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-When 10.0g of ice at 0.0°C is added to 80.0 g of water at 35°C that is contained in an insulated container, what is the final tempera HINTS: AHvap = 40.7 kJ/mol at 100°C; AHfus = 6.01 kJ/mol at 0.00°C; Cs(steam) = 2.01 J/g°C; Cs(liquid water) = 4.184 /g C; Cslice %3D 27.8 °C 13.4 °C 2.80 °C 22.2 °C 25.0 °C

-When 10.0g of ice at 0.0°C is added to 80.0 g of water at 35°C that is contained in an insulated container, what is the final tempera HINTS: AHvap = 40.7 kJ/mol at 100°C; AHfus = 6.01 kJ/mol at 0.00°C; Cs(steam) = 2.01 J/g°C; Cs(liquid water) = 4.184 /g C; Cslice %3D 27.8 °C 13.4 °C 2.80 °C 22.2 °C 25.0 °C

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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What is the final temperature when the mixture reaches thermal equilibrium?
**Question 7** When 10.0 g of ice at 0.0°C is added to 80.0 g of water at 35°C that is contained in an insulated container, what is the final temperature? **HINTS:** - ΔHvap = 40.7 kJ/mol at 100°C - ΔHfus = 6.01 kJ/mol at 0.00°C - Cᵢ(steam) = 2.01 J/g°C - Cᵢ(liquid water) = 4.184 J/g°C - Cᵢ(ice) = 2.09 J/g°C **Options:** - 27.8°C - 13.4°C - 2.80°C - 22.2°C - 25.0°C --- **Note:** Moving to another question will save this response. **Explanation:** This problem involves the calculation of the final temperature after mixing 10.0 g of ice at 0.0°C with 80.0 g of water at 35°C in an insulated container. Insulated containers imply no heat exchange with the environment. To accurately determine the final temperature, consider the energy interactions involving changes in states, specific heat capacities, the heat absorbed or released during phase changes (melting of ice), and the respective changes in temperatures. The given hints provide various constants such as the heat of vaporization (ΔHvap), the heat of fusion (ΔHfus), and specific heat capacities for different phases of water. Carefully evaluating these energies will help in identifying the correct final temperature of the system from the given multiple-choice options.
Transcribed Image Text:**Question 7** When 10.0 g of ice at 0.0°C is added to 80.0 g of water at 35°C that is contained in an insulated container, what is the final temperature? **HINTS:** - ΔHvap = 40.7 kJ/mol at 100°C - ΔHfus = 6.01 kJ/mol at 0.00°C - Cᵢ(steam) = 2.01 J/g°C - Cᵢ(liquid water) = 4.184 J/g°C - Cᵢ(ice) = 2.09 J/g°C **Options:** - 27.8°C - 13.4°C - 2.80°C - 22.2°C - 25.0°C --- **Note:** Moving to another question will save this response. **Explanation:** This problem involves the calculation of the final temperature after mixing 10.0 g of ice at 0.0°C with 80.0 g of water at 35°C in an insulated container. Insulated containers imply no heat exchange with the environment. To accurately determine the final temperature, consider the energy interactions involving changes in states, specific heat capacities, the heat absorbed or released during phase changes (melting of ice), and the respective changes in temperatures. The given hints provide various constants such as the heat of vaporization (ΔHvap), the heat of fusion (ΔHfus), and specific heat capacities for different phases of water. Carefully evaluating these energies will help in identifying the correct final temperature of the system from the given multiple-choice options.
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