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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![**Transcription for Educational Website:**
---
**Topic: Thermodynamics and Enthalpy Change**
**Problem 2: Using Hess's Law to Calculate Enthalpy Change**
Given Reactions:
1. \( A \rightarrow B \) with \(\Delta H = +20 \text{ kJ}\)
2. \( C \rightarrow B \) with \(\Delta H = +80 \text{ kJ}\)
**Objective:** Calculate the enthalpy change for the reaction \( A \rightarrow C \).
**Solution Approach:**
- Apply Hess's Law, which states that the total enthalpy change in a chemical reaction is the same regardless of the pathway taken, provided the initial and final conditions are the same.
- From Hess's Law, to find the enthalpy change for \( A \rightarrow C \), we need to reverse the second reaction:
\[
B \rightarrow C \quad \text{with} \quad \Delta H = -80 \text{ kJ}
\]
- Combine the pathways:
\[
\begin{align*}
A \rightarrow B & \quad \Delta H = +20 \text{ kJ}, \\
B \rightarrow C & \quad \Delta H = -80 \text{ kJ}.
\end{align*}
\]
- Total \(\Delta H\) for \( A \rightarrow C \):
\[
\Delta H = (+20 \text{ kJ}) + (-80 \text{ kJ}) = -60 \text{ kJ}
\]
Thus, the enthalpy change for the reaction \( A \rightarrow C \) is \(-60 \text{ kJ}\).
---
**Source:** Problem Set 5 - Chapter 5
(Note: This transcription represents the specified section of the educational document. The content offers a clear explanation of applying Hess's Law in calculating enthalpy changes for chemical reactions.)
---](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd7374a00-925b-4659-a7ff-f60a4e3f7577%2F25d4d8aa-6507-4aa6-8213-e30b989bc9bd%2Fwdjpx8g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website:**
---
**Topic: Thermodynamics and Enthalpy Change**
**Problem 2: Using Hess's Law to Calculate Enthalpy Change**
Given Reactions:
1. \( A \rightarrow B \) with \(\Delta H = +20 \text{ kJ}\)
2. \( C \rightarrow B \) with \(\Delta H = +80 \text{ kJ}\)
**Objective:** Calculate the enthalpy change for the reaction \( A \rightarrow C \).
**Solution Approach:**
- Apply Hess's Law, which states that the total enthalpy change in a chemical reaction is the same regardless of the pathway taken, provided the initial and final conditions are the same.
- From Hess's Law, to find the enthalpy change for \( A \rightarrow C \), we need to reverse the second reaction:
\[
B \rightarrow C \quad \text{with} \quad \Delta H = -80 \text{ kJ}
\]
- Combine the pathways:
\[
\begin{align*}
A \rightarrow B & \quad \Delta H = +20 \text{ kJ}, \\
B \rightarrow C & \quad \Delta H = -80 \text{ kJ}.
\end{align*}
\]
- Total \(\Delta H\) for \( A \rightarrow C \):
\[
\Delta H = (+20 \text{ kJ}) + (-80 \text{ kJ}) = -60 \text{ kJ}
\]
Thus, the enthalpy change for the reaction \( A \rightarrow C \) is \(-60 \text{ kJ}\).
---
**Source:** Problem Set 5 - Chapter 5
(Note: This transcription represents the specified section of the educational document. The content offers a clear explanation of applying Hess's Law in calculating enthalpy changes for chemical reactions.)
---
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