Vapor implies the existence of a condensed phase that is the source or destination of the gas, or with which the gas may be in equilibrium; while gas does not make such an assumption. By definition vapor pressure seems the pressure of vapor ABOVE the liquid which is in equilibrium with liquid and how the hell we are applying the concept of vapor pressure in open container while discussing boiling? The equilibrium vapor pressure varies with temperature because of two factors - 1)kinetic energy of particles and 2) number density.
Both increase non-negligibly with temperature. The surface of the liquid is not something that simply compresses a gas. It also evaporates. Without understanding this, one cannot distinguish between options B and C.
vapor shower, I've been reading about vapor pressure and it's a bit confusing. For example when water is in equilibrium between the solid and liquid phase, my textbook says that the vapor pressure is equal betwe... The partial pressure of vapor is approximately equal to (saturated) vapor pressure and the pressure difference to external pressure is compensated by partial pressure of the system air. If the mass transfer is faster than evaporation, the open system does not reach saturation and vapor partial pressure is smaller than (saturated) vapor pressure. thermodynamics - Does the term "vapor pressure" even mean anything in ...
vapor shower, At the right low gas pressure means no liquid; increasing pressure below the critical T eventually induces liquid formation in equilibrium; attempts to increase pressure simply increase liquid while decreasing vapor at constant pressure. Eventually there is no more vapor and pressure on the liquid measures the compressibility of the liquid. Vapor pressure or equilibrium vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature in a closed system.
