Adiabatic Processes

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An ideal gas undergoes reversible adiabatic compression. Which of the following correctly describes the thermodynamic changes during this process?

RankGuru · Accepted Answer

An adiabatic process is defined as one in which no heat is exchanged between the system and its surroundings, so $q = 0$ by definition. Applying the first law: $\Delta \cup = q - w = 0 - w = -w$. During compression, work is done ON the gas by the surroundings, so $w < 0$ (work done by the system is negative in compression). Therefore $\Delta \cup = -w > 0$, meaning internal energy increases. For an ideal gas, internal energy depends only on temperature, so an increase in $U$ implies an increase in $T$. This is why a bicycle pump gets warm during rapid inflation — an example of adiabatic compression. Option B describes adiabatic expansion, not compression. Option C is wrong because heat exchange $q > 0$ contradicts the adiabatic condition. Option D would apply to an isothermal process for an ideal gas, not an adiabatic one. This is a concept-rich NCERT topic distinguishing adiabatic from isothermal processes. Plausibility check: compressing any gas does work on it, increasing its energy and temperature, regardless of the working substance.

Adiabatic Processes

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