Questions: Question 5 2 pts Which of the following thermodynamic quantities are NOT state functions: heat (q), work (w), enthalpy change (ΔH), and/or internal energy change (ΔU)? q only w only ΔH q and w ΔH and ΔU

Solution Steps

State functions are properties that depend only on the current state of a system, not on the path taken to reach that state. Common examples of state functions include internal energy (\(\Delta U\)), enthalpy (\(\Delta H\)), and entropy.

Heat (\(q\)) and work (\(w\)) are not state functions because they depend on the path taken during a process. The amount of heat transferred or work done can vary depending on how the process is carried out.

• \(q\) only: Incorrect, as both \(q\) and \(w\) are not state functions.
• \(w\) only: Incorrect, as both \(q\) and \(w\) are not state functions.
• \(\Delta H\): Incorrect, as \(\Delta H\) is a state function.
• \(q\) and \(w\): Correct, both are not state functions.
• \(\Delta H\) and \(\Delta U\): Incorrect, as both are state functions.

Final Answer