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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Question
Consider the first three written formulas, and then use Hess’ law to find the change in enthalpy , ΔH° , at 25°C for the written equation.
![### Chemical Reactions and Their Energies
This section examines several chemical reactions involving chlorine monofluoride (ClF), oxygen (O₂), and fluorine (F₂), alongside their respective enthalpy changes (ΔH).
1. **Reaction 1:**
\[
2 \text{ClF} + \text{O}_2 \rightarrow \text{F}_2\text{O} \quad \Delta H = 167.4 \text{ kJ/mol}
\]
In this reaction, chlorine monofluoride (ClF) reacts with oxygen (O₂) to form oxygen difluoride (F₂O). The reaction releases 167.4 kJ of energy per mole.
2. **Reaction 2:**
\[
2 \text{ClF} + 2 \text{O}_2 (\text{g}) \rightarrow \text{Cl}_2\text{O} + 3 \text{F}_2\text{O} \quad \Delta H = 341.2 \text{ kJ/mol}
\]
Here, chlorine monofluoride (ClF) reacts with gaseous oxygen (O₂) to produce dichlorine monoxide (Cl₂O) and three moles of oxygen difluoride (F₂O). This reaction releases 341.2 kJ of energy per mole.
3. **Reaction 3:**
\[
2 \text{F}_2 + \text{O}_2 \rightarrow 2 \text{F}_2\text{O} \quad \Delta H = -43.4 \text{ kJ/mol}
\]
In this reaction, fluorine (F₂) reacts with oxygen (O₂) to form oxygen difluoride (F₂O). The reaction absorbs 43.4 kJ of energy per mole.
4. **Decomposition Reaction:**
\[
\text{Equation}: \text{ClF}_3 \rightarrow \text{ClF} + \text{F}_2
\]
The decomposition of chlorine trifluoride (ClF₃) into chlorine monofluoride (ClF) and fluorine (F₂) is described, though the energy change is not specified in this reaction.
These reactions provide insights into the energetic changes accompanying the chemical transformations](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F61b74698-3f34-41c6-b209-082ec83323f3%2F8567951d-8dae-4efd-9297-a22e9f9d9301%2F5mc03no_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemical Reactions and Their Energies
This section examines several chemical reactions involving chlorine monofluoride (ClF), oxygen (O₂), and fluorine (F₂), alongside their respective enthalpy changes (ΔH).
1. **Reaction 1:**
\[
2 \text{ClF} + \text{O}_2 \rightarrow \text{F}_2\text{O} \quad \Delta H = 167.4 \text{ kJ/mol}
\]
In this reaction, chlorine monofluoride (ClF) reacts with oxygen (O₂) to form oxygen difluoride (F₂O). The reaction releases 167.4 kJ of energy per mole.
2. **Reaction 2:**
\[
2 \text{ClF} + 2 \text{O}_2 (\text{g}) \rightarrow \text{Cl}_2\text{O} + 3 \text{F}_2\text{O} \quad \Delta H = 341.2 \text{ kJ/mol}
\]
Here, chlorine monofluoride (ClF) reacts with gaseous oxygen (O₂) to produce dichlorine monoxide (Cl₂O) and three moles of oxygen difluoride (F₂O). This reaction releases 341.2 kJ of energy per mole.
3. **Reaction 3:**
\[
2 \text{F}_2 + \text{O}_2 \rightarrow 2 \text{F}_2\text{O} \quad \Delta H = -43.4 \text{ kJ/mol}
\]
In this reaction, fluorine (F₂) reacts with oxygen (O₂) to form oxygen difluoride (F₂O). The reaction absorbs 43.4 kJ of energy per mole.
4. **Decomposition Reaction:**
\[
\text{Equation}: \text{ClF}_3 \rightarrow \text{ClF} + \text{F}_2
\]
The decomposition of chlorine trifluoride (ClF₃) into chlorine monofluoride (ClF) and fluorine (F₂) is described, though the energy change is not specified in this reaction.
These reactions provide insights into the energetic changes accompanying the chemical transformations
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