Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) → 2NH₂(g) In the second step, ammonia and oxygen react to form nitric oxide and water: 4 NH3(g) + 50₂(g) 4 NO(g) + 6H₂O(g) ΔΗ= -905, kJ Calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. kJ - X AH=-92. KJ 5
Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) → 2NH₂(g) In the second step, ammonia and oxygen react to form nitric oxide and water: 4 NH3(g) + 50₂(g) 4 NO(g) + 6H₂O(g) ΔΗ= -905, kJ Calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. kJ - X AH=-92. KJ 5
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 88SCQ
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### Formation of Nitric Oxide (NO)
Nitric oxide (NO) can be formed from nitrogen, hydrogen, and oxygen in two steps. Let's explore these steps in detail.
#### Step 1: Formation of Ammonia
In the first step, nitrogen and hydrogen react to form ammonia:
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \quad \Delta H = -92 \, \text{kJ} \]
#### Step 2: Formation of Nitric Oxide and Water
In the second step, ammonia and oxygen react to form nitric oxide and water:
\[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \quad \Delta H = -905 \, \text{kJ} \]
#### Calculation
Calculate the net change in enthalpy for the formation of **one mole** of nitric oxide from nitrogen, hydrogen, and oxygen from these reactions. Round your answer to the nearest kJ.
**Answer:**
[ \( \boxed{kJ} \) ]
*Hint: Consider the enthalpy changes involved in both steps and remember that the formation of 4 moles of NO is calculated in step 2.*
---
### Explanation of the Given Information
The image contains:
- Chemical equations with their respective enthalpy changes (ΔH) indicating the heat released or absorbed during the reactions.
- A computational form field for entering the final answer in kilojoules (kJ).
### Step-by-Step Calculation Guide
1. **Identify the Enthalpy Changes:**
- For the first reaction: ΔH = -92 kJ.
- For the second reaction: ΔH = -905 kJ.
2. **Analyze the Reactions:**
- The first reaction produces 2 moles of NH₃ from 1 mole of N₂ and 3 moles of H₂.
- The second reaction uses 4 moles of NH₃ to produce 4 moles of NO.
3. **Determine Enthalpy for One Mole of NO:**
- Since the second reaction yields 4 m](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F11fddf9f-a89a-44ba-8382-9c550e4fed12%2F65c55f4d-3094-4f2e-ba43-8eaf2f821f5e%2Feamj7ri_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Sure, here is the transcription formatted for an educational website:
---
### Formation of Nitric Oxide (NO)
Nitric oxide (NO) can be formed from nitrogen, hydrogen, and oxygen in two steps. Let's explore these steps in detail.
#### Step 1: Formation of Ammonia
In the first step, nitrogen and hydrogen react to form ammonia:
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightarrow 2\text{NH}_3(g) \quad \Delta H = -92 \, \text{kJ} \]
#### Step 2: Formation of Nitric Oxide and Water
In the second step, ammonia and oxygen react to form nitric oxide and water:
\[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \quad \Delta H = -905 \, \text{kJ} \]
#### Calculation
Calculate the net change in enthalpy for the formation of **one mole** of nitric oxide from nitrogen, hydrogen, and oxygen from these reactions. Round your answer to the nearest kJ.
**Answer:**
[ \( \boxed{kJ} \) ]
*Hint: Consider the enthalpy changes involved in both steps and remember that the formation of 4 moles of NO is calculated in step 2.*
---
### Explanation of the Given Information
The image contains:
- Chemical equations with their respective enthalpy changes (ΔH) indicating the heat released or absorbed during the reactions.
- A computational form field for entering the final answer in kilojoules (kJ).
### Step-by-Step Calculation Guide
1. **Identify the Enthalpy Changes:**
- For the first reaction: ΔH = -92 kJ.
- For the second reaction: ΔH = -905 kJ.
2. **Analyze the Reactions:**
- The first reaction produces 2 moles of NH₃ from 1 mole of N₂ and 3 moles of H₂.
- The second reaction uses 4 moles of NH₃ to produce 4 moles of NO.
3. **Determine Enthalpy for One Mole of NO:**
- Since the second reaction yields 4 m
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