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How much heat would be required to convert 7.47 mol of a pure substance from a liquid at 40.0°C to a gas at 113.0°C? Cliquid = 1.45 J/mol·°C 0.65 J/mol·°C Cgas = AHvaporization = 1.23 kJ/mol Tboiling = 88.5 °C

How much heat would be required to convert 7.47 mol of a pure substance from a liquid at 40.0°C to a gas at 113.0°C? Cliquid = 1.45 J/mol·°C 0.65 J/mol·°C Cgas = AHvaporization = 1.23 kJ/mol Tboiling = 88.5 °C

Human Anatomy & Physiology (11th Edition)
Human Anatomy & Physiology (11th Edition)
11th Edition
ISBN:9780134580999
Author:Elaine N. Marieb, Katja N. Hoehn
Publisher:Elaine N. Marieb, Katja N. Hoehn
Chapter1: The Human Body: An Orientation
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**Question 24 of 26** How much heat would be required to convert 7.47 mol of a pure substance from a liquid at 40.0°C to a gas at 113.0°C? **Information Provided:** - \( C_{\text{liquid}} = 1.45 \, \text{J/mol} \cdot °\text{C} \) - \( C_{\text{gas}} = 0.65 \, \text{J/mol} \cdot °\text{C} \) - \( T_{\text{boiling}} = 88.5 \, °\text{C} \) - \( \Delta H_{\text{vaporization}} = 1.23 \, \text{kJ/mol} \) **Explanation:** This table provides the specific heat capacities of the substance in both its liquid and gaseous states, the boiling temperature, and the enthalpy of vaporization, which is the heat required to convert the substance from liquid to gas at its boiling point. To determine the total heat required, you would need to calculate: 1. The heat needed to raise the temperature of the liquid from 40.0°C to 88.5°C. 2. The heat required for the phase change at the boiling point (using the enthalpy of vaporization). 3. The heat required to raise the temperature of the gas from 88.5°C to 113.0°C.
Transcribed Image Text:**Question 24 of 26** How much heat would be required to convert 7.47 mol of a pure substance from a liquid at 40.0°C to a gas at 113.0°C? **Information Provided:** - \( C_{\text{liquid}} = 1.45 \, \text{J/mol} \cdot °\text{C} \) - \( C_{\text{gas}} = 0.65 \, \text{J/mol} \cdot °\text{C} \) - \( T_{\text{boiling}} = 88.5 \, °\text{C} \) - \( \Delta H_{\text{vaporization}} = 1.23 \, \text{kJ/mol} \) **Explanation:** This table provides the specific heat capacities of the substance in both its liquid and gaseous states, the boiling temperature, and the enthalpy of vaporization, which is the heat required to convert the substance from liquid to gas at its boiling point. To determine the total heat required, you would need to calculate: 1. The heat needed to raise the temperature of the liquid from 40.0°C to 88.5°C. 2. The heat required for the phase change at the boiling point (using the enthalpy of vaporization). 3. The heat required to raise the temperature of the gas from 88.5°C to 113.0°C.
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