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O Attempt 2 The combustion of 1.910 g of propanol (C,H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.97 K. The heat capacity of the bomb calorimeter is 12.90 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. AH = 2.16 x10-3 kJ/mol Incorrect

O Attempt 2 The combustion of 1.910 g of propanol (C,H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.97 K. The heat capacity of the bomb calorimeter is 12.90 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. AH = 2.16 x10-3 kJ/mol Incorrect

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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
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my previous answer was -2.16*10^-3.
**Title: Calculating Enthalpy Change for the Combustion of Propanol** **Introduction:** The combustion of 1.910 g of propanol (\( \text{C}_3\text{H}_8\text{O} \)) increases the temperature of a bomb calorimeter from 298.00 K to 302.97 K. The heat capacity of the bomb calorimeter is 12.90 kJ/K. Determine \( \Delta H \) for the combustion of propanol to carbon dioxide gas and liquid water. **Procedure:** 1. **Mass of Propanol Combusted:** 1.910 g 2. **Initial Temperature of Calorimeter:** 298.00 K 3. **Final Temperature of Calorimeter:** 302.97 K 4. **Heat Capacity of Calorimeter:** 12.90 kJ/K **Calculation:** - Calculate the change in temperature (\( \Delta T \)): - \( \Delta T = 302.97 \, \text{K} - 298.00 \, \text{K} = 4.97 \, \text{K} \) - Calculate the heat absorbed by the calorimeter using the formula: - \( q = C \times \Delta T \) - Where \( q \) is the heat absorbed by the calorimeter, \( C \) is the heat capacity, and \( \Delta T \) is the change in temperature. - \( q = 12.90 \, \text{kJ/K} \times 4.97 \, \text{K} \) - Solve for \( q \). **Result:** - **Attempted Calculation:** The initial calculation in the image shows an incorrect value of \( \Delta H = 2.16 \times 10^{-3} \) kJ/mol. The correct calculation needs to be redone based on proper conversion factors and stoichiometry. **Conclusion:** Determining \( \Delta H \) requires accurate mass calculations and usage of appropriate stoichiometric coefficients when converting grams of a substance to moles. Always double-check your calculations for accuracy. **Note:** In this setup, recalculation is necessary to ensure correct interpretation and conversion for educational purposes.
Transcribed Image Text:**Title: Calculating Enthalpy Change for the Combustion of Propanol** **Introduction:** The combustion of 1.910 g of propanol (\( \text{C}_3\text{H}_8\text{O} \)) increases the temperature of a bomb calorimeter from 298.00 K to 302.97 K. The heat capacity of the bomb calorimeter is 12.90 kJ/K. Determine \( \Delta H \) for the combustion of propanol to carbon dioxide gas and liquid water. **Procedure:** 1. **Mass of Propanol Combusted:** 1.910 g 2. **Initial Temperature of Calorimeter:** 298.00 K 3. **Final Temperature of Calorimeter:** 302.97 K 4. **Heat Capacity of Calorimeter:** 12.90 kJ/K **Calculation:** - Calculate the change in temperature (\( \Delta T \)): - \( \Delta T = 302.97 \, \text{K} - 298.00 \, \text{K} = 4.97 \, \text{K} \) - Calculate the heat absorbed by the calorimeter using the formula: - \( q = C \times \Delta T \) - Where \( q \) is the heat absorbed by the calorimeter, \( C \) is the heat capacity, and \( \Delta T \) is the change in temperature. - \( q = 12.90 \, \text{kJ/K} \times 4.97 \, \text{K} \) - Solve for \( q \). **Result:** - **Attempted Calculation:** The initial calculation in the image shows an incorrect value of \( \Delta H = 2.16 \times 10^{-3} \) kJ/mol. The correct calculation needs to be redone based on proper conversion factors and stoichiometry. **Conclusion:** Determining \( \Delta H \) requires accurate mass calculations and usage of appropriate stoichiometric coefficients when converting grams of a substance to moles. Always double-check your calculations for accuracy. **Note:** In this setup, recalculation is necessary to ensure correct interpretation and conversion for educational purposes.
Expert Solution
Step 1

To calculate the heat capacity of propane in kJ/mol, first of we calculate the moles of propanol present in 1.910 g of propanol.

We know that the molar mass of propane is = 60.0952 g/mol

The number moles

= mass in gram/molar mass

The number of moles of propane is

= (1.910 g) / (60.0952 g/mol)

= 0.03178 moles

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