Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.429-g sample of biphenyl (C12H10) in a bomb calorimeter containing 1170. g of water. The temperature increases from 26.00 °C to 29.00 °C. The heat capacity of water is 4.184 Jgl°C-1. Water The molar heat of combustion is -6251 kJ per mole of biphenyl. C12H10(s) + 29/2 O2(g) →12 CO2(g) + 5 H2O(1) + Energy Calculate the heat capacity of the calorimeter. Insulated outside Sample dish Burning sample heat capacity of calorimeter J/°C Steel bomb nhomber
Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.429-g sample of biphenyl (C12H10) in a bomb calorimeter containing 1170. g of water. The temperature increases from 26.00 °C to 29.00 °C. The heat capacity of water is 4.184 Jgl°C-1. Water The molar heat of combustion is -6251 kJ per mole of biphenyl. C12H10(s) + 29/2 O2(g) →12 CO2(g) + 5 H2O(1) + Energy Calculate the heat capacity of the calorimeter. Insulated outside Sample dish Burning sample heat capacity of calorimeter J/°C Steel bomb nhomber
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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 112AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each...
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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.
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![### Understanding Bomb Calorimetry
A **bomb calorimeter**, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as **calibrating the calorimeter**.
#### Laboratory Experiment Example
In the laboratory, a student burns a **0.429-g sample of biphenyl (C₁₂H₁₀)** in a bomb calorimeter containing **1170. g of water**. The temperature increases from **26.00 °C** to **29.00 °C**. The heat capacity of water is **4.184 J g⁻¹°C⁻¹**.
The molar heat of combustion is **–6251 kJ per mole** of biphenyl.
The chemical equation for this reaction is:
\[ \text{C}_{12}\text{H}_{10}(s) + \frac{29}{2} \text{O}_2(g) \rightarrow 12 \text{CO}_2(g) + 5 \text{H}_2\text{O}(l) + \text{Energy} \]
Calculate the heat capacity of the calorimeter.
\[ \text{heat capacity of calorimeter} = \_\_\_\_\_\_\_\_\_ \text{ J/°C} \]
### Diagram Explanation
The diagram on the right shows the internal structure of a combustion (bomb) calorimeter. Here's a detailed explanation:
- **Ignition Wires:** Deliver an electrical spark to ignite the fuel sample.
- **Thermometer:** Measures the temperature change in the water.
- **Stirrer:** Ensures even heat distribution in the water.
- **Water:** Surrounds the sample, absorbing the heat released from the combustion.
- **Sample Dish:** Holds the sample to be combusted.
- **Burning Sample:** The sample that is combusted to measure its heat of combustion.
- **Steel Bomb:** The robust container where the combustion reaction takes place.
- **Insulated Outside Chamber:** Minimizes heat exchange with the surroundings, ensuring accurate measurements.
#### Calorimeter Setup
The sample is placed in the sample dish inside the steel bomb, which is then filled with oxygen. The bomb is sealed and placed in the insulated chamber filled with](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86b14285-d986-492a-886d-db2235fe87ed%2F441415a2-75f2-480b-b405-e1ea378b1b0d%2Fc10wrp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Understanding Bomb Calorimetry
A **bomb calorimeter**, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as **calibrating the calorimeter**.
#### Laboratory Experiment Example
In the laboratory, a student burns a **0.429-g sample of biphenyl (C₁₂H₁₀)** in a bomb calorimeter containing **1170. g of water**. The temperature increases from **26.00 °C** to **29.00 °C**. The heat capacity of water is **4.184 J g⁻¹°C⁻¹**.
The molar heat of combustion is **–6251 kJ per mole** of biphenyl.
The chemical equation for this reaction is:
\[ \text{C}_{12}\text{H}_{10}(s) + \frac{29}{2} \text{O}_2(g) \rightarrow 12 \text{CO}_2(g) + 5 \text{H}_2\text{O}(l) + \text{Energy} \]
Calculate the heat capacity of the calorimeter.
\[ \text{heat capacity of calorimeter} = \_\_\_\_\_\_\_\_\_ \text{ J/°C} \]
### Diagram Explanation
The diagram on the right shows the internal structure of a combustion (bomb) calorimeter. Here's a detailed explanation:
- **Ignition Wires:** Deliver an electrical spark to ignite the fuel sample.
- **Thermometer:** Measures the temperature change in the water.
- **Stirrer:** Ensures even heat distribution in the water.
- **Water:** Surrounds the sample, absorbing the heat released from the combustion.
- **Sample Dish:** Holds the sample to be combusted.
- **Burning Sample:** The sample that is combusted to measure its heat of combustion.
- **Steel Bomb:** The robust container where the combustion reaction takes place.
- **Insulated Outside Chamber:** Minimizes heat exchange with the surroundings, ensuring accurate measurements.
#### Calorimeter Setup
The sample is placed in the sample dish inside the steel bomb, which is then filled with oxygen. The bomb is sealed and placed in the insulated chamber filled with
![**Bomb Calorimeter**
**A bomb calorimeter**, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as **calibrating** the calorimeter.
In the laboratory, a student burns a **0.434-g** sample of **bisphenol A (C₁₅H₁₆O₂)** in a bomb calorimeter containing **1010 g of water.** The temperature increases from **24.20 °C to 27.10 °C**. The heat capacity of water is **4.184 J g⁻¹°C⁻¹**.
The molar heat of combustion is **-7821 kJ per mole of bisphenol A**.
\[ C_{15}H_{16}O_{2}(s) + 18 O_{2}(g) \longrightarrow 15 CO_{2}(g) + 8 H_2O(l) + \text{Energy} \]
Calculate the heat capacity of the calorimeter.
\[ \text{heat capacity of calorimeter} = \boxed{ \ \ \ \ } \text{J/°C} \]
**Diagram Explanation:**
The diagram to the right shows a **Combustion (bomb) calorimeter** with the following components:
1. **Ignition wires heat sample**: Wires used to ignite the sample in the bomb.
2. **Stirrer**: Ensures uniform temperature distribution in the water.
3. **Thermometer**: Measures the temperature of the water.
4. **Insulated outside chamber**: Minimizes heat loss to the surroundings.
5. **Sample dish**: Holds the sample to be combusted.
6. **Burning sample**: The substance undergoing combustion.
7. **Steel bomb**: Contains the reaction to ensure constant volume.
8. **Water**: Absorbs the heat from the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86b14285-d986-492a-886d-db2235fe87ed%2F441415a2-75f2-480b-b405-e1ea378b1b0d%2F310b7s8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Bomb Calorimeter**
**A bomb calorimeter**, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as **calibrating** the calorimeter.
In the laboratory, a student burns a **0.434-g** sample of **bisphenol A (C₁₅H₁₆O₂)** in a bomb calorimeter containing **1010 g of water.** The temperature increases from **24.20 °C to 27.10 °C**. The heat capacity of water is **4.184 J g⁻¹°C⁻¹**.
The molar heat of combustion is **-7821 kJ per mole of bisphenol A**.
\[ C_{15}H_{16}O_{2}(s) + 18 O_{2}(g) \longrightarrow 15 CO_{2}(g) + 8 H_2O(l) + \text{Energy} \]
Calculate the heat capacity of the calorimeter.
\[ \text{heat capacity of calorimeter} = \boxed{ \ \ \ \ } \text{J/°C} \]
**Diagram Explanation:**
The diagram to the right shows a **Combustion (bomb) calorimeter** with the following components:
1. **Ignition wires heat sample**: Wires used to ignite the sample in the bomb.
2. **Stirrer**: Ensures uniform temperature distribution in the water.
3. **Thermometer**: Measures the temperature of the water.
4. **Insulated outside chamber**: Minimizes heat loss to the surroundings.
5. **Sample dish**: Holds the sample to be combusted.
6. **Burning sample**: The substance undergoing combustion.
7. **Steel bomb**: Contains the reaction to ensure constant volume.
8. **Water**: Absorbs the heat from the reaction.
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