KCET 2026 Chemistry Solved Paper

Concept:A state function depends only on the present state of the system, not on the path taken to reach that state.Explanation:Internal energy $U$ and entropy $S$ depend only on the current state of the system, such as temperature, pressure, and volume.Therefore, both $U$ and $S$ are state functions.So, Option B is correct.Now, examine the other options.Option A says internal energy changes in all processes, but this is false.In an isothermal process for an ideal gas, temperature remains constant, so $\Delta U = 0$.Thus, internal energy does not necessarily change in every process.Option C says work is a state function, which is wrong.Work depends on the path followed during the process, so it is a path function.Option D says work done in an adiabatic process is always zero, which is also wrong.In an adiabatic process, heat exchanged is zero, so $q = 0$.From the first law of thermodynamics, $\Delta U = q + w$.With $q = 0$, we get $\Delta U = w$.Therefore, work done is not necessarily zero in an adiabatic process.Answer:Option B: Internal energy and entropy are state functions.