An Iron block of 10kg at 200 C is dropped into a container with cold water...
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An Iron block of 10kg at 200 C is dropped into a container with cold water of 0.05m^3 at 29 C. Assume the container is adiabatic, and that water and Iron can be treated as incompressible substances with constant specific heat. After the Iron block and water come to an equilibrium temperature, what is the entropy change of the system, in units of J/K? Assume that the specific heat of water is 4.2 kJ/kg-K, and the specific heat of Iron is 0.45 kJ/kg-K. The density of water is 1000 kg/m^3. Iron Water An Iron block of 10kg at 200 C is dropped into a container with cold water of 0.05m^3 at 29 C. Assume the container is adiabatic, and that water and Iron can be treated as incompressible substances with constant specific heat. After the Iron block and water come to an equilibrium temperature, what is the entropy change of the system, in units of J/K? Assume that the specific heat of water is 4.2 kJ/kg-K, and the specific heat of Iron is 0.45 kJ/kg-K. The density of water is 1000 kg/m^3. Iron Water
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Related Book For
Thermodynamics An Engineering Approach
ISBN: 978-0073398174
8th edition
Authors: Yunus A. Cengel, Michael A. Boles
Posted Date:
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