Problem 2: 0.4 kg of ice at – 10°C are mixed with 0.2 kg of water at 50°C. The water and ice are mixed in a calorimeter so that no heat escapes the system. The specific heat of ice is c; = 2090 J/(kg.°C), the la- tent heat of fusion of water is Lf = 3.33× 10° J/kg, and the specific heat of water is cu = 4186 J/(kg.°C). (a) What is the final temperature of the system? (b) How many kg of ice remain in the end? (c) How many kg of water remain in the end?

Problem 2: 0.4 kg of ice at – 10°C are mixed with 0.2 kg of water at 50°C. The water and ice are mixed in a calorimeter so that no heat escapes the system. The specific heat of ice is c; = 2090 J/(kg.°C), the la- tent heat of fusion of water is Lf = 3.33× 10° J/kg, and the specific heat of water is cu = 4186 J/(kg.°C). (a) What is the final temperature of the system? (b) How many kg of ice remain in the end? (c) How many kg of water remain in the end?

Physics for Scientists and Engineers: Foundations and Connections

1st Edition

ISBN:9781133939146

Author:Katz, Debora M.

Publisher:Katz, Debora M.

Chapter21: Heat And The First Law Of Thermodynamics

Section: Chapter Questions

Problem 21PQ

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Question

Problem 2: 0.4 kg of ice at – 10°C are mixed with 0.2 kg of water at 50°C. The water and ice are mixed
in a calorimeter so that no heat escapes the system. The specific heat of ice is c; = 2090 J/(kg.°C), the la-
tent heat of fusion of water is Lf = 3.33× 10° J/kg, and the specific heat of water is cu = 4186 J/(kg-°C).
(a) What is the final temperature of the system?
(b) How many kg of ice remain in the end?
(c) How many kg of water remain in the end?

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