Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Estimation of the Enthalpy of Combustion of Anthracene
**Problem Statement:**
When 1.022 g of anthracene, \( \text{C}_{14}\text{H}_{10} \), is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 25.65°C. Assuming that the specific heat of water is 4.18 J/(g·°C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene (kJ/mol).
**Calculations:**
1. **Determine the heat absorbed by the water (\( q \)):**
\[ q = m \cdot c \cdot \Delta T \]
Where:
- \( m \) = mass of water (500.0 g)
- \( c \) = specific heat of water (4.18 J/(g·°C))
- \( \Delta T \) = temperature change (25.65°C)
\[ q = 500.0 \, \text{g} \cdot 4.18 \, \frac{\text{J}}{\text{g·°C}} \cdot 25.65 \, \text{°C} \]
2. **Convert the heat absorbed by the water to kilojoules (kJ):**
\[ q \text{(in kJ)} = q \text{(in J)} \times \frac{1 \, \text{kJ}}{1000 \, \text{J}} \]
3. **Determine moles of anthracene combusted:**
\[ \text{Moles of anthracene} = \frac{1.022 \, \text{g}}{\text{Molecular weight of } \text{C}_{14}\text{H}_{10}} \]
The molecular weight of anthracene (\( \text{C}_{14}\text{H}_{10} \)):
\[ 14 \times 12.01 \, \text{g/mol} + 10 \times 1.008 \, \text{g/mol} = 178.23 \, \text{g/mol} \]
4. **Convert the heat absorbed by the water to per mole of anthracene:**
\[ \](https://content.bartleby.com/qna-images/question/7b0fedb7-adbc-492c-aa14-9f5d12342848/c0763564-3ec1-4d22-aa4c-b157edaff047/pmx9wq_processed.png)
Transcribed Image Text:### Estimation of the Enthalpy of Combustion of Anthracene
**Problem Statement:**
When 1.022 g of anthracene, \( \text{C}_{14}\text{H}_{10} \), is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 25.65°C. Assuming that the specific heat of water is 4.18 J/(g·°C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene (kJ/mol).
**Calculations:**
1. **Determine the heat absorbed by the water (\( q \)):**
\[ q = m \cdot c \cdot \Delta T \]
Where:
- \( m \) = mass of water (500.0 g)
- \( c \) = specific heat of water (4.18 J/(g·°C))
- \( \Delta T \) = temperature change (25.65°C)
\[ q = 500.0 \, \text{g} \cdot 4.18 \, \frac{\text{J}}{\text{g·°C}} \cdot 25.65 \, \text{°C} \]
2. **Convert the heat absorbed by the water to kilojoules (kJ):**
\[ q \text{(in kJ)} = q \text{(in J)} \times \frac{1 \, \text{kJ}}{1000 \, \text{J}} \]
3. **Determine moles of anthracene combusted:**
\[ \text{Moles of anthracene} = \frac{1.022 \, \text{g}}{\text{Molecular weight of } \text{C}_{14}\text{H}_{10}} \]
The molecular weight of anthracene (\( \text{C}_{14}\text{H}_{10} \)):
\[ 14 \times 12.01 \, \text{g/mol} + 10 \times 1.008 \, \text{g/mol} = 178.23 \, \text{g/mol} \]
4. **Convert the heat absorbed by the water to per mole of anthracene:**
\[ \
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