Chapter 24, Problem 37A

The combined molecular kinetic energies of molecules in a very large container of cold water are greater than the combined molecular kinetic energies in a cup of hot tea. Pretend you partially immerse the teacup in the cold water and that the tea absorbs 10 joules of energy from the water and becomes hotter, while the water that gives up 10 joules of energy becomes cooler. Would this energy transfer violate the first law of thermodynamics? The second law of thermodynamics? Explain.

To determine

To identify: Whether the energy transfer violates the first and second law of thermodynamics.

Explanation of Solution

Introduction:

First Law of Thermodynamics,

  $\Delta U=Q-W$

Where,

  $\Delta U=$ Internal energy

  $Q=$ Heat

  $W=$ Work done

Second law of Thermodynamics,

  $\Delta S=\frac{\Delta Q}{T}\text{}\text{}$

Where,

  $\Delta S=\frac{\Delta Q}{T}\text{}\text{}$ Entropy

  $\Delta Q=$ Heat

  $T=$ Temperature

The first law of thermodynamic is application of conservation of energy, the energy cannot created nor be destroyed and it can be transfer to one body to another body. So, in this case the first law of thermodynamic is not violet. In second law of thermodynamic, the entropy of an isolated system cannot decrease and constant for reversible process. In this the heat is transferred from colder body to hotter body which is not possible in thermodynamic according to the second law of thermodynamics so, the second law of thermodynamic is violet.

Conclusion:

Hence, the given situation violates the second law of thermodynamics but not first law.