cold water of

0.1m^(^(^()))3

at

29\\\\deg 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

4.2k(J)/(k)g-K

, and the specific heat of Iron is

0.45k(J)/(k)g-K

. The density of water is 1000

k(g)/(m^(^(^())))3

.

cold water of 0.1m3 at 29 . 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 4.2kJ/kgK, and the specific heat of Iron is 0.45kJ/kgK. The density of water is 1000 kg/m3 cold water of 0.1m3 at 29 . 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 4.2kJ/kgK, and the specific heat of Iron is 0.45kJ/kgK. The density of water is 1000 kg/m3