Question

For an adiabatic change in a system, the condition which is applicable is

• A. \( q = 0 \)
• B. \( w = 0 \)
• C. \( q = -w \)
• D. \( q = w \)

Hint:

In an adiabatic process, there is no heat exchange with the surroundings, so \( q = 0 \). The change in internal energy is entirely due to work done on or by the system.

Answer 1

The Correct Option is A

In thermodynamics, an adiabatic process is one where no heat is transferred into or out of the system. This means that the system is perfectly insulated from its surroundings. The first law of thermodynamics is given by the equation:

\( \Delta U = q + w \)

where:

• \( \Delta U \) is the change in internal energy.
• \( q \) is the heat exchanged.
• \( w \) is the work done on or by the system.

For an adiabatic process, the condition \( q = 0 \) applies. Thus, any change in the internal energy of the system is solely due to the work done by or on the system and is expressed by:

\( \Delta U = w \)

Therefore, for an adiabatic change in a system, the correct condition is:

\( q = 0 \)

Answer 2

In thermodynamics, an adiabatic process is one in which no heat is exchanged between the system and its surroundings. This means that the heat transfer (\( q \)) is zero. Therefore, the condition that applies to an adiabatic change is:

\( q = 0 \)

This condition is fundamental to understanding adiabatic processes as it differentiates them from other types of thermodynamic processes, such as isothermal processes where temperature remains constant or isobaric processes where pressure remains constant.

Given options:

\( q = 0 \)

\( w = 0 \)

\( q = -w \)

\( q = w \)

The correct choice for an adiabatic change in a system is therefore:

\( q = 0 \)