**Problem 13: Heat Calculation for Phase Changes of Water** **Objective:** Determine the amount of heat, in kilojoules (kJ), needed to warm 31.6 grams of ice from -10°C to steam at 175°C. **Given Data:** - Heat capacity of ice: \(2.09 \, \text{J/g°C}\) - Heat capacity of liquid water: \(4.18 \, \text{J/g°C}\) - Heat capacity of steam: \(1.84 \, \text{J/g°C}\) - Enthalpy of fusion (\( \Delta H_{\text{fus}} \)) for water: \(6.02 \, \text{kJ/mol}\) - Enthalpy of vaporization (\( \Delta H_{\text{vap}} \)) for water: \(40.7 \, \text{kJ/mol}\) **Process:** 1. **Warming Ice from -10°C to 0°C:** - Use the specific heat capacity of ice to calculate the energy required. 2. **Melting Ice at 0°C:** - Use the enthalpy of fusion to calculate the energy required to convert ice to liquid water. 3. **Heating Liquid Water from 0°C to 100°C:** - Use the specific heat capacity of liquid water to calculate the energy required. 4. **Vaporizing Water at 100°C:** - Use the enthalpy of vaporization to calculate the energy required to convert water to steam. 5. **Heating Steam from 100°C to 175°C:** - Use the specific heat capacity of steam to calculate the energy required. **Calculation Methodology:** - Break down the calculations into steps corresponding to each phase change and temperature change. - Calculate the total heat by summing the energy required for each step. - Convert units where necessary to ensure consistency and accuracy. This comprehensive approach ensures an understanding of thermodynamics and phase transitions in water.
**Problem 13: Heat Calculation for Phase Changes of Water** **Objective:** Determine the amount of heat, in kilojoules (kJ), needed to warm 31.6 grams of ice from -10°C to steam at 175°C. **Given Data:** - Heat capacity of ice: \(2.09 \, \text{J/g°C}\) - Heat capacity of liquid water: \(4.18 \, \text{J/g°C}\) - Heat capacity of steam: \(1.84 \, \text{J/g°C}\) - Enthalpy of fusion (\( \Delta H_{\text{fus}} \)) for water: \(6.02 \, \text{kJ/mol}\) - Enthalpy of vaporization (\( \Delta H_{\text{vap}} \)) for water: \(40.7 \, \text{kJ/mol}\) **Process:** 1. **Warming Ice from -10°C to 0°C:** - Use the specific heat capacity of ice to calculate the energy required. 2. **Melting Ice at 0°C:** - Use the enthalpy of fusion to calculate the energy required to convert ice to liquid water. 3. **Heating Liquid Water from 0°C to 100°C:** - Use the specific heat capacity of liquid water to calculate the energy required. 4. **Vaporizing Water at 100°C:** - Use the enthalpy of vaporization to calculate the energy required to convert water to steam. 5. **Heating Steam from 100°C to 175°C:** - Use the specific heat capacity of steam to calculate the energy required. **Calculation Methodology:** - Break down the calculations into steps corresponding to each phase change and temperature change. - Calculate the total heat by summing the energy required for each step. - Convert units where necessary to ensure consistency and accuracy. This comprehensive approach ensures an understanding of thermodynamics and phase transitions in water.
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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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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Transcribed Image Text:**Problem 13: Heat Calculation for Phase Changes of Water**
**Objective:** Determine the amount of heat, in kilojoules (kJ), needed to warm 31.6 grams of ice from -10°C to steam at 175°C.
**Given Data:**
- Heat capacity of ice: \(2.09 \, \text{J/g°C}\)
- Heat capacity of liquid water: \(4.18 \, \text{J/g°C}\)
- Heat capacity of steam: \(1.84 \, \text{J/g°C}\)
- Enthalpy of fusion (\( \Delta H_{\text{fus}} \)) for water: \(6.02 \, \text{kJ/mol}\)
- Enthalpy of vaporization (\( \Delta H_{\text{vap}} \)) for water: \(40.7 \, \text{kJ/mol}\)
**Process:**
1. **Warming Ice from -10°C to 0°C:**
- Use the specific heat capacity of ice to calculate the energy required.
2. **Melting Ice at 0°C:**
- Use the enthalpy of fusion to calculate the energy required to convert ice to liquid water.
3. **Heating Liquid Water from 0°C to 100°C:**
- Use the specific heat capacity of liquid water to calculate the energy required.
4. **Vaporizing Water at 100°C:**
- Use the enthalpy of vaporization to calculate the energy required to convert water to steam.
5. **Heating Steam from 100°C to 175°C:**
- Use the specific heat capacity of steam to calculate the energy required.
**Calculation Methodology:**
- Break down the calculations into steps corresponding to each phase change and temperature change.
- Calculate the total heat by summing the energy required for each step.
- Convert units where necessary to ensure consistency and accuracy.
This comprehensive approach ensures an understanding of thermodynamics and phase transitions in water.
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