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What is the enthalpy for reaction 1 reversed? reaction 1 reversed: CO2¬CO + ¿O2

What is the enthalpy for reaction 1 reversed? reaction 1 reversed: CO2¬CO + ¿O2

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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To understand how to use Hess's law to find the enthalpy of an overall reaction: 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 important to note that the change in enthalpy is a state function, meaning it is independent of the 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 \( \Delta H \).
Transcribed Image Text:To understand how to use Hess's law to find the enthalpy of an overall reaction: 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 important to note that the change in enthalpy is a state function, meaning it is independent of the 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 \( \Delta H \).
**Title: Understanding Enthalpy Change in Reversed Chemical Reactions** **Introduction:** In this lesson, we will explore how to determine the enthalpy for a reversed chemical reaction. Specifically, we'll examine a reaction where carbon dioxide (CO₂) is converted to carbon monoxide (CO) and half a molecule of oxygen (O₂). **Reaction Details:** - **Original Reaction:** This is the typical format where substances react to form products. - **Reversed Reaction:** \( \text{CO}_2 \rightarrow \text{CO} + \frac{1}{2}\text{O}_2 \) In this reversed reaction, carbon dioxide is decomposed into carbon monoxide and oxygen. **Key Concepts:** 1. **Enthalpy (ΔH):** A measure of the total heat content in a system. It is a crucial factor in predicting the energy changes in a reaction. 2. **Reversing Reaction Effects:** - When a reaction is reversed, the sign of the enthalpy change (ΔH) also reverses. This reflects the energy absorbed or released during the process of decomposition versus formation. **Conclusion:** To find the enthalpy change for the reversed reaction, simply take the negative of the enthalpy change of the original reaction. This approach helps in understanding energy flow and stability in chemical processes. This lesson provides foundational knowledge for exploring thermodynamic principles in chemical reactions.
Transcribed Image Text:**Title: Understanding Enthalpy Change in Reversed Chemical Reactions** **Introduction:** In this lesson, we will explore how to determine the enthalpy for a reversed chemical reaction. Specifically, we'll examine a reaction where carbon dioxide (CO₂) is converted to carbon monoxide (CO) and half a molecule of oxygen (O₂). **Reaction Details:** - **Original Reaction:** This is the typical format where substances react to form products. - **Reversed Reaction:** \( \text{CO}_2 \rightarrow \text{CO} + \frac{1}{2}\text{O}_2 \) In this reversed reaction, carbon dioxide is decomposed into carbon monoxide and oxygen. **Key Concepts:** 1. **Enthalpy (ΔH):** A measure of the total heat content in a system. It is a crucial factor in predicting the energy changes in a reaction. 2. **Reversing Reaction Effects:** - When a reaction is reversed, the sign of the enthalpy change (ΔH) also reverses. This reflects the energy absorbed or released during the process of decomposition versus formation. **Conclusion:** To find the enthalpy change for the reversed reaction, simply take the negative of the enthalpy change of the original reaction. This approach helps in understanding energy flow and stability in chemical processes. This lesson provides foundational knowledge for exploring thermodynamic principles in chemical reactions.
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