Question

Which of the following is true for an adiabatic process?

• A. Temperature remains constant throughout the process
• B. All heat absorbed is equal to work done on the system
• C. Energy change is equal to work done on the system
• D. Energy is static variable and dependent on the path

Hint:

In adiabatic processes, heat transfer is zero, so work entirely changes internal energy.

Answer 1

The Correct Option is C

Concept: An adiabatic process is defined as a process in which: \[ Q = 0 \] From the First Law of Thermodynamics: \[ \Delta U = Q - W \] where: - $\Delta U$ = internal energy change - $Q$ = heat supplied to system - $W$ = work done by system

Step 1: Apply adiabatic condition.
Since: \[ Q = 0 \] Substitute into first law: \[ \Delta U = -W \]

Step 2: Physical interpretation.
This means: - If system does work, internal energy decreases - If work is done on system, internal energy increases Thus energy change is fully governed by work interaction.

Step 3: Check options carefully.
(A) False: temperature can change in adiabatic compression/expansion (B) False: since $Q=0$, no heat-work equality exists (C) True: $\Delta U = -W$ directly relates energy change to work (D) False: internal energy is a state function, not path-dependent Final Answer: \[ \boxed{\text{Energy change is governed by work in adiabatic process}} \]