Slope of the saturated vapor pressure curve, abbreviated as m, describes how the vapor pressure of a substance changes with temperature when the substance is in equilibrium between its liquid and vapor phases. This slope is crucial in thermodynamics, particularly in the Clausius-Clapeyron equation, which relates the change in vapor pressure to temperature. The slope indicates how sensitive the vapor pressure is to changes in temperature.
Implications
- The slope is generally steeper at higher temperatures, indicating that vapor pressure increases rapidly with temperature near the boiling point.
- The slope helps explain phenomena like boiling, condensation, and atmospheric processes, as it governs the relationship between temperature and vapor pressure.
Slope of Saturated Vapor Pressure Curve Formula |
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| \( m \;=\; \dfrac{ 4098 \cdot \left( 0.6108 \cdot exp \cdot \dfrac{ 17.27 \cdot T_{mean} }{ T_{mean} + 273.3 } \right) }{ ( T_{mean} + 273.3 )^2 }\) | ||
| Symbol | English | Metric |
| \( m \) = Slope of Saturated Vapor Pressure Curve | - | \(kPa\;/\;C\) |
| \( exp \) = 2.7183 (Base of Natural Logarithm) | - | \(dimensionless\) |
| \( T_{mean} \) = Mean Daily Air Temperature at 2 Meters Height | - | \(C\) |
