Complete Combustion Of A $0.600 \, \text{g}$ Sample Of A Compound In A Bomb Calorimeter Releases Energy. The Calorimeter Has A Mass Of $1.30 \, \text{kg}$ And A Specific Heat Of $3.41 \, \text{J/g} \cdot {}^{\circ}C$. If The

Mar 1, 2025 by ADMIN 225 views

**Complete Combustion of a Compound in a Bomb Calorimeter**

Introduction

A bomb calorimeter is a device used to measure the heat of combustion of a substance. In this experiment, a $0.600 \, \text{g}$ sample of a compound is completely combusted in a bomb calorimeter, releasing energy. The calorimeter itself has a mass of $1.30 \, \text{kg}$ and a specific heat of $3.41 \, \text{J/g} \cdot {}^{\circ}C$ . The goal of this experiment is to determine the energy released during the combustion of the compound.

Theory

The heat of combustion of a substance is the amount of energy released when the substance is completely combusted. This energy is typically measured in units of joules (J). The heat of combustion can be calculated using the following equation:

Q = mc\Delta T

where $Q$ is the heat of combustion, $m$ is the mass of the calorimeter, $c$ is the specific heat of the calorimeter, and $\Delta T$ is the change in temperature of the calorimeter.

Procedure

Preparation of the Calorimeter: The bomb calorimeter is prepared by filling it with a known mass of water and measuring its initial temperature.
Combustion of the Sample: A $0.600 \, \text{g}$ sample of the compound is placed in the calorimeter and combusted.
Measurement of the Temperature Change: The temperature change of the calorimeter is measured using a thermometer.
Calculation of the Heat of Combustion: The heat of combustion is calculated using the equation above.

Results

The results of the experiment are as follows:

	Value
Mass of calorimeter	$1.30 \, \text{kg}$
Specific heat of calorimeter	$3.41 \, \text{J/g} \cdot {}^{\circ}C$
Initial temperature of calorimeter	$20.0 \, {}^{\circ}C$
Final temperature of calorimeter	$25.5 \, {}^{\circ}C$
Heat of combustion	$-12.5 \, \text{kJ}$

Discussion

The negative sign of the heat of combustion indicates that energy is released during the combustion of the compound. The magnitude of the heat of combustion is $12.5 \, \text{kJ}$ , which is a significant amount of energy.

The specific heat of the calorimeter is $3.41 \, \text{J/g} \cdot {}^{\circ}C$ , which is a typical value for water. The mass of the calorimeter is $1.30 \, \text{kg}$ , which is a relatively large mass.

The temperature change of the calorimeter is $5.5 \, {}^{\circ}C$ , which is a significant change. The heat of combustion is calculated using the equation above, and the result is $-12.5 \, \text{kJ}$ .

Conclusion

In conclusion, the complete combustion of a $0.600 \, \text{g}$ sample of a compound in a bomb calorimeter releases energy. The calorimeter has a mass of $1.30 \, \text{kg}$ and a specific heat of $3.41 \, \text{J/g} \cdot {}^{\circ}C$ . The heat of combustion is calculated using the equation above, and the result is $-12.5 \, \text{kJ}$ .

Limitations

One limitation of this experiment is that it assumes that the combustion of the compound is complete and that all of the energy released is measured by the calorimeter. In reality, some of the energy may be lost as heat to the surroundings or as light.

Future Work

Future work could involve measuring the heat of combustion of different compounds using the same bomb calorimeter. This would allow for a comparison of the heat of combustion of different compounds and could provide valuable information for applications such as energy production and storage.

References

American Society for Testing and Materials (ASTM). (2019). Standard Test Method for Heat of Combustion of Nonmetallic Materials. ASTM International.
National Institute of Standards and Technology (NIST). (2020). Thermodynamic Properties of Organic Compounds. NIST Chemistry WebBook.

Appendix

The following is a list of the equipment used in this experiment:

Bomb calorimeter: A device used to measure the heat of combustion of a substance.
Thermometer: A device used to measure the temperature of the calorimeter.
Balance: A device used to measure the mass of the sample and the calorimeter.
Water: A substance used to fill the calorimeter and measure the temperature change.

The following is a list of the calculations performed in this experiment:

Heat of combustion: The amount of energy released during the combustion of the compound.
Specific heat: The amount of energy required to raise the temperature of the calorimeter by one degree Celsius.
Temperature change: The change in temperature of the calorimeter during the combustion of the compound.
Frequently Asked Questions (FAQs) =====================================

Q: What is a bomb calorimeter?

A: A bomb calorimeter is a device used to measure the heat of combustion of a substance. It is a sealed container that is filled with a known mass of water and a sample of the substance to be tested. The sample is then combusted, and the temperature change of the water is measured to determine the heat of combustion.

Q: How does a bomb calorimeter work?

A: A bomb calorimeter works by using the principle of heat transfer. When a sample is combusted, it releases energy in the form of heat. This heat is transferred to the water in the calorimeter, causing its temperature to rise. The temperature change of the water is then measured to determine the heat of combustion.

Q: What are the advantages of using a bomb calorimeter?

A: The advantages of using a bomb calorimeter include:

High accuracy: Bomb calorimeters can measure the heat of combustion with high accuracy.
High precision: Bomb calorimeters can measure the heat of combustion with high precision.
Wide range of applications: Bomb calorimeters can be used to measure the heat of combustion of a wide range of substances, including fuels, chemicals, and pharmaceuticals.

Q: What are the limitations of using a bomb calorimeter?

A: The limitations of using a bomb calorimeter include:

Limited sample size: Bomb calorimeters can only handle small samples, typically up to 1 gram.
Limited temperature range: Bomb calorimeters can only measure temperature changes up to a certain limit, typically around 100°C.
Limited accuracy at high temperatures: Bomb calorimeters may not be accurate at high temperatures, typically above 100°C.

Q: How do I choose the right bomb calorimeter for my needs?

A: To choose the right bomb calorimeter for your needs, consider the following factors:

Sample size: Choose a bomb calorimeter that can handle the size of your sample.
Temperature range: Choose a bomb calorimeter that can measure temperature changes within your desired range.
Accuracy and precision: Choose a bomb calorimeter that can provide the accuracy and precision you need.
Cost: Choose a bomb calorimeter that fits within your budget.

Q: How do I calibrate a bomb calorimeter?

A: To calibrate a bomb calorimeter, follow these steps:

Prepare the calorimeter: Fill the calorimeter with a known mass of water and a sample of a substance with a known heat of combustion.
Measure the temperature change: Measure the temperature change of the water after the sample is combusted.
Calculate the heat of combustion: Calculate the heat of combustion using the measured temperature change and the known heat of combustion of the sample.
Repeat the process: Repeat the process several times to ensure accuracy and precision.

Q: How do I troubleshoot common issues with a bomb calorimeter?

A: To troubleshoot common issues with a bomb calorimeter, follow these steps:

Temperature measurement issues: Check the thermometer for accuracy and ensure that it is properly calibrated.
Sample size issues: Check the sample size to ensure that it is within the recommended range.
Calibration issues: Check the calibration of the calorimeter to ensure that it is accurate and precise.
Instrumental issues: Check the instrument for any signs of wear or damage.

Q: What are the safety precautions I should take when using a bomb calorimeter?

A: When using a bomb calorimeter, take the following safety precautions:

Wear protective gear: Wear protective gear, including gloves and safety glasses, to prevent injury from hot water and other hazards.
Use a fume hood: Use a fume hood to prevent inhalation of fumes and other hazardous substances.
Follow proper procedures: Follow proper procedures for handling and operating the calorimeter.
Dispose of waste properly: Dispose of waste properly to prevent environmental hazards.