) + HCI(aq) → KCI(aq) + H2O(1) A,H° = -55.8 kJ/mol-reaction O D. H2SO4(aq) + NaOH(aq) → Na,SO4(aq) + H20(1) O E. NH4CI(s) → NH3(g) + HCI(g) A,H° = 176.4 kJ/mol-reaction Reset Selection

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**Neutralization Reaction Thermochemical Equations**

**Question:**
Which equation is a balanced thermochemical equation for a neutralization (acid-base) reaction?

**Options:**

- **A.** 
  \[
  \text{KOH(aq) + HNO}_3\text{(aq) } \rightarrow \text{KNO}_3\text{(aq) + H}_2\text{O(l)}
  \]

- **B.** 
  \[
  \text{2 HCl(aq) + Zn(s) } \rightarrow \text{ZnCl}_2\text{(aq) + H}_2\text{(l)} \quad \Delta H^\circ = -153.9 \text{ kJ/mol-reaction}
  \]

- **C.** 
  \[
  \text{KOH(aq) + HCl(aq) } \rightarrow \text{KCl(aq) + H}_2\text{O(l)} \quad \Delta H^\circ = -55.8 \text{ kJ/mol-reaction}
  \]

- **D.** 
  \[
  \text{H}_2\text{SO}_4\text{(aq) + NaOH(aq) } \rightarrow \text{Na}_2\text{SO}_4\text{(aq) + H}_2\text{O(l)}
  \]

- **E.** 
  \[
  \text{NH}_4\text{Cl(s) } \rightarrow \text{NH}_3\text{(g) + HCl(g)} \quad \Delta H^\circ = 176.4 \text{ kJ/mol-reaction}
  \]

**Explanation:**

A neutralization reaction typically involves an acid and a base reacting to form water and a salt. In this context, choices A and C are classic examples of neutralization reactions between a strong acid and a strong base resulting in water and a salt.

- **Choice A** is the neutralization of potassium hydroxide (KOH), a base, with nitric acid (HNO₃), producing potassium nitrate (KNO₃) and water.
  
- **Choice C** involves the reaction of potassium hydroxide (KOH) with hydrochloric acid (HCl) to form potassium chloride (KCl) and water.

**
Transcribed Image Text:**Neutralization Reaction Thermochemical Equations** **Question:** Which equation is a balanced thermochemical equation for a neutralization (acid-base) reaction? **Options:** - **A.** \[ \text{KOH(aq) + HNO}_3\text{(aq) } \rightarrow \text{KNO}_3\text{(aq) + H}_2\text{O(l)} \] - **B.** \[ \text{2 HCl(aq) + Zn(s) } \rightarrow \text{ZnCl}_2\text{(aq) + H}_2\text{(l)} \quad \Delta H^\circ = -153.9 \text{ kJ/mol-reaction} \] - **C.** \[ \text{KOH(aq) + HCl(aq) } \rightarrow \text{KCl(aq) + H}_2\text{O(l)} \quad \Delta H^\circ = -55.8 \text{ kJ/mol-reaction} \] - **D.** \[ \text{H}_2\text{SO}_4\text{(aq) + NaOH(aq) } \rightarrow \text{Na}_2\text{SO}_4\text{(aq) + H}_2\text{O(l)} \] - **E.** \[ \text{NH}_4\text{Cl(s) } \rightarrow \text{NH}_3\text{(g) + HCl(g)} \quad \Delta H^\circ = 176.4 \text{ kJ/mol-reaction} \] **Explanation:** A neutralization reaction typically involves an acid and a base reacting to form water and a salt. In this context, choices A and C are classic examples of neutralization reactions between a strong acid and a strong base resulting in water and a salt. - **Choice A** is the neutralization of potassium hydroxide (KOH), a base, with nitric acid (HNO₃), producing potassium nitrate (KNO₃) and water. - **Choice C** involves the reaction of potassium hydroxide (KOH) with hydrochloric acid (HCl) to form potassium chloride (KCl) and water. **
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