The table below illustrates the differences between boiling and evaporation.
| Boiling | Evaporation |
|---|---|
| A process in which a substance changes its state from the liquid state to the gaseous state | A process in which a substance changes its state from the liquid state to the gaseous state without boiling |
| Fast | Slow |
| Bubbles are formed | No bubbles formed |
| Occurs throughout the liquid | Takes place only from the exposed surface of the liquid |
| Occurs at a definite temperature – Boiling point | Occurs at all temperature |
| Source of energy needed | Energy supplied by surroundings |
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I know this is for high-school purposes and this is a “classic question”, but the only factual difference between evaporation and boiling is that the latter occurs by definition only in a closed system and is defined to happen only when the vapor pressure equals the atmospheric pressure. That is why the bubbles form, as we know.
And one last caveat – make sure you define the vapor pressure as the total pressure of the vapor phase. Not necessarily the pressure that the vapor exerts on the surface of the fluid, or how would bubbles be formed?
Great web resource, though! Keep up the great stuff.
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