A 66-kg copper block initially at 140°C is dropped into an insulated tank that contains 90 L of water at 10°C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is cp = 4.18 kJ/kg-K. The density of water is 997 kg/m³. The specific heat of copper at 27°C is cp = 0.386 kJ/kg-K.

A 66-kg copper block initially at 140°C is dropped into an insulated tank that contains 90 L of water at 10°C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is cp = 4.18 kJ/kg-K. The density of water is 997 kg/m³. The specific heat of copper at 27°C is cp = 0.386 kJ/kg-K.

Elements Of Electromagnetics

7th Edition

ISBN:9780190698614

Author:Sadiku, Matthew N. O.

Publisher:Sadiku, Matthew N. O.

ChapterMA: Math Assessment

Section: Chapter Questions

Problem 1.1MA

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A 54-kg copper block initially at 140°C is dropped into an insulated tank that contains 90 L of water at 10°C. Determine the final equilibrium temperature and the total entropy change for this process. The specific heat of water at 25°C is cp=4.18 kJ/kg-K. The density of water is 997 kg/m³. The specific heat of copper at 27°C is cp=0.386 kJ/kg-K. 90 L Water Copper K. The final equilibrium temperature is The total entropy change during this process is KJ/K.