# Tag Info

0

If the system is at lower pressures where the ideal gas law is close to valid, then the partial pressure of the volatile species (mole fraction times total pressure) can be used in place of the vapor pressure with the Clausius Clapeyron equation. At higher pressures, the free energy of the liquid is affected by the higher overall pressure, as is the partial ...

2

Two carbon dioxide scrubbers come to mind: lithium hydroxide and soda-lime. (https://en.wikipedia.org/wiki/Lithium_hydroxide)"Lithium hydroxide is used in breathing gas purification systems for spacecraft, submarines, and rebreathers to remove carbon dioxide from exhaled gas by producing lithium carbonate and water: 2 LiOH•H2O + CO2 → Li2CO3 + 3 H2O or ...

2

As the approximation, the saturated vapour pressure does not depend on the total pressure, only on the substance and temperature. (*) If there is nothing but the vapor in the gaseous phase under the piston then the amount of vapor and its pressure accomodate to external pressure. (**) If the external pressure is kept greater than saturated vapor pressure ...

1

The van der Wals expression can be shown graphically at constant temperature by the curve ABCDEFG in following diagramm, if the temperature is lower thant the critical temperature. Try to follow the line. Start at A with a large volume of gas and a small pressure. Increase the pressure. The volume decreases from A to B and C. But after C, along CDE, the ...

2

Fundamentally, the problem is in the problem statement. The proper form for the Van der Waals equation is $[P+(a/V_m^2)](V_m\color{blue}{-b})=RT$ which would give a cubic equation when we try to isolate the molar volume. It is this cubic equation that usually has one or three roots that can be correlated with the possible phases, as described in the other ...

Top 50 recent answers are included