Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Understanding Enthalpy Change Calculation Using Hess's Law**
To find the enthalpy change (ΔH) for the following reaction:
\[ \text{Equation 4:} \quad 2 \, \text{N}_2(g) + 5 \, \text{O}_2(g) \rightarrow 2 \, \text{N}_2\text{O}_5(g) \quad \Delta H = \, ??????? \]
We need to use the given equations and their enthalpy changes:
1. **Equation 1:**
\[ 2 \, \text{H}_2\text{O}(l) \rightarrow 2 \, \text{H}_2(g) + \text{O}_2(g) \quad \Delta H = 571.6 \, \text{kJ} \]
2. **Equation 2:**
\[ \text{N}_2\text{O}_5(g) + \text{H}_2\text{O}(l) \rightarrow 2 \, \text{HNO}_3(l) \quad \Delta H = -73.7 \, \text{kJ} \]
3. **Equation 3:**
\[ 2 \, \text{H}_2(g) + 6 \, \text{O}_2(g) + 2 \, \text{N}_2(g) \rightarrow 4 \, \text{HNO}_3(l) \quad \Delta H = -696.4 \, \text{kJ} \]
### Steps to Determine ΔH for Equation 4:
To calculate the ΔH for Equation 4, you must manipulate these equations following Hess's Law. Here are your options:
- Flip Equation 1 only
- Flip Equation 2 only
- Flip Equation 3 only
- Flip Equation 1 and Equation 2 only
- Flip Equation 1 and Equation 3 only
- Flip Equation 2 and Equation 3 only
- Flip no equation
Consider the stoichiometry and the resulting target equation to choose the correct options.](https://content.bartleby.com/qna-images/question/80bd6999-b702-4bab-9a9d-3d78c3747c19/bd375625-9a99-447a-891f-1e561dd3d30f/rvn9d3_processed.jpeg)
Transcribed Image Text:**Understanding Enthalpy Change Calculation Using Hess's Law**
To find the enthalpy change (ΔH) for the following reaction:
\[ \text{Equation 4:} \quad 2 \, \text{N}_2(g) + 5 \, \text{O}_2(g) \rightarrow 2 \, \text{N}_2\text{O}_5(g) \quad \Delta H = \, ??????? \]
We need to use the given equations and their enthalpy changes:
1. **Equation 1:**
\[ 2 \, \text{H}_2\text{O}(l) \rightarrow 2 \, \text{H}_2(g) + \text{O}_2(g) \quad \Delta H = 571.6 \, \text{kJ} \]
2. **Equation 2:**
\[ \text{N}_2\text{O}_5(g) + \text{H}_2\text{O}(l) \rightarrow 2 \, \text{HNO}_3(l) \quad \Delta H = -73.7 \, \text{kJ} \]
3. **Equation 3:**
\[ 2 \, \text{H}_2(g) + 6 \, \text{O}_2(g) + 2 \, \text{N}_2(g) \rightarrow 4 \, \text{HNO}_3(l) \quad \Delta H = -696.4 \, \text{kJ} \]
### Steps to Determine ΔH for Equation 4:
To calculate the ΔH for Equation 4, you must manipulate these equations following Hess's Law. Here are your options:
- Flip Equation 1 only
- Flip Equation 2 only
- Flip Equation 3 only
- Flip Equation 1 and Equation 2 only
- Flip Equation 1 and Equation 3 only
- Flip Equation 2 and Equation 3 only
- Flip no equation
Consider the stoichiometry and the resulting target equation to choose the correct options.
Transcribed Image Text:**Consider the problem below:**
*(Equation 1)* \(2 \, \text{H}_2\text{O}_{(l)} \rightarrow 2 \, \text{H}_2_{(g)} + \text{O}_2_{(g)} \) \(\Delta H = 571.6 \, \text{kJ}\)
*(Equation 2)* \(\text{N}_2\text{O}_5_{(g)} + \text{H}_2\text{O}_{(l)} \rightarrow 2 \, \text{HNO}_3_{(l)} \) \(\Delta H = -73.7 \, \text{kJ}\)
*(Equation 3)* \(2 \, \text{H}_2_{(g)} + 6 \, \text{O}_2_{(g)} + 2 \, \text{N}_2_{(g)} \rightarrow 4 \, \text{HNO}_3_{(l)} \) \(\Delta H = -696.4 \, \text{kJ}\)
*(Equation 4)* \(2 \, \text{N}_2_{(g)} + 5 \, \text{O}_2_{(g)} \rightarrow 2 \, \text{N}_2\text{O}_5_{(g)} \) \(\Delta H = ???????\)
To find \(\Delta H\) for equation 4, you must:
- **Options:**
- Flip equation 1 only
- Flip equation 2 only
- Flip equation 3 only
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