Question

During an adiabatic process in an ideal gas, which of the following is true?

• A. Heat is transferred to the system.
• B. Temperature remains constant.
• C. No heat is transferred to or from the system.
• D. Pressure remains constant.

Hint:

Remember: "Adiabatic" means thermally isolated ($Q = 0$).
Do not confuse adiabatic with isothermal ($T = \text{constant}$). In an adiabatic expansion, the gas temperature will actually drop.

Answer 1

The Correct Option is C

Step 1: Understanding the Question:
The question asks for the defining characteristic of an adiabatic process in an ideal gas system.

Step 2: Key Formula or Approach: This is a definitional thermodynamics question. An adiabatic process is a thermodynamic process in which there is no thermal energy exchange between the system and its surroundings:
\[ Q = 0 \]

Step 3: Detailed Explanation:

• An adiabatic process occurs when the system is enclosed by thermally insulating walls (adiabatic boundaries) or when the process happens so quickly that there is no time for heat exchange to occur.

• Under these conditions, the heat interaction \(Q\) is exactly zero (Option C).

• However, other state properties like temperature, pressure, and volume can change.

• An isothermal process (Option B) is where temperature remains constant.

• An isobaric process (Option D) is where pressure remains constant.

Step 4: Final Answer:
During an adiabatic process, no heat is transferred to or from the system.