Biogenic Sulfur Gases as Biosignatures on Temperate Sub-Neptune Waterworlds
Chemistry project Class 12th ( Rate of evaporation of different liquids )
1.
2. To Determine the Rate of Evaporation
of different liquids and then
Compare it with respect to different
factors and density.
VIDHI KISHOR
12TH F
Dr. PRATHIBHA SINGH
3. 1. Certificate
2. Acknowledgement
3. Theory Involved
4. Uses of solutions
5. Experiment
a. Materials required
b. Procedure
c. Observation table
d. Conclusions
f. Result
6. Bi bliography
4. Guided By :-
Class :- XII – F
Year :- 2016- 2017
Roll No :- ________________
School :- Mount Carmel School
Certified to be the bona fide work done by-
Miss __________________ of class XII-F in the
Chemistry Lab during the year 2016-2017.
Date :-________
Submitted for Central Board of Secondary
Education.
Examination held in Chemistry lab at Mount
Carmel School.
EXAMINER
Date :-_________
5. I wish to express my deep
gratitude and sincere thanks to my
chemistry teacher, Dr Pratibha Singh,
Mount Carmel School for her
encouragement and for all the facilities
that she provided for the completion of
this project work. I take this opportunity
to express my deep sense of gratitude for
her invaluable guidance, constant
encouragement , immense motivation ,
which has sustained my efforts at all the
stages of this project work. I am also
thankful to Mrs. Jiji (Lab Assistant )
without whom all this would never have
been possible .
6. A liquid’s surface area and temperature affect its rate of
evaporation. Evaporation rate also depends upon the
type of liquids, since liquids are made up of different
molecules and differ in the amount of abstraction that
exists between the molecules.
FACTORS INFLUENCING THE RATE OF EVAPORATION
Temperature:
It is also affected by temperature. As the temperature of air is
increased, its capacity to hold moisture also increases.
Any increase in air temperature raises the temperature of
liquid at the evaporation source which means that more
energy is available to the liquid molecules for escaping from
liquid to a gaseous state. Hence evaporation is directly
proportional to the temperature of evaporating surface.
Warmer the evaporating surface, higher the rate of
evaporation.
Air-pressure:
Evaporation is also affected by the atmospheric pressure
exerted on the evaporating surface. Lower pressure on open
surface of the liquid results in the higher rate of evaporation.
7. Relative humidity:
The rate of evaporation is closely related with the relative
humidity of air. Since the moisture holding capacity of air at a
given temperature is limited, drier air evaporates more liquid
than moist air. In other words, higher the vapour pressure,
lower the rate of evaporation. It is a common experience that
evaporation is greater in summer and at mid-day than in
winter and at night.
Because molecules or atoms evaporates from a liquid’s
surface area allows more molecules or atoms to leave the
liquid, and evaporation occurs more quickly. For example-
same amount of water will evaporate faster if spilled on a
table than it is left in the cup. Higher temperature also
increases the rate of evaporation. At higher temperature
molecules or atoms have a higher average speed. And
more particles are able to break free on liquid’s surface.
8. Most liquids are made up of mutual attraction among
different molecules help explain why some liquids
evaporates faster than others. Attractions between
molecules arise because molecules typically have
regions that carry a slight positive charge. These
regions of electric charges are created because some
tons in a molecule are often more electronegative than
the hydrogen atoms. Intermolecular attractions affect
the rate of evaporation of a liquid because strong
intermolecular attraction hold the molecules in a liquid
more tightly. As a result ,liquids with strong
intermolecular attractions evaporate more slowly than
those with strong intermolecular forces this is the
reason why gasoline evaporates faster than water. The
stronger the forces keeping the molecules together in
the liquid state the more energy that must be input in
order to evaporate them.
13. An important industrial use of acetone involves its reaction
with phenol for the manufacture of Bishenol A. Bishenol A
is an important component of many polymers such as
Polycarbonates, polyurethanes and epoxy resins. Acetone is
also used extensively for the safe transporting and storing
of acetylene. Vessels containing a porous material are first
filled with acetone followed by acetylene, which dissolve
into acetone.One litres of acetone can dissolve around 250
liters of acetylene. Acetone is often the primary
component in nail polish remover. Acetonitrile,an organic
solvent ,is used as well ,Acetone is also used as a superglue
remover. It can be used for thinning and cleaning fiberglass
resins and epoxies . It is a strong solvent for most plastics
and synthetic fibers. Acetone can also dissolve many
plastics, including those used in consumer targeted
Nalgene bottles. Acetone is also used as a drying Nalgene
bottles. Acetone is also used as a drying agent, due to the
readiness with which it binds to water, and its volatility.
Acetone can also be used on hair. It can be used a rinse
before shampooing to remove build up, Oil and hard
water minerals.
14. From biological standpoint, water has
many distinct properties that are critical
for the proliferation of life that set it
apart from other substances. It carries
out this role by allowing organic
compounds to react in ways that
ultimately allow replication. All known
forms of life depend on water.
Water is vital both as a solvent in many
ways and respiration. Photosynthetic
cells use the sun’s energy to split off
water’s hydrogen from oxygen. Hydrogen
is then combined with CO2 in the
process. Water is also central to acid
base neutrality and enzyme function.
15. It is flammable liquid with a fruity smell.
Acetaldehyde occurs naturally in ripe fruit,
coffee and fresh bread and is produced by
plants as a part of their normal metabolism. It is
popularity known as the chemical that causes
hangovers.
In the chemical industry, acetaldehyde is used
as an intermediate in the production of acetic
acid, certain esters and a number of other
chemicals.
In the liver, the enzyme alcohol dehydrogenase
converts ethanol into acetaldehyde, which is
then further converted into acetic acid by
alcohol dehydrogenase .The last step of alcohol
fermentation in bacteria ,plants and yeast
involve the conversion of pyruvate into
acetaldehyde by enzyme pyruvate
decarboxylase, followed by the conversion of
acetaldehyde into ethanol. The latter reaction is
again catalyzed by an alcohol
dehyrogenase,now operating the opposite
direction.
16. The largest single use of ethanol is an a motor fuel
and fuel additive. Ethanol may also be utilized as a
rocket fuel and is currently used in lightweight rocket
powered racing aircraft. Ethanol combustion in an
internal combustion engine yields many of the
products of incomplete combustion produces by
gasoline and significantly larger amounts of
formaldehyde and related species such as
acetaldehyde.
Ethanol fuels flue-less, real flame fireplaces. Ethanol
is kept in a burner containing a wick such as glass
wool, a safety shield to reduce the chances of
accidents and an extinguisher such as a plate or
shutter to cut off oxygen . It provides almost the
same visual benefits of a real flame log or coal fire
without the need to vent the fumes via a flue as
ethanol produces very little hazardous carbon
monoxide and a little or no noticeable scent . It does
emit carbon dioxide and requires oxygen.
Therefore,external ventilation of the room containing
the fire is needed to ensure safe operation .Ethanol is
an important industrial ingredient and has
widespread use as a base chemical for other organic
compounds . These include ethyl halides, ethyl esters
and butadiene.
17.
18. PROCEDURE
i. Take three beakers of equal volume and lable
them as A,B ,C D .Pour 10ml of each liquid in
these beaker.
ii. Find their respective masses using
(density=mass/volume).
iii. Keep the beakers at similar conditions for
30mins after recording their masses.
iv. After half an hour note the masses of these
beakers and calculate the loss in mass of
them.
Put 10ml of different liquids in beakers of
different surface areas.
Heat the beakers to different temperatures
and note their volumes.
19. OBSERVATION
Density of water =1 g/cc
Density of acetone =0.791 g/cc
Density of acetaldehyde =0.78 g/cc
Density of ethanol =0.789 g/cc
Now as we have taken 10ml of all substances , therefore
their respective masses will be:
Mass of 10ml water =10gm
Mass of 10ml acetone =7.9gm
Mass of 10ml acetaldehyde =7.8gm
Mass of 10ml ethanol =7.79 gm
After keeping the beakers at room temperature for half
an hour we find the remaining masses to be:
Mass of remaining water = 9.9 gm
Mass of remaining acetone =7.5gm
Mass of remaining acetaldehyde =7.4gm
Mass of remaining ethanol =7.6 gm
20. OBSERVATION TABLE
Different
surface
area
Acetone
(ml)
Ethanol
(ml)
Water
(ml)
Acetaldehyde
(ml)
Beaker 9.5 9.7 9.9 9.5
Watch
Glass
9.0 9.3 9.7 9.3
Conical
Flask
9.3 9.6 9.9 9.5
Liquids (ml) Temperatures (in Degree Celsius )
25⁰ 27⁰ 29⁰ 31⁰
Acetone 9.5 9.3 9.0 8.8
Water 9.9 9.8 9.6 9.3
Acetaldehyde 9.5 9.3 9.2 9.0
Ethanol 9.7 9.4 9.2 8.9
Variation of volume liquids evaporate in different
surface area.
Variation of rate of evaporation of liquids at
different temperatures.
21. CONCLUSION
From the observation we conclude that loss in
mass is directly proportional to the rate of
evaporation i.e. higher is the loss in mass higher
is the rate of evaporation.
From the observation it is clearly seen that,
rate of evaporation is directly proportional to the
surface area i.e. more the surface area more is
the rate of evaporation.
The rate of evaporation also depends upon the
temperature , more is the energy of the
molecules ,more is the rate of evaporation.
More is the density, less will be the rate of
evaporation.
22. This experiment clearly establishes the
relation between the rate of
evaporation of different liquids and
the factors on which it depends .
