In a chemical system with positive change in internal energy (\(\Delta E > 0\), indicating energy gain), heat is absorbed (\(q > 0\)), and the system undergoes expansion, making it feel cool to the touch.
Let's analyze each statement:
a. **The system has gained energy.**
- True. Since \(\Delta E > 0\), the system has gained energy.
b. **The system has lost energy.**
- False. \(\Delta E > 0\) indicates a gain in energy, not a loss.
c. **Heat is flowing into the system.**
- True. Since \(q > 0\), heat is being absorbed by the system.
d. **Heat is flowing out of the system.**
- False. \(q > 0\) implies heat is entering, not leaving the system.
e. **The system undergoes an expansion.**
- True. \(w \geq 0\) indicates work is done on the system, possibly causing expansion.
f. **The system undergoes a compression.**
- False. \(w \geq 0\) suggests work is done on the system, not compression.
g. **The system would feel cool to the touch.**
- True. When heat is absorbed (\(q > 0\)), it can make the system feel cool.
h. **The system would feel warm to the touch.**
- False. If heat is absorbed (\(q > 0\)), the system would feel cool, not warm.
Correct statements: a, c, e, g