Thermodynamics 1 problem: A 2-kg block of ice with an initial temperature of -30

Question

Thermodynamics 1 problem:

A 2-kg block of ice with an initial temperature of -30°C is dropped into an insulated tank containing 10 kg of liquid water at an initial temperature of 20°C. The heat capacity of the solid ice is 2.03 kJ/kg-°C and the heat capacity of the liquid water is 4.18 kJ/kg-°C. The heat of fusion for water is 333.4 kJ/kg. Assume that all of these quantities are independent of temperature, and that the pressure is 1 bar.

(a) Determine the final phase of the water in the tank.

(b) Calculae the final temperature (°C) of the water in the tank.

Explanation / Answer

The process is irreversible

Heat lost by ice = heat gained by water

mCp( To - Ti ) = mCp (Ti - To)

2.03 (273 - 243 ) = 4.18 ( 293-To)

To = 278.44 Kelvin

To = 278.44 -273

To = 5.44 C ans

Water trying to cool

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