Suppose a 10 g block of aluminum at 80°C is placed in 50 ml of cold water at 15°

Question

Suppose a 10 g block of aluminum at 80°C is placed in 50 ml of cold water at 15°C located in a perfectly insulated flask. Define clearly the initial state of this system, the final state of the system, the change in entropy of the system, if any, the change in entropy of the surroundings, if any, the change in energy of the system and surroundings, if any. Don’t give any numbers, just state what happens and why. Define the reverse process and give all pertinent changes in the thermodynamic parameters.

Explanation / Answer

Initially the system consists of 10 gm of aluminium block at 80 deg.c and 50m of cold water at 15 deg.c, when the block is placed in water at 15 deg.c, since the system is insulated, the heat from aluminium block is transferred to water. This results in water gaining heat and aluminium block loosing heat.

Water gains entropy and aluminium looses entropy. The net results is an increased entropy of the system. The entropy of universe to that extent decreases. since entropy of universe= 0

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