Solved: Chemistry Question for NEET

NEET ChemistryMedium

The correct option for free expansion of an ideal gas under adiabatic condition is

$q = 0, \Delta T = 0$ and $w = 0$

$q = 0, \Delta T < 0$ and $w > 0$

$q < 0, \Delta T = 0$ and $w = 0$

$q > 0, \Delta T > 0$ and $w > 0$

Step-by-Step Solution

For free expansion, external pressure $P_{ex} = 0$ , so work $w = -P_{ex}\Delta V = 0$ . For an adiabatic process, $q = 0$ . By the first law of thermodynamics, $\Delta U = q + w = 0$ . Since internal energy of an ideal gas depends only on temperature, $\Delta U = 0$ implies $\Delta T = 0$ .

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