19. Ice at 0 °C is placed in a Styrofoam cup containing 361 g of a soft drink at 23.0 °C. Some ice remains after the ice and the soft drink reach an equilibrium temperature of 0 °C. Determine the mass of the ice that has melted. Assume the specific heat of the drink to be the same as pure water. (It requires 334 J of heat to melt 1 g of ice at 0 °C)

19. Ice at 0 °C is placed in a Styrofoam cup containing 361 g of a soft drink at 23.0 °C. Some ice remains after the ice and the soft drink reach an equilibrium temperature of 0 °C. Determine the mass of the ice that has melted. Assume the specific heat of the drink to be the same as pure water. (It requires 334 J of heat to melt 1 g of ice at 0 °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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40.0 g of an unknown metal at 100.0°C is added to 50.0 g of water at 30.0°C. When the system reaches equilibrium, the temperature is 34.5°C. What is the specific heat of the metal?
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2. A metal sample having a temperature of 100°C and a mass of 45.2 g was placed in 50 g of water with a temperature of 26°C. At equilibrium, the final temperature was 32.7°C a) How much heat flowed into the water? b) What is the specific heat of the metal?
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17. An ice cube is placed in a sealed insulated container of hot water at 80°C. After five minutes, the ice cube disappears. Ice Cube Heat ener Hot Water 5 min. Water Which best describes the change that took place inside the container? The total heat energy in the container was reduced by the ice cube. The hot water lost the same amount of heat energy as the ice cube gained. in the hot water was reduced by kinetic energy in the ice cube. O Heat energy in the ice cube was dissipated into the hot water.
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4. Aluminum metal melts at 658.5°C. What would be the final temperature if 28.0 grams of solid aluminum at this temperature were placed into 520 grams of liquid aluminum at 1000.0°C? The heat of fusion for aluminum is 396 J/ -1 -1 g, and the specific heat of liquid aluminum is 0.481 J-g`¹deg-¹. (Note: this is the aluminum analog to the process you just did in lab!)
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