Combustion reactions involve reacting a substance with oxygen. when compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C₂ H₂ (-1300. kJ/mol), C₂H6 (-1560. kJ/mol), and H₂ (-286 kJ/mol), calculate AH for the reaction ΔΗ = C₂H₂(g) + 2H₂(g) → C₂H6 (9) kj
Combustion reactions involve reacting a substance with oxygen. when compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C₂ H₂ (-1300. kJ/mol), C₂H6 (-1560. kJ/mol), and H₂ (-286 kJ/mol), calculate AH for the reaction ΔΗ = C₂H₂(g) + 2H₂(g) → C₂H6 (9) kj
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
![**Understanding Combustion Reactions**
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion, we can calculate the enthalpy change (ΔH) for different reactions.
Given enthalpies of combustion:
- **C₂H₂**: -1300 kJ/mol
- **C₂H₆**: -1560 kJ/mol
- **H₂**: -286 kJ/mol
**Problem: Calculate ΔH for the following reaction**
\[ C_2H_2(g) + 2H_2(g) \rightarrow C_2H_6(g) \]
\[
ΔH = \, \text{______}\, \text{kJ}
\]
**Steps to Calculate the Enthalpy Change (ΔH)**
1. **Write down the reaction in terms of moles and their respective enthalpies of combustion:**
\[
\text{Reactants:}\, C_2H_2(g)\, \text{and}\, 2H_2(g)
\]
\[
\text{Products:}\, C_2H_6(g)
\]
2. **Sum the enthalpies of combustion for the reactants:**
\[
ΔH_{reactants} = ΔH_{C₂H₂} + 2ΔH_{H₂}
\]
\[
ΔH_{reactants} = -1300\, \text{kJ/mol} + 2(-286\, \text{kJ/mol})
\]
\[
ΔH_{reactants} = -1300\, \text{kJ/mol} - 572\, \text{kJ/mol}
\]
\[
ΔH_{reactants} = -1872\, \text{kJ/mol}
\]
3. **Sum the enthalpy of combustion for the product:**
\[
ΔH_{products} = ΔH_{C₂H₆}
\]
\[
ΔH_{products} = -1560\, \text{kJ/mol}
\]
4. **Calculate the overall ΔH for the reaction:**
\[
ΔH = ΔH_{products} - ΔH_{reactants}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F216d8975-823a-443e-8abc-06f056adfa09%2F6a0c8a1c-4cb8-4c94-8ae2-6535ce8dd9d1%2F2czj05_processed.png&w=3840&q=75)
Transcribed Image Text:**Understanding Combustion Reactions**
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion, we can calculate the enthalpy change (ΔH) for different reactions.
Given enthalpies of combustion:
- **C₂H₂**: -1300 kJ/mol
- **C₂H₆**: -1560 kJ/mol
- **H₂**: -286 kJ/mol
**Problem: Calculate ΔH for the following reaction**
\[ C_2H_2(g) + 2H_2(g) \rightarrow C_2H_6(g) \]
\[
ΔH = \, \text{______}\, \text{kJ}
\]
**Steps to Calculate the Enthalpy Change (ΔH)**
1. **Write down the reaction in terms of moles and their respective enthalpies of combustion:**
\[
\text{Reactants:}\, C_2H_2(g)\, \text{and}\, 2H_2(g)
\]
\[
\text{Products:}\, C_2H_6(g)
\]
2. **Sum the enthalpies of combustion for the reactants:**
\[
ΔH_{reactants} = ΔH_{C₂H₂} + 2ΔH_{H₂}
\]
\[
ΔH_{reactants} = -1300\, \text{kJ/mol} + 2(-286\, \text{kJ/mol})
\]
\[
ΔH_{reactants} = -1300\, \text{kJ/mol} - 572\, \text{kJ/mol}
\]
\[
ΔH_{reactants} = -1872\, \text{kJ/mol}
\]
3. **Sum the enthalpy of combustion for the product:**
\[
ΔH_{products} = ΔH_{C₂H₆}
\]
\[
ΔH_{products} = -1560\, \text{kJ/mol}
\]
4. **Calculate the overall ΔH for the reaction:**
\[
ΔH = ΔH_{products} - ΔH_{reactants}
![### Thermochemical Data and Reaction Enthalpies
Given the following data:
1. \( 2 \text{ClF}(g) + \text{O}_2(g) \rightarrow \text{Cl}_2 \text{O}(g) + \text{F}_2 \text{O}(g) \)
- \( \Delta H = 167.4 \text{ kJ} \)
2. \( 2 \text{ClF}_3(g) + 2 \text{O}_2(g) \rightarrow \text{Cl}_2 \text{O}(g) + 3 \text{F}_2 \text{O}(g) \)
- \( \Delta H = 341.4 \text{ kJ} \)
3. \( 2 \text{F}_2(g) + \text{O}_2(g) \rightarrow 2 \text{F}_2 \text{O}(g) \)
- \( \Delta H = -43.4 \text{ kJ} \)
### Problem Statement
Calculate \( \Delta H \) for the reaction:
\[ \text{ClF}(g) + \text{F}_2(g) \rightarrow \text{ClF}_3(g) \]
### Solution
INSERT CALCULATION PROCESS
### Answer
\[ \Delta H = \_\_\_\_\_\_ \text{ kJ} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F216d8975-823a-443e-8abc-06f056adfa09%2F6a0c8a1c-4cb8-4c94-8ae2-6535ce8dd9d1%2Fhazgpl_processed.png&w=3840&q=75)
Transcribed Image Text:### Thermochemical Data and Reaction Enthalpies
Given the following data:
1. \( 2 \text{ClF}(g) + \text{O}_2(g) \rightarrow \text{Cl}_2 \text{O}(g) + \text{F}_2 \text{O}(g) \)
- \( \Delta H = 167.4 \text{ kJ} \)
2. \( 2 \text{ClF}_3(g) + 2 \text{O}_2(g) \rightarrow \text{Cl}_2 \text{O}(g) + 3 \text{F}_2 \text{O}(g) \)
- \( \Delta H = 341.4 \text{ kJ} \)
3. \( 2 \text{F}_2(g) + \text{O}_2(g) \rightarrow 2 \text{F}_2 \text{O}(g) \)
- \( \Delta H = -43.4 \text{ kJ} \)
### Problem Statement
Calculate \( \Delta H \) for the reaction:
\[ \text{ClF}(g) + \text{F}_2(g) \rightarrow \text{ClF}_3(g) \]
### Solution
INSERT CALCULATION PROCESS
### Answer
\[ \Delta H = \_\_\_\_\_\_ \text{ kJ} \]
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