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city for the solid, which is not given in the table. It is 255.7 J/K m

city for the solid, which is not given in the table. It is 255.7 J/K m

Chemistry
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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**Heating Curve of 1 Mole of Octane** **Objective:** Sketch a heating curve for 1 mole of octane from -57°C to 150°C. Use the provided data and perform necessary calculations for each step. **Data:** - **Boiling Point:** 125.7°C - **Melting Point:** -56.8°C - **ΔH_vap (Enthalpy of Vaporization):** 41.5 kJ/mol - **ΔH_fus (Enthalpy of Fusion):** 20.7 kJ/mol - **Molar Heat Capacity (liquid):** 254.6 J/(mol°C) - **Molar Heat Capacity (gas):** 316.9 J/(mol°C) - **Molar Heat Capacity (solid, not given in table):** 255.7 J/(mol°C) **Instructions:** 1. **Start at -57°C:** - Octane is in a solid state at this temperature. - Calculate the energy needed to heat the solid octane to its melting point (-56.8°C). 2. **Melting (-56.8°C):** - Use ΔH_fus (20.7 kJ/mol) to calculate the energy required for the phase change from solid to liquid. 3. **Heat Liquid to Boiling Point:** - Calculate the energy required to heat the liquid octane from its melting point (-56.8°C) to its boiling point (125.7°C) using the molar heat capacity of liquid octane. 4. **Vaporization (125.7°C):** - Use ΔH_vap (41.5 kJ/mol) to calculate the energy needed for the phase change from liquid to gas. 5. **Heat Gas to 150°C:** - Calculate the energy required to heat the gaseous octane from its boiling point (125.7°C) to 150°C using the molar heat capacity of gaseous octane. **Graph Explanation:** - The heating curve will start at the initial temperature of -57°C. - It will display a slope corresponding to the heating of the solid octane. - A plateau will represent the phase change from solid to liquid at the melting point. - The curve will then rise as the liquid octane is heated to the boiling point. - Another plateau will represent the phase change from liquid
Transcribed Image Text:**Heating Curve of 1 Mole of Octane** **Objective:** Sketch a heating curve for 1 mole of octane from -57°C to 150°C. Use the provided data and perform necessary calculations for each step. **Data:** - **Boiling Point:** 125.7°C - **Melting Point:** -56.8°C - **ΔH_vap (Enthalpy of Vaporization):** 41.5 kJ/mol - **ΔH_fus (Enthalpy of Fusion):** 20.7 kJ/mol - **Molar Heat Capacity (liquid):** 254.6 J/(mol°C) - **Molar Heat Capacity (gas):** 316.9 J/(mol°C) - **Molar Heat Capacity (solid, not given in table):** 255.7 J/(mol°C) **Instructions:** 1. **Start at -57°C:** - Octane is in a solid state at this temperature. - Calculate the energy needed to heat the solid octane to its melting point (-56.8°C). 2. **Melting (-56.8°C):** - Use ΔH_fus (20.7 kJ/mol) to calculate the energy required for the phase change from solid to liquid. 3. **Heat Liquid to Boiling Point:** - Calculate the energy required to heat the liquid octane from its melting point (-56.8°C) to its boiling point (125.7°C) using the molar heat capacity of liquid octane. 4. **Vaporization (125.7°C):** - Use ΔH_vap (41.5 kJ/mol) to calculate the energy needed for the phase change from liquid to gas. 5. **Heat Gas to 150°C:** - Calculate the energy required to heat the gaseous octane from its boiling point (125.7°C) to 150°C using the molar heat capacity of gaseous octane. **Graph Explanation:** - The heating curve will start at the initial temperature of -57°C. - It will display a slope corresponding to the heating of the solid octane. - A plateau will represent the phase change from solid to liquid at the melting point. - The curve will then rise as the liquid octane is heated to the boiling point. - Another plateau will represent the phase change from liquid
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