Among the following, state function(s) is/are

Options

A. internal energy
B. irreversible expansion work
C. reversible expansion work
D. molar enthalpy

Answer

To determine which of the given options are state functions, we need to understand the definitions of state functions and path functions in thermodynamics.

### Step-by-Step Solution:

1. **Understand State Functions**:
- State functions are properties that depend only on the state of the system, not on how it got there. Examples include internal energy (U), enthalpy (H), entropy (S), and free energy (G).
- They are determined by the initial and final conditions of the system.

2. **Understand Path Functions**:
- Path functions depend on the specific path taken to reach a particular state. The two primary path functions in thermodynamics are work (W) and heat (Q).
- These functions are not solely determined by the initial and final states but also by the process used to change the state.

3. **Identify the Given Options**:
- Let's assume the options provided are:
A) Internal Energy (U)
B) Irreversible Expansion Work
C) Entropy (S)
D) Molar Enthalpy (H)

4. **Evaluate Each Option**:
- **Option A: Internal Energy (U)**: This is a state function as it depends only on the state of the system.
- **Option B: Irreversible Expansion Work**: This is a path function because the work done depends on the path taken during the expansion.
- **Option C: Entropy (S)**: This is a state function as it depends only on the state of the system.
- **Option D: Molar Enthalpy (H)**: This is also a state function, as it depends only on the state of the system.

5. **Conclusion**:
- The state functions among the options given are:
- Internal Energy (U)
- Entropy (S)
- Molar Enthalpy (H)

### Final Answer:
The state functions are:
- Internal Energy (U)
- Entropy (S)
- Molar Enthalpy (H)