A soft drink (230 mL of mostly water) initially at 17.0 C is cooled by adding 148 g of ice cubes at 0 C. What mass of ice remains when the temperature of the drink reaches equilibrium (water and ice at 0 C)? The enthalpy of fusion of water (i.e., the heat required to melt ice) is 6.007 kJ/mol. The density of the water is 1.0 g/mL. Assume the specific heat capacity of water is constant and equal to 4.184 J/g/C.
A soft drink (230 mL of mostly water) initially at 17.0 C is cooled by adding 148 g of ice cubes at 0 C. What mass of ice remains when the temperature of the drink reaches equilibrium (water and ice at 0 C)? The enthalpy of fusion of water (i.e., the heat required to melt ice) is 6.007 kJ/mol. The density of the water is 1.0 g/mL. Assume the specific heat capacity of water is constant and equal to 4.184 J/g/C.
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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A soft drink (230 mL of mostly water) initially at 17.0 C is cooled by adding 148 g of ice cubes at 0 C. What mass of ice remains when the temperature of the drink reaches equilibrium (water and ice at 0 C)? The enthalpy of fusion of water (i.e., the heat required to melt ice) is 6.007 kJ/mol. The density of the water is 1.0 g/mL. Assume the specific heat capacity of water is constant and equal to 4.184 J/g/C.
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