Which of the following are state functions?

Options

A. Enthalpy
B. Heat
C. Free energy
D. work

Answer

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

### Step-by-Step Solution:

1. **Understand the Definitions**:
- **State Functions**: These are properties that depend only on the state of the system, defined by its current conditions (such as temperature, pressure, and volume). They do not depend on how the system reached that state.
- **Path Functions**: These are properties that depend on the specific path taken to reach a particular state. They are related to the process the system undergoes.

2. **Identify the Given Options**:
- The options given are: Enthalpy, Heat, Free Energy, and Work.

3. **Classify Each Option**:
- **Enthalpy (H)**: This is a state function because it depends only on the initial and final states of the system.
- **Heat (q)**: This is a path function because it depends on the process taken to transfer energy into or out of the system.
- **Free Energy (G)**: This is also a state function as it depends only on the state of the system.
- **Work (W)**: This is a path function because the amount of work done depends on the path taken to change the state of the system.

4. **Conclusion**:
- From the analysis, we can conclude that the state functions among the given options are **Enthalpy** and **Free Energy**.

### Final Answer:
- The correct state functions are **Enthalpy** and **Free Energy**.