Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![Lead(II) oxide can be reduced to form elemental lead through the reaction:
\[ \text{PbO}(s) + \text{C}(s) \rightarrow \text{Pb}(s) + \text{CO}(g) \]
Calculate \(\Delta H^\circ\) for the above reaction given the following (all values are at \(25^\circ \text{C}\)):](https://content.bartleby.com/qna-images/question/b3cca2f6-99a8-4436-ac34-ddd5c6eac033/6fbd5867-9249-495c-acc8-fec2ffd26ecf/21nv1yh_processed.png)
Transcribed Image Text:Lead(II) oxide can be reduced to form elemental lead through the reaction:
\[ \text{PbO}(s) + \text{C}(s) \rightarrow \text{Pb}(s) + \text{CO}(g) \]
Calculate \(\Delta H^\circ\) for the above reaction given the following (all values are at \(25^\circ \text{C}\)):
![**Thermochemical Equation Manipulation**
In this example, we will explore how to manipulate thermochemical equations to find the enthalpy change (\( \Delta H^\circ \)) for a given reaction.
1. **Reaction Equations and \(\Delta H^\circ\):**
- Equation 1:
\[
2 \, \text{CO}(g) + \cancel{\text{O}_2(g)} \rightarrow 2 \, \text{CO}_2(g) \quad \Delta H^\circ = -566.0 \, \text{kJ}
\]
- Equation 2:
\[
2 \, \text{NO}(g) \rightarrow \text{N}_2(g) + \cancel{\text{O}_2(g)} \quad \Delta H^\circ = -180.5 \, \text{kJ}
\]
2. **Overall Reaction:**
The overall chemical reaction is derived by combining the above equations and eliminating common species on both sides:
\[
2 \, \text{CO}(g) + 2 \, \text{NO}(g) \rightarrow 2 \, \text{CO}_2(g) + \text{N}_2(g)
\]
3. **Overall Enthalpy Change:**
The overall enthalpy change is the sum of the enthalpy changes from each individual reaction:
\[
\Delta H^\circ = -746.5 \, \text{kJ}
\]
This demonstrates the principle of Hess's Law, where the total enthalpy change is the sum of the enthalpy changes of individual steps, allowing you to calculate the enthalpy for a desired reaction from known values.](https://content.bartleby.com/qna-images/question/b3cca2f6-99a8-4436-ac34-ddd5c6eac033/6fbd5867-9249-495c-acc8-fec2ffd26ecf/bo78nyg_processed.png)
Transcribed Image Text:**Thermochemical Equation Manipulation**
In this example, we will explore how to manipulate thermochemical equations to find the enthalpy change (\( \Delta H^\circ \)) for a given reaction.
1. **Reaction Equations and \(\Delta H^\circ\):**
- Equation 1:
\[
2 \, \text{CO}(g) + \cancel{\text{O}_2(g)} \rightarrow 2 \, \text{CO}_2(g) \quad \Delta H^\circ = -566.0 \, \text{kJ}
\]
- Equation 2:
\[
2 \, \text{NO}(g) \rightarrow \text{N}_2(g) + \cancel{\text{O}_2(g)} \quad \Delta H^\circ = -180.5 \, \text{kJ}
\]
2. **Overall Reaction:**
The overall chemical reaction is derived by combining the above equations and eliminating common species on both sides:
\[
2 \, \text{CO}(g) + 2 \, \text{NO}(g) \rightarrow 2 \, \text{CO}_2(g) + \text{N}_2(g)
\]
3. **Overall Enthalpy Change:**
The overall enthalpy change is the sum of the enthalpy changes from each individual reaction:
\[
\Delta H^\circ = -746.5 \, \text{kJ}
\]
This demonstrates the principle of Hess's Law, where the total enthalpy change is the sum of the enthalpy changes of individual steps, allowing you to calculate the enthalpy for a desired reaction from known values.
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