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Why are liquids like ether and acetone kept in cool places?
well ether tend to evaporate easily in room temperature, lowering the temperature would probably lower the chance of it evaporating. Also, they're both flammable; keeping them below their flash point reduces the chance of an explosion.
How can the rate of evaporation of water from an open beaker be decreased?
The rate of evaporation of water from an open beaker can be decreased by placing a lid or cover over the beaker to reduce the surface area exposed to the air and prevent airflow. Additionally, lowering the temperature of the surroundings can help slow down the evaporation process. Adding solutes like salt to the water can also decrease the rate of evaporation.
What the develop and hypothesis on keep your candy cool with the power of Evaporation?
To develop a hypothesis, you could state that if you wrap candy in a damp paper towel and place it in a container in front of a fan, then the evaporation of water from the paper towel will absorb heat from the candy, keeping it cool. The hypothesis predicts the outcome of the experiment based on the proposed relationship between evaporation and cooling.
Why should we keep ether and acetone in cool places?
Ether and acetone are both highly flammable liquids with low flash points, so storing them in cool places helps reduce the risk of ignition. Additionally, keeping these chemicals in cool environments helps prevent evaporation and potential loss of chemical potency.
Compare and contrast between boiling and evaporation?
Evaporation takes place at any temperature but boiling takes place only at a substance's boiling point.
How leaves cool the tree?
leaf of a tree have water on them always and when evaporation takes place it will cool the plant
Why does the evaporation of sweat cool your body on the warm day?
Evaporation is the vaporization that takes place only on the surface of a liquid. Evaporation takes up energy - and it takes up that energy from the warm surface of your skin. Thus, when sweat evaporates, it takes heat from your skin, cooling it.
What is a scientific principle concerning a transfer of heat that takes place during the evaporation of liquids?
The latent heat of evaporation - (if you wet your finger and then blow on it it feels cool this is because the evaporating water takes heat out of your finger). This heat is recovered when the liquid re-condenses - (water droplets forming on the outside of a cold glass of beer heat the glass with this recovered energy and the beer in the glass warms up far more quickly than it would if the air was dry).
What do you do when your really hot?
Drink cool -- not cold -- liquids, and rest in a cool place with a breeze, if possible.
When your body sweats which process is at work too cool your body off?
The process of evaporation helps cool your body when it sweats. As sweat evaporates from your skin, it takes heat with it, helping to lower your body temperature.
Why are liquids like ether and acetone kept in cool places?
well ether tend to evaporate easily in room temperature, lowering the temperature would probably lower the chance of it evaporating. Also, they're both flammable; keeping them below their flash point reduces the chance of an explosion.
We cool ourselves by sweating and allowing evaporation to take what from your bodies?
We cool ourselves by sweating and allowing evaporation to take excess heat from our bodies. As sweat evaporates, it takes away heat energy from our skin, cooling us down in the process.
Can evaporation take place without the increase in temperature Give example.?
Yes. When you cool by sweating - it drops.
What is the independent variable for keep your candy cool with the power of evaporation?
hypothesis of candy cool with the power of evaporation
What are the things takes place in a girl's periods?
cool is goog...
Why does a liquid cool when evaporated?
Evaporation Takes Place Layer By Layer. Then Heat, In The Stages Of Evaporation Just Effects The First Layer Of The Liquid . Heat Makes An Increase Of Enegry Between The Particles. The Particles, With That Energy, Trys To Move And Seperate ThemSelves From The Whole Liquid. The Higher Engery Partides Rise, Leaving The Less Engery Ones Behind, There For Making The Liquid Cool.
Why does the evaporation of sweat cool your body on a warm day?
When sweat evaporates from your skin, it takes away heat energy from your body, cooling you down.
