2CIF (g) +O2 (g) → Cl20 (g) + F20 (g) 2CIF3 (g) + 202 (g) → Cl20 (g) +3F20 (g) AH°a = 341.4 kJ/mol 2F2 (g) + O2 (g) → 2F20 (g) AH° = 167.4 kJ/mol %3D %3D AH°g = -43.4 kJ/mol At the same temperature, use Hess' law to calculate AH° for the following reaction: CIF (g) +F2 (g) → CIF3 (g)
2CIF (g) +O2 (g) → Cl20 (g) + F20 (g) 2CIF3 (g) + 202 (g) → Cl20 (g) +3F20 (g) AH°a = 341.4 kJ/mol 2F2 (g) + O2 (g) → 2F20 (g) AH° = 167.4 kJ/mol %3D %3D AH°g = -43.4 kJ/mol At the same temperature, use Hess' law to calculate AH° for the following reaction: CIF (g) +F2 (g) → CIF3 (g)
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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At 25 °C, the following heats of reaction are known:
![### Thermochemical Calculations Using Hess's Law
#### Given Reactions and Their Enthalpy Changes:
1. **Reaction 1:**
\[ 2 \text{ClF (g)} + \text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text{O (g)} + \text{F}_2\text{O (g)} \]
\[ \Delta H^\circ = 167.4 \text{ kJ/mol} \]
2. **Reaction 2:**
\[ 2 \text{ClF}_3 \text{(g)} + 2\text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text{O (g)} + 3\text{F}_2\text{O (g)} \]
\[ \Delta H^\circ = 341.4 \text{ kJ/mol} \]
3. **Reaction 3:**
\[ 2\text{F}_2 \text{(g)} + \text{O}_2 \text{(g)} \rightarrow 2\text{F}_2\text{O (g)} \]
\[ \Delta H^\circ = -43.4 \text{ kJ/mol} \]
#### Problem Statement:
At the same temperature, use Hess's Law to calculate \(\Delta H^\circ\) for the following reaction:
\[ \text{ClF (g)} + \text{F}_2 \text{(g)} \rightarrow \text{ClF}_3 \text{(g)} \]
### Step-by-Step Solution:
Let’s denote the given reactions as follows:
- Reaction 1:
\[ 2 \text{ClF (g)} + \text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text{O (g)} + \text{F}_2\text{O (g)} \]
\[ \Delta H^\circ_1 = 167.4 \text{kJ/mol} \]
- Reaction 2:
\[ 2 \text{ClF}_3 \text{(g)} + 2 \text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe6b9d5aa-37b3-4cd7-947f-ee9211cbc626%2F7c0bdeec-b9ff-492e-9815-9bef5096593e%2Fsyoaapq.jpeg&w=3840&q=75)
Transcribed Image Text:### Thermochemical Calculations Using Hess's Law
#### Given Reactions and Their Enthalpy Changes:
1. **Reaction 1:**
\[ 2 \text{ClF (g)} + \text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text{O (g)} + \text{F}_2\text{O (g)} \]
\[ \Delta H^\circ = 167.4 \text{ kJ/mol} \]
2. **Reaction 2:**
\[ 2 \text{ClF}_3 \text{(g)} + 2\text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text{O (g)} + 3\text{F}_2\text{O (g)} \]
\[ \Delta H^\circ = 341.4 \text{ kJ/mol} \]
3. **Reaction 3:**
\[ 2\text{F}_2 \text{(g)} + \text{O}_2 \text{(g)} \rightarrow 2\text{F}_2\text{O (g)} \]
\[ \Delta H^\circ = -43.4 \text{ kJ/mol} \]
#### Problem Statement:
At the same temperature, use Hess's Law to calculate \(\Delta H^\circ\) for the following reaction:
\[ \text{ClF (g)} + \text{F}_2 \text{(g)} \rightarrow \text{ClF}_3 \text{(g)} \]
### Step-by-Step Solution:
Let’s denote the given reactions as follows:
- Reaction 1:
\[ 2 \text{ClF (g)} + \text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text{O (g)} + \text{F}_2\text{O (g)} \]
\[ \Delta H^\circ_1 = 167.4 \text{kJ/mol} \]
- Reaction 2:
\[ 2 \text{ClF}_3 \text{(g)} + 2 \text{O}_2 \text{(g)} \rightarrow \text{Cl}_2\text
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