91影视

In the given four experiments, blocks A and B brought together in an insulating box to reach a final temperature have four entropy values in each experiment.

This problem is based on the concept of the second law of thermodynamics which is an extended postulate to the concept of entropy. The law states that if a process occurs in a closed system, the entropy of the system increases for irreversible processes and remains constant for reversible processes. It never decreases.

Formula:

The entropy change of the system,$螖S猢�0$

As per the given concept and equation (i), the entropy change of the system of two blocks A and B with entropy changes $鈭�S_1$and $鈭�S_1$can be given as:

$$\begin{gathered} 螖S猢�0 \\ 螖S_1+螖S_2猢�0 \\ 螖S_1猢�-螖S_2 \end{gathered}$$

Thus, there must exist either a negative equal entropy value of entropy change of block B or a lower negative value of entropy change of block B for every entropy value of block A.

Thus, the values of A and B that match the condition are$(8,-8),(5,-5),(3,-3),\text{(9,}-\text{2)}$.