A 30 g ice cube at 0 °C is put in an equal mass of 98 °C water in an insulated container, and allowed to melt. After a while the resulting mixture is at a final (uniform) temperature. How much heat energy does the ice require to completely melt at 0 °C? What is the uniform temperature of the resulting 'mixture'? Note: assume that the heat capacity of water and ice are independent of temperature, and are 4200 J/kgK and 2100 J/kgK, respectively. The heats of fusion and vapourization of water are 3.33x10° J/kg and 2.35×10° J/kg, respectively. How much heat energy does the ice require to completely melt at 0 °C? Answer = What is the resulting temperature of the total liquid (in °C)? Answer = "C

A 30 g ice cube at 0 °C is put in an equal mass of 98 °C water in an insulated container, and allowed to melt. After a while the resulting mixture is at a final (uniform) temperature. How much heat energy does the ice require to completely melt at 0 °C? What is the uniform temperature of the resulting 'mixture'? Note: assume that the heat capacity of water and ice are independent of temperature, and are 4200 J/kgK and 2100 J/kgK, respectively. The heats of fusion and vapourization of water are 3.33x10° J/kg and 2.35×10° J/kg, respectively. How much heat energy does the ice require to completely melt at 0 °C? Answer = What is the resulting temperature of the total liquid (in °C)? Answer = "C

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 119AE: In regions with dry climates, evaporative coolers are used to cool air. A typical electric air...

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