Each standard thermodynamic process holds one quantity constant, which simplifies the first law $Q = \Delta U + W$.
The table summarises how the first law applies to each process.
| Process | Constant Quantity | Key Equation | Work Done |
|---|---|---|---|
| Isovolumetric | Volume ($V$) | $Q = \Delta U$ | $W = 0$ |
| Isobaric | Pressure ($P$) | $Q = \Delta U + P \Delta V$ | $W = P \Delta V$ |
| Isothermal | Temperature ($T$) | $Q = W$ | $W = nRT \ln \frac{V_2}{V_1}$ |
| Adiabatic | No heat exchange ($Q = 0$) | $PV^{\gamma} = \text{constant}$ | $W = \frac{P_1V_1 - P_2V_2}{\gamma - 1}$ |
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