Vaporization Condensation
Vaporization Condensation - Related Videos
02:39
Phase Transitions: Vaporization and Condensation
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2020
The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize (convert into vapor). The process is called vaporization—a surface phenomenon. Vaporization occurs when the thermal motion of the molecules overcome the intermolecular forces, and the molecules (at the surface) escape into the gaseous state. When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules...
02:34
Vapor Pressure
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2020
When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules move randomly about, they will occasionally collide with the surface of the condensed phase, and in some cases, these collisions will result in the molecules re-entering the condensed phase. The change from the gas phase to the liquid is called condensation. When the rate of condensation becomes equal to the rate of vaporization, neither the amount of the liquid nor the amount of the vapor...
11:32
Vapor-liquid Equilibrium
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2023
Source: Michael G. Benton and Kerry M. Dooley, Department of Chemical Engineering, Louisiana State University, Baton Rouge, LA Vapor-liquid equilibrium is paramount in engineering applications such as distillation, environmental modeling, and general process design. Understanding the interactions of components in a mixture is very important in designing, operating and analyzing such separators. The activity coefficient is an excellent tool for relating molecular interactions to mixture...
03:28
Vapor Pressure Lowering
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2020
The equilibrium vapor pressure of a liquid is the pressure exerted by its gaseous phase when vaporization and condensation are occurring at equal rates: Dissolving a nonvolatile substance in volatile liquid results in a lowering of the liquid’s vapor pressure. This phenomenon can be explained by considering the effect of added solute molecules on the liquid's vaporization and condensation processes. To vaporize, solvent molecules must be present at the surface of the solution. The presence of...
01:18
Vaporization
0 Views •
2019
The physical form of a substance changes by changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize (convert into vapor). The process is called vaporization—a surface phenomenon. For vaporization to occur, kinetic energy must be greater than the intermolecular forces that keep molecules bonded. The amount of energy needed to vaporize a quantity of liquid at a given pressure and a constant temperature is called the heat of vaporization. When...
FAQs
Intermolecular forces determine how strongly molecules remain associated in the liquid. During vaporization, more energy is required when those attractions are harder to overcome. Condensation reverses this energy change as gas molecules return to the liquid state. This relationship helps chemists interpret why energy flow is central to controlling phase transitions and heat transfer.
At phase equilibrium, vaporization and condensation continue simultaneously at equal rates, so the amounts of liquid and gas remain constant even though molecules still exchange phases. Changing temperature or pressure can disturb this balance and shift the relative amounts of each phase. Recognizing dynamic equilibrium is important when analyzing closed systems and chemical processing conditions.
Temperature changes the energy available to molecules, while pressure changes the conditions under which liquid and gas phases are favored. Adjusting either variable can promote vaporization or condensation and alter the position of phase equilibrium. Chemists use this control to manage heat transfer, separate liquid mixtures, and regulate processes involving solvents or other volatile substances.
Evaporation and boiling both represent vaporization, but they occur under different conditions. Evaporation can occur from a liquid surface, whereas boiling represents more extensive vapor formation when the system reaches the required condition throughout the liquid. This distinction helps explain why liquid loss can occur gradually during handling, while controlled boiling supports procedures such as distillation.
Distillation uses vaporization to move components from a liquid mixture into the gas phase, followed by condensation to collect the resulting liquid. Temperature, pressure, and energy flow must be controlled so the phase changes occur in a useful sequence. The method supports purification and separation of liquid mixtures by exploiting their different tendencies to enter the vapor phase.
Solvent recovery relies on transferring a solvent into the vapor phase and then returning it to a liquid for collection. Managing temperature, pressure, and energy flow allows the process to recover usable solvent while separating it from other material. This application connects phase-change control with laboratory purification and industrial chemical processing.
Vaporization and condensation provide a way to move energy through a system. Vaporization involves energy uptake, while condensation accompanies the return to the liquid state and associated energy release. Refrigeration uses this paired behavior to support heat transfer, making control of phase transitions relevant to engineered cooling systems as well as chemistry.
Cloud formation illustrates the broader environmental significance of these transitions. Water entering the gas phase and later returning to liquid contributes to the movement of matter between atmospheric and condensed states. The same principles of energy exchange, temperature, and equilibrium used in chemistry help interpret condensation in natural systems and connect laboratory concepts with atmospheric behavior.