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Sodium acetate is used in many hot packs, which rely on the ability of sodium acetate trihydrate (SAT) to become supercooled, and then spontaneously crystallize via an exothermic process. A solution is made from 50.0 grams of SAT dissolved in 50.0 g of water heated above the melting point of SAT, and is slowly supercooled below room temperature, to 16°C. Assume the specific heat capacity of SAT is 2.19 J/g ·°C and the specific heat capacity of water is 4.184 J/g-°c. The molar enthalpy of fusion is 35.9 kJ/mol for SAT and its molar mass is 136.08 g/mol. Upon crystallization, the temperature increases from 16.0 °C to the melting point of SAT. What is the final temperature of the SAT?

Sodium acetate is used in many hot packs, which rely on the ability of sodium acetate trihydrate (SAT) to become supercooled, and then spontaneously crystallize via an exothermic process. A solution is made from 50.0 grams of SAT dissolved in 50.0 g of water heated above the melting point of SAT, and is slowly supercooled below room temperature, to 16°C. Assume the specific heat capacity of SAT is 2.19 J/g ·°C and the specific heat capacity of water is 4.184 J/g-°c. The molar enthalpy of fusion is 35.9 kJ/mol for SAT and its molar mass is 136.08 g/mol. Upon crystallization, the temperature increases from 16.0 °C to the melting point of SAT. What is the final temperature of the SAT?

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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Sodium acetate is used in many hot packs, which rely on the ability of sodium acetate trihydrate (SAT) to become supercooled, and then spontaneously crystallize via an exothermic process. A solution is made from 50.0 grams of SAT dissolved in 50.0 g of water heated above the melting point of SAT, and is slowly supercooled below room temperature, to 16°C. Assume the specific heat capacity of SAT is 2.19 J/g •°C and the specific heat capacity of water is 4.184 J/g•°C. The molar enthalpy of fusion is 35.9 kJ/mol for SAT and its molar mass is 136.08 g/mol. Upon crystallization, the temperature increases from 16.0 °C to the melting point of SAT. What is the final temperature of the SAT? 96.241 °C 1 2 3 4 6. C 7 8. 9. +/- x 100
Transcribed Image Text:Sodium acetate is used in many hot packs, which rely on the ability of sodium acetate trihydrate (SAT) to become supercooled, and then spontaneously crystallize via an exothermic process. A solution is made from 50.0 grams of SAT dissolved in 50.0 g of water heated above the melting point of SAT, and is slowly supercooled below room temperature, to 16°C. Assume the specific heat capacity of SAT is 2.19 J/g •°C and the specific heat capacity of water is 4.184 J/g•°C. The molar enthalpy of fusion is 35.9 kJ/mol for SAT and its molar mass is 136.08 g/mol. Upon crystallization, the temperature increases from 16.0 °C to the melting point of SAT. What is the final temperature of the SAT? 96.241 °C 1 2 3 4 6. C 7 8. 9. +/- x 100
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