Which is clapeyron Clausius equation?

The Clapeyron-Clausius equation is a differential equation giving the interdependence of the pressure and temperature along the phase equilibrium curve of a pure substance. This equation was suggested by B. Clapeyron in 1834 and improved by R. Clausius in 1850.

What does Clapeyron equation describe?

Equation (2.165), which is referred to as the Clapeyron equation, describes a general relationship among the pressure, temperature, volume change, and enthalpy change for a single-component, two-phase system at equilibrium.

What is Clausius-Clapeyron law?

The Clausius Clapeyron equation calculates the rate of increase in vapour pressure per unit increase in temperature. Let T be the temperature and p be the saturation vapour pressure. The Clausius Clapeyron equation for liquid-vapour equilibrium is then used. dpdT=L(T(Vv−Vl))

When can Clausius-Clapeyron be used?

The equation describes the phase transition between two phases of matter that have the same composition. Thus, the Clausius-Clapeyron equation can be used to estimate vapor pressure as a function of temperature or to find the heat of the phase transition from the vapor pressures at two temperatures.

Why is Clausius-Clapeyron equation important?

Equation 23.4. 27 is known as the Clausius-Clapeyron Equation and allows us to estimate the vapor pressure at another temperature, if the vapor pressure is known at some temperature, and if the enthalpy of vaporization is known.

What is the Clausius-Clapeyron relation and why is it important for climate?

The Clausius-Clapeyron relationship predicts an increase in the water holding capacity of air (the saturation water vapor pressure) of approximately 7% per degree Celsius rise in temperature2.

What is Clausius-Clapeyron’s equation of latent heat?

The left hand side is the rate of increase of vapour pressure with temperature, while S2 − S1 is equal to L/T, where L is the specific latent heat of vaporization. Thus we arrive at the Clausius-Clapeyron equation: dPdT=LT(V2−VL).