In a process, `701 J` of heat is absorbed by a system and `394 J` of work is done by the system. What is the change in internal energy for the process?

Explanation

To find the change in internal energy (ΔU) of the system, we can use the First Law of Thermodynamics, which is given by the equation:

\[ \Delta U = Q + W \]

Where:
- ΔU is the change in internal energy,
- Q is the heat absorbed by the system,
- W is the work done by the system.

### Step-by-step Solution:

1. **Identify the values given:**
- Heat absorbed (Q) = 701 J
- Work done by the system (W) = -394 J (Note: Work done by the system is considered negative in this context because it is work done on the surroundings.)

2. **Substitute the values into the equation:**
\[ \Delta U = Q + W \]
\[ \Delta U = 701 J + (-394 J) \]

3. **Perform the arithmetic:**
\[ \Delta U = 701 J - 394 J \]
\[ \Delta U = 307 J \]

4. **Conclusion:**
The change in internal energy (ΔU) for the process is:
\[ \Delta U = 307 J \]

### Final Answer:
The change in internal energy is **307 Joules**.

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