The equations given in the problem introduction can be added together to give the following reaction: overall: C + 02→CO However, one of them must be reversed. Which one?
The equations given in the problem introduction can be added together to give the following reaction: overall: C + 02→CO However, one of them must be reversed. Which one?
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
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 61PS: The standard enthalpy of formation of solid barium oxide, BaO, is 553.5 kJ/mol, and the standard...
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Please answer question 10 part A
![## Learning Goal:
To understand how to use Hess's law to find the enthalpy of an overall reaction.
### Hess’s Law:
The change in enthalpy, \( \Delta H \), is the heat absorbed or produced during any reaction at constant pressure. Hess's law states that \( \Delta H \) for an overall reaction is the sum of the \( \Delta H \) values for the individual reactions. For example, if we wanted to know the enthalpy change for the reaction:
\[ 3\text{Mn} + 3\text{O}_2 \rightarrow 3\text{MnO}_2 \]
we could calculate it using the enthalpy values for the following individual steps:
- **Step 1**: \( 4\text{Al} + 3\text{O}_2 \rightarrow 2\text{Al}_2\text{O}_3 \)
- **Step 2**: \( 3\text{Mn} + 2\text{Al}_2\text{O}_3 \rightarrow 3\text{MnO}_2 + 4\text{Al} \)
**Overall**: \( 3\text{Mn} + 3\text{O}_2 \rightarrow 3\text{MnO}_2 \)
If the enthalpy change is \( -3352 \, \text{kJ/mol} \) for step 1 and \( 1792 \, \text{kJ/mol} \) for step 2, then the enthalpy change for the overall reaction is calculated as follows:
\[
\Delta H = -3352 + 1792 = -1560 \, \text{kJ/mol}
\]
It is also significant to note that the change in enthalpy is a state function, meaning it is independent of path. In other words, the sum of the \( \Delta H \) values for any set of reactions that produce the desired product from the starting materials gives the same overall \( \Delta H \).
---
### Now consider the following set of reactions:
1. \( \text{CO} + \frac{1}{2}\text{O}_2 \rightarrow \text{CO}_2 \), \( \Delta H = -283 \, \text{kJ/mol} \)
2. \( \text{C} + \text{O}_2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fded90a0e-1aa2-42d3-8902-387fb21746ad%2F1a86a2ab-5900-4866-b868-b89f96a12759%2F86tdzh4_processed.png&w=3840&q=75)
Transcribed Image Text:## Learning Goal:
To understand how to use Hess's law to find the enthalpy of an overall reaction.
### Hess’s Law:
The change in enthalpy, \( \Delta H \), is the heat absorbed or produced during any reaction at constant pressure. Hess's law states that \( \Delta H \) for an overall reaction is the sum of the \( \Delta H \) values for the individual reactions. For example, if we wanted to know the enthalpy change for the reaction:
\[ 3\text{Mn} + 3\text{O}_2 \rightarrow 3\text{MnO}_2 \]
we could calculate it using the enthalpy values for the following individual steps:
- **Step 1**: \( 4\text{Al} + 3\text{O}_2 \rightarrow 2\text{Al}_2\text{O}_3 \)
- **Step 2**: \( 3\text{Mn} + 2\text{Al}_2\text{O}_3 \rightarrow 3\text{MnO}_2 + 4\text{Al} \)
**Overall**: \( 3\text{Mn} + 3\text{O}_2 \rightarrow 3\text{MnO}_2 \)
If the enthalpy change is \( -3352 \, \text{kJ/mol} \) for step 1 and \( 1792 \, \text{kJ/mol} \) for step 2, then the enthalpy change for the overall reaction is calculated as follows:
\[
\Delta H = -3352 + 1792 = -1560 \, \text{kJ/mol}
\]
It is also significant to note that the change in enthalpy is a state function, meaning it is independent of path. In other words, the sum of the \( \Delta H \) values for any set of reactions that produce the desired product from the starting materials gives the same overall \( \Delta H \).
---
### Now consider the following set of reactions:
1. \( \text{CO} + \frac{1}{2}\text{O}_2 \rightarrow \text{CO}_2 \), \( \Delta H = -283 \, \text{kJ/mol} \)
2. \( \text{C} + \text{O}_2
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