The Clausius-Clapeyron Calculator is a powerful tool used to determine the vapor pressure of a substance at a different temperature. This calculation is crucial in various scientific and industrial applications, helping predict how the vapor pressure of a substance changes with temperature. The formula used for this calculation is:
P2 = P1 * exp((ΔH_vap / R) * ((1 / T1) - (1 / T2)))
Where:
- P2 is the vapor pressure at temperature T2.
- P1 is the vapor pressure at temperature T1.
- ΔH_vap is the heat of vaporization.
- R is the universal gas constant (approximately 8.314 J/(mol·K)).
- T1 is the initial temperature in Kelvin.
- T2 is the final temperature in Kelvin.
General Terms Table
To assist users in understanding the various terms associated with the Clausius-Clapeyron Calculator, here’s a helpful table of general terms commonly searched for:
| Term | Definition |
|---|---|
| Vapor Pressure | Pressure exerted by a vapor in equilibrium |
| Heat of Vaporization | Energy required to turn a substance into vapor |
| Universal Gas Constant | A fundamental physical constant |
| Kelvin | Unit of temperature in the International System of Units |
Example of Clausius-Clapeyron Calculator
Let’s consider an example to illustrate the application of the Clausius-Clapeyron equation. Suppose we have a substance with a vapor pressure of 1000 Pa at an initial temperature (T1) of 300 K. The heat of vaporization (ΔH_vap) is 40 kJ/mol. Now, we want to find the vapor pressure at a final temperature (T2) of 350 K.
Applying the formula:
P2 = 1000 * exp((40 * 1000 / (8.314)) * ((1 / 300) - (1 / 350)))
Calculating this expression gives us the vapor pressure at T2.
Most Common FAQs
A: Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases.
A: The heat of vaporization is experimentally determined by measuring the heat required to vaporize a specific amount of substance.
A: The universal gas constant relates energy and temperature in the equation, providing a consistent unit of measurement.