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

Question

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

when block of Aluminium is placed in water , the combined water + aluminium system will try to reach an equilibrium . So that temperature of the aluminium block will decrease and that of cold water will increase. As cold water is kept in an insulated container no exchange of heat will occur between the systenm and surrounding.

So, change in energy of the surrounding = 0.

change in energy of the system = +ve

change in enropy of the surrounding = 0

change in entropy of the system = +ve

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