When liquid and vapour phases are in equilibrium and liquid are in equilibrium with its vapor the rate of vaporization and the rate of condensation are in?
If solution and gas phases are well stirred (There is no gradient of concentrations in each phase), the process of a evaporation/condensation can be written as the chemical reaction
H2Og = H2O, d[H2Og]/dt = -k1[H2O]g + k2[H2O]. In equilibrium k1[H2O]g = k2[H2O], the rate of vaporization is equal to the rate of condensation. If H2O is consumed in the gas phase, this results in water flux from liquid to gas phase. If temperature changes, this results in water flux from one phase to another.
To exist a dynamic equilibrium between a liquid and its vapour, the rate of evaporation of liquid should be equal to the rate of condensation of vapour. At vapor–liquid equilibrium, a liquid with individual components in certain concentrations will have an equilibrium vapor in which the concentrations or partial pressures of the vapor components have certain values depending on all of the liquid component concentrations and the temperature. When the rate of condensation becomes equal to the rate of vaporization, neither the amount of the liquid nor the amount of the vapor in the container changes. The vapor in the container is then said to be in equilibrium with the liquid. Vapour-liquid Equilibrium is achieved when the partial pressure of the vapour phase is equal to the saturated vapour pressure of the liquid phase at a given temperature. In other words, it is when the two steps are in Equilibrium. Now, some of the vapor molecules condense back into a liquid. The system reaches the point where the rate of evaporation is equal to the rate of condensation. This is considered a dynamic equilibrium between the liquid and vapor phase. 5 – Liquid-Liquid Equilibrium. In liquid-liquid equilibrium, the liquids can either be miscible, partially miscible or immiscible. Miscible liquids are liquids that can mix together to form a single phase. Since both microscopic processes are still in motion, such a situation is often referred to as dynamic equilibrium. The magnitude of the vapor pressure of a liquid depends mainly on two factors: the strength of the forces holding the molecules together and the temperature. Liquid and gas phases are in equilibrium at the boiling temperature. If a substance is in a closed container at the boiling point, then the liquid is boiling and the gas is condensing at the same rate without net change in their relative amount.
Please, don't teach me to elementary things. I'm no longer involved in your useless discussions.
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