Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N2(g) + 3 H,(g) → 2 NH3(g) AH=-92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH,(g) + 20,(9) → HNO3(g) + H,0(g) AH=-330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ.

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### Formation of Nitric Acid

**Overview:**

Nitric acid can be synthesized in a two-step process involving atmospheric gases: nitrogen, hydrogen, and oxygen. This procedure relies on hydrogen prepared by reforming natural gas.

**Step 1: Formation of Ammonia**

In the first step, nitrogen and hydrogen react to form ammonia. The balanced chemical equation for this reaction is:

\[ 
N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \quad \Delta H = -92 \text{ kJ} 
\]

**Step 2: Formation of Nitric Acid and Water**

In the second step, ammonia and oxygen react to produce nitric acid and water. The balanced chemical equation is:

\[ 
NH_3(g) + 2O_2(g) \rightarrow HNO_3(g) + \text{H}_2\text{O}(g) \quad \Delta H = -330 \text{ kJ} 
\]

**Thermodynamics:**

To find the net change in enthalpy for the formation of one mole of nitric acid from these reactions:

1. Sum the enthalpy changes of the two reactions.
2. Express the result for the formation of one mole of nitric acid.

**Calculation:**

Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen, and oxygen. Round your answer to the nearest kJ.

\[ \Delta H_{\text{net}} = \Delta H_1 + \Delta H_2 \]

**Input:**

\[ 
\text{Enter your answer in kJ:} \; \square 
\]

---

**Note:** This lesson demonstrates the application of thermodynamics in chemical reactions, particularly in the synthesis of industrial chemicals like nitric acid, highlighting the conservation of energy principle.
Transcribed Image Text:### Formation of Nitric Acid **Overview:** Nitric acid can be synthesized in a two-step process involving atmospheric gases: nitrogen, hydrogen, and oxygen. This procedure relies on hydrogen prepared by reforming natural gas. **Step 1: Formation of Ammonia** In the first step, nitrogen and hydrogen react to form ammonia. The balanced chemical equation for this reaction is: \[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \quad \Delta H = -92 \text{ kJ} \] **Step 2: Formation of Nitric Acid and Water** In the second step, ammonia and oxygen react to produce nitric acid and water. The balanced chemical equation is: \[ NH_3(g) + 2O_2(g) \rightarrow HNO_3(g) + \text{H}_2\text{O}(g) \quad \Delta H = -330 \text{ kJ} \] **Thermodynamics:** To find the net change in enthalpy for the formation of one mole of nitric acid from these reactions: 1. Sum the enthalpy changes of the two reactions. 2. Express the result for the formation of one mole of nitric acid. **Calculation:** Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen, and oxygen. Round your answer to the nearest kJ. \[ \Delta H_{\text{net}} = \Delta H_1 + \Delta H_2 \] **Input:** \[ \text{Enter your answer in kJ:} \; \square \] --- **Note:** This lesson demonstrates the application of thermodynamics in chemical reactions, particularly in the synthesis of industrial chemicals like nitric acid, highlighting the conservation of energy principle.
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