**Title: Comparing Fuel Efficiency Using Bomb Calorimetry****Introduction:**In this educational exercise, we evaluate the efficiency of three fuel samples by calculating the heat of combustion for each when 1.00 mol is burned. The fuels investigated are hydrazine (N₂H₄), octane (C₈H₁₈), and TNT (C₇H₅N₃O₆). The data gathered from bomb calorimetry experiments allows us to determine the energy each fuel releases, which is a critical factor in assessing their suitability for various applications.**Experiment Details:****a. Hydrazine (N₂H₄):**- **Sample Mass:** 1.000 g- **Initial Temperature:** 24.62°C- **Final Temperature:** 28.16°C- **Calorimeter Heat Capacity:** 5860 J/°CTo determine the heat of combustion, calculate the total energy absorbed by the calorimeter using:\[ q = \text{Calorimeter heat capacity} \times (\text{Final Temperature} - \text{Initial Temperature}) \]**Answer:** -665 kJ/mol---**b. Octane (C₈H₁₈):**- **Sample Mass:** 1.000 g- **Water Mass:** 1200 g- **Initial Temperature:** 25.00°C- **Final Temperature:** 33.20°C- **Calorimeter Heat Capacity:** 837 J/°C- **Specific Heat of Water:** 4.184 J/g°CCalculate the energy change in the water and calorimeter separately, then sum both to determine the overall energy release.\[ q_{\text{water}} = \text{Water Mass} \times \text{Specific Heat of Water} \times (\text{Final Temp} - \text{Initial Temp}) \]\[ q_{\text{calorimeter}} = \text{Calorimeter Heat Capacity} \times (\text{Final Temp} - \text{Initial Temp}) \]**Answer:** -5500 kJ/mol---**c. TNT (C₇H₅N₃O₆):**- **Sample Mass:** 0.500 g- **Water Mass:** 610 g- **Initial Temperature:** 20.00°C- **Final Temperature:**

General formula to calculate heat released in a combustion reaction in a calorimeter ----

8. What is the best fuel? Order the three samples according to the amount of heat released when 1.00 mol is combusted. a. A 1.000 g sample of the rocket fuel hydrazine (N2H4) is burned in a bomb calorimeter. The temperature rises from 24.62°C to 28.16°C. The heat capacity of the calorimeter (including the water) is 5860 J/°C. Calculate the heat of combustion of hydrazine, in kJ/mol. A: -665 kJ/mol b. A 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter containing 1200 g of water at an initial temperature of 25.00°C. After the reaction, the final temperature of the water is 33.20°C. The heat capacity of the calorimeter is 837 J/°C. The specific heat of water is 4.184 J/g°C. Calculate the heat of combustion of octane in kJ/mol. A: -5500 kJ/mol c. A 0.500 g sample of TNT (C7H5N306) is burned in a bomb calorimeter containing 610 g of water at an initial temperature of 20.00°C. After the reaction, the final temperature of the water is 22.5°C. The heat capacity of the calorimeter is 420 J/°C. The specific heat of water is 4.184 J/g°C. Calculate the heat of combustion of TNT in kJ/mol. A: -3400kJ/mol

8. What is the best fuel? Order the three samples according to the amount of heat released when 1.00 mol is combusted. a. A 1.000 g sample of the rocket fuel hydrazine (N2H4) is burned in a bomb calorimeter. The temperature rises from 24.62°C to 28.16°C. The heat capacity of the calorimeter (including the water) is 5860 J/°C. Calculate the heat of combustion of hydrazine, in kJ/mol. A: -665 kJ/mol b. A 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter containing 1200 g of water at an initial temperature of 25.00°C. After the reaction, the final temperature of the water is 33.20°C. The heat capacity of the calorimeter is 837 J/°C. The specific heat of water is 4.184 J/g°C. Calculate the heat of combustion of octane in kJ/mol. A: -5500 kJ/mol c. A 0.500 g sample of TNT (C7H5N306) is burned in a bomb calorimeter containing 610 g of water at an initial temperature of 20.00°C. After the reaction, the final temperature of the water is 22.5°C. The heat capacity of the calorimeter is 420 J/°C. The specific heat of water is 4.184 J/g°C. Calculate the heat of combustion of TNT in kJ/mol. A: -3400kJ/mol

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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