Search results
Results from the WOW.Com Content Network
Evaporation is a type of vaporization that occurs on the surface of a liquid as it changes into the gas phase. [1] A high concentration of the evaporating substance in the surrounding gas significantly slows down evaporation, such as when humidity affects rate of evaporation of water. [2]
Quantity Description A: Surface area (in m 2) : N: Number of gas molecules t: Time (in s) φ: Flux of the gas molecules (in m −2 s −1) : α: Anomalous evaporation coefficient, 0 ≤ α ≤ 1, to match experimental results to theoretical predictions (Knudsen noted that experimental fluxes are lower than theoretical fluxes) [3]
˙ is the vaporization rate of the droplet (kg.s −1) is the liquid specific heat at constant pressure (J.kg −1.K −1) is the heat flux entering the droplet (J.s −1) The heat flux entering the droplet can be expressed as: [1]
The US data is collected and compiled into an annual evaporation map. [4] The measurements range from under 30 to over 120 inches per year. Formulas can be used for calculating the rate of evaporation from a water surface such as a swimming pool. [5] [6] In some countries, the evaporation rate far exceeds the precipitation rate.
diagram of a double-effect falling film evaporator. Condensing vapors from flash tank B1 heat evaporator A2. •1=feed •2=product •3=steam •4=vapors. In chemical engineering, a multiple-effect evaporator is an apparatus for efficiently using the heat from steam to evaporate water. [1]
The pressure on a pressure-temperature diagram (such as the water phase diagram shown above) is the partial pressure of the substance in question. A phase diagram in physical chemistry , engineering , mineralogy , and materials science is a type of chart used to show conditions (pressure, temperature, etc.) at which thermodynamically distinct ...
The Wells curve demonstrates that respiratory droplets rapidly dry out or fall to the ground after being exhaled. The Wells curve (or Wells evaporation falling curve of droplets) is a diagram, developed by W. F. Wells in 1934, which describes what is expected to happen to small droplets once they have been exhaled into air. [1]
In the case of an equilibrium solid, such as a crystal, this can be defined as the pressure when the rate of sublimation of a solid matches the rate of deposition of its vapor phase. For most solids this pressure is very low, but some notable exceptions are naphthalene , dry ice (the vapor pressure of dry ice is 5.73 MPa (831 psi, 56.5 atm) at ...