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Rolling boil of water in an electric kettle. Boiling or ebullition is the rapid phase transition from liquid to gas or vapour; the reverse of boiling is condensation.Boiling occurs when a liquid is heated to its boiling point, so that the vapour pressure of the liquid is equal to the pressure exerted on the liquid by the surrounding atmosphere.
For example, at any given temperature, methyl chloride has the highest vapor pressure of any of the liquids in the chart. It also has the lowest normal boiling point (−24.2 °C), which is where the vapor pressure curve of methyl chloride (the blue line) intersects the horizontal pressure line of one atmosphere ( atm ) of absolute vapor pressure.
The result is that in dilute ideal solutions, the extent of boiling-point elevation is directly proportional to the molal concentration (amount of substance per mass) of the solution according to the equation: [2] ΔT b = K b · b c. where the boiling point elevation, is defined as T b (solution) − T b (pure solvent).
Two different regimes may be distinguished in the nucleate boiling range. When the temperature difference is between approximately 4 to 10 °C (7.2 to 18.0 °F) above T S, isolated bubbles form at nucleation sites and separate from the surface.
A well-known example of a positive azeotrope is an ethanol–water mixture (obtained by fermentation of sugars) consisting of 95.63% ethanol and 4.37% water (by mass), which boils at 78.2 °C. [10] Ethanol boils at 78.4 °C, water boils at 100 °C, but the azeotrope boils at 78.2 °C, which is lower than either of its constituents. [11] Indeed ...
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These two curves necessarily meet where the mixture becomes purely one component, namely where x 1 = 0 (and x 2 = 1, pure component 2) or x 1 = 1 (and x 2 = 0, pure component 1). The temperatures at those two points correspond to the boiling points of each of the two pure components.
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