Step 1: Understanding the Concept.
A quantity in thermodynamics falls into one of two boxes. A state function only cares where the system is right now, so it is the same number no matter how the system got there. A path function cares about the journey, so it can come out different for two processes that start and end at the same two states.
Step 2: Key Approach.
The fastest way to sort the four options is to write down how each one is calculated, and check whether that calculation needs "path" information (like the exact shape of a $P$-$V$ curve) or only "state" information (like $T$, $P$, $V$ at the endpoints).
Step 3: Detailed Explanation.
Enthalpy is $H=U+PV$. Every symbol on the right, $U$, $P$, $V$, is fixed once the state is fixed, so $H$ is fixed too. State function.
Entropy change between two states works out to the same number along a reversible path or an irreversible one, precisely because $S$ was built to only depend on the state. State function.
Internal energy $U$, for a simple system, depends only on state variables like temperature. Even though heat $Q$ and work $W$ separately change with the path, the first law $\Delta U = Q-W$ keeps their difference fixed for any path between two given states. State function.
Work, though, is literally defined as an area under a $P$-$V$ curve, $W=\int P\,dV$. Draw two different curves between the same start and end point on a $P$-$V$ diagram, one going through high pressure and one through low pressure, and the areas underneath, that is, the work, come out different. So work depends on the path, not just the state.
Step 4: Final Answer.
Enthalpy, entropy and internal energy are all fixed by the state alone, but work changes with the path taken between two states.
\[ \boxed{\text{Work}} \]
