Question

Which of the following is true for an adiabatic process?

• A. \(\Delta H = 0\)
• B. \(\Delta W = 0\)
• C. \(\Delta Q = 0\)
• D. \(\Delta V = 0\)

Hint:

Remember: Adiabatic means “No Heat Exchange”. Therefore \(q=0\) is always the defining condition.

Answer 1

The Correct Option is C

Concept: An adiabatic process is a thermodynamic process in which no heat is exchanged between the system and the surroundings. The defining condition for an adiabatic process is: \[ q=0 \] According to the first law of thermodynamics, \[ \Delta U=q+w \] For an adiabatic process, \[ q=0 \] therefore, \[ \Delta U=w \] Thus, the change in internal energy is entirely due to work done.

Step 1: Recall the definition of an adiabatic process. In an adiabatic process, the system is perfectly insulated. Hence, \[ \boxed{\Delta Q=0} \]

Step 2: Examine other options. \[ \Delta H=0 \] is not generally true. \[ \Delta W=0 \] is also not true because work may be done during expansion or compression. Similarly, \[ \Delta V=0 \] is not a necessary condition.

Step 3: Select the correct statement. The only universally true condition for an adiabatic process is: \[ \boxed{\Delta Q=0} \] Hence, the correct option is \[ \boxed{(3)} \]