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CGP EDU Academic Team
Published on: September 12, 2026
If an ideal gas expands adiabatically, it does positive work and its internal energy decreases.
Text Solution
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A
In an adiabatic process, there is no heat exchange with the surroundings (Q = 0). According to the first law of thermodynamics, we have:
\[ \Delta U = Q - W \]
Since Q = 0, it simplifies to:
\[ \Delta U = -W \]
This means that if the gas does positive work (W > 0), the internal energy (U) of the gas must decrease (\Delta U < 0). Therefore, the statement is true.
\[ \Delta U = Q - W \]
Since Q = 0, it simplifies to:
\[ \Delta U = -W \]
This means that if the gas does positive work (W > 0), the internal energy (U) of the gas must decrease (\Delta U < 0). Therefore, the statement is true.
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