1. Check each statement one by one

A thermodynamic system is described by variables like internal energy $U$, entropy $S$, pressure $P$, volume $V$, etc. We test each option.

2. Option A: "The change in entropy can never be zero"

This is false.

Entropy change can be zero in some processes. For example:

• In a reversible adiabatic (isentropic) process, $\Delta S = 0$ So it is wrong to say entropy change can never be zero.

3. Option B: "Internal energy and entropy are state functions"

This is true.

A state function depends only on the initial and final states, not on the path followed.

Both:

• Internal energy $U$
• Entropy $S$

are state functions in thermodynamics.

Hence, option B is correct.

4. Option C: "The internal energy changes in all processes"

This is false.

Internal energy does not change in all processes. Example:

• For an ideal gas in an isothermal process, temperature remains constant.
• Since internal energy of an ideal gas depends only on temperature, $\Delta U = 0$ So this statement is incorrect.

5. Option D: "The work done in an adiabatic process is always zero"

This is false.

In an adiabatic process, $Q = 0$ but work may still be done.

Using first law: $\Delta U = Q - W$ Since $Q=0$, $\Delta U = -W$ So generally $W \neq 0$.

For example, during adiabatic expansion, the gas does work.

6. Final conclusion

Only Option B is correct.

7. Comparison with stored correct answer

Stored correct answer: B

Derived answer: B

They agree.