2. Compare the various says of issue in terms ofpotential and kinetic energy
3. Describe the significant events that take place alengthy a heatingcurve.
You are watching: Is the evaporation of water endothermic or exothermic
4. Interpret a phase diagram.
vaporization condensationevaporation equilibrium vapor pressureboiling point heat of vaporization freezingpoint warm of fusionsublimation deposition heatingcurve phase diagram
Matter on Earthexists as either liquid, solid, or gas. Other than water, many matterexists in a solitary phase (liquid, solid, or gas) however have the right to be made to readjust phaseby including or deleting push or temperature.
Energy and PhaseChanges
According to thekinetic-molecular theory, a substances phase is figured out by the balance of itskinetic and intermolecular forces. What this implies is that you can convertmatter from one phase to one more by simply including or deleting kinetic energy(heat). When attempting to understand also the phase transforms it is essential toremember what is emerging in enperform and exothermic reactions.
|liquid to gas - vaporization, by process of evaporation|
|solid to gas - sublimation|
|liquid to solid - freezing|
|gas to liquid - condensation|
|gregarding solid - deposition|
Evaporation is again explained by theKinetic-molecular concept. When the kinetic power of the molecules in aliquid become greater than the intermolecular attractions in between them,evaporation occurs.
|within a liquid, evaporation is constantly developing to some degree at the surchallenge of the liquid|
|Temperature and also evaporation rate are directly related|
|Liquids through high evaporation prices are sassist to be volatile - commonly flammable because of the presence of organic materials and oxides|
|Evaporation cools a surchallenge or solution by removing the molecules via the highest possible kinetic energy|
|Many options in a closed container are in liquid-vapor equilibrium|
|condensation and also evaporation rates are equal|
|rate of molecules leaving the solution are equal to the molecules entering the liquid|
|The solution is at equilibrium vapor pressure|
The boiling point of a liquid is directly relatedto the vapor press of the liquid. Vapor pressure is a meacertain of thevapor current in a liquid. When the vapor press equals the atmosphericpush boiling occurs. It is necessary to remember that vaporization isan endothermic process as warmth is rerelocated from the liquid with boiling.
|vapor pressure of a liquid is straight related to the temperature applied to the liquid|
|the boiling allude is straight pertained to the atmospheric press exerted on the solution|
|boiling occurs as soon as the vapor push = atmospheric pressure|
|the temperature of a liquid will certainly reprimary consistent at the boiling point until every one of the liquid is vaporized.|
Freezing and also Melting:
The freezing and also melting points of a liquid existat the same temperature and represent an equilibrium between the liquid andsolid phases.
|melting and freezing points are not substantially impacted by atmospheric pressure|
|melting counts on the warmth of fusion which like the boiling is an endothermic process|
|freezing offers the exact same amount of energy as the warmth of fushion bu is an exothermic process|
The heating curve is a representation of thephases of a substance compared to the temperature and internal energy of asubstance. The blue lines reexisting the various phases of a substancewhile the red lines reexisting the heats of fusion and vaporization.
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|endothermic reactions relocate from left to ideal as the products increase in kinetic energy and also become much less organized|
The phase diagram is another representation ofthe internal energy of a substance compared with the press and temperature ofits surroundings.
|temperature and also push are inversely related to the process of vaporization|
|press has little result on the melting and also freezing of a substance|
|the triple allude is a allude wbelow all three phases occur in equilibrium|