Final answer:
The correct option for free expansion of an ideal gas under adiabatic conditions is 'A. q=0, ΔT=0, w=0' because there is no heat transfer (q=0), no work done on or by the gas (w=0), and no change in internal energy implies the temperature remains constant (ΔT=0).
Step-by-step explanation:
In an adiabatic process of an ideal gas,
the correct option for free expansion under adiabatic conditions is A. q=0, ΔT≠0, w=0.
This is because, in an adiabatic process, there is no heat transfer, which is denoted by q=0. During free expansion, the gas does no work since it expands against a vacuum, and thus w=0. Despite there being no heat transfer or work done, the temperature of the gas can change in an adiabatic process.
Specifically, during free expansion, the internal energy of the gas does not change (ΔEint=0), so the temperature of an ideal gas remains constant; therefore, ΔT=0, which differs from the normal expectations of an adiabatic process where a temperature change is associated with work done by or on the gas.