chemistry investigatory project on to determine the rate evaporation of different liquids

this file contains investigatory projects on chemistry topic to determine the rate of evaporation of different liquids like:- water, aldehyde, ketone, ethanol. of you like follow me on my instagram @vishal2782003

1. KENDRIYA VIDYALA No. 1
SHAHJAHANPUR



CHEMISTRY
INVESTIGATORY PROJECT

2. Aim Of The Experiment
To Determine the Rate of Evaporation
of different liquids .






Submitted By:
VISHAL SHARMA

Class:
XII A

Roll No. :
Submitted To:
Mr. VISHNU KUMAR SAHU
Signature:

3. -:INDEX:-

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. Bibliography

4. Certificate
This is to certify that Vishal Sharma of Class- XII,
section- A has successfully completed the
Chemistry investigatory project entitled.
To Determine the Rate of
Evaporation of different liquids.
This report is the result of My endeavours
and research. It is finalized under The guidance
and supervision in the academic
year 2020-2021 by Mr. Vishnu Kumar Sahu.


Submitted for CBSE Examination
held in Chemistry lab at
Kendriya Vidyalaya No. 1 Cantt Shahjahanpur.

Examiner’s signature

5. In the accomplishment of this project successfully many
people have bestowed on me their blessings and their
Immense support.
I would like to express my special thanks of gratitude to my
Teacher Mr Vishnu Kumar Sahu as well as our principal Mr
Ratan Kumar who gave me the golden opportunity to do this
wonderful project on the topic “To Determine the Rate of
Evaporation of different liquids..” Which also helped me in
doing a lot of research and I came to know about so many
new things.
Secondly I would also like to thank my parents and my
Friends who helped me a lot in finalizing this project within
the given time.
Last but not the least I would like to thank The Lab assistant
all the people who had helped me directly or indirectly
during the completion of this project.


NAME- VISHAL SHARMA
CLASS-XII A

6. THEORY INVOLVED
1. RATE OF EVAPORATION
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.

FACTOR’S INFLUENCING THE RATE OF EVAPORATION
 TEMPRATURE
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.
 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.

7. 2. SURFACE AREA AND TEMPRATURE

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
3. INTERMOLECULAR FORCES
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.

8. ETHANOL
IUPAC Name Ethanol
Other Names Ethyl Alcohol , Grain Alcohol ,
Hydroxyethane , Drinking Alcohol
Molecular Formula C₂H₅OH
Structure

PROPERTIES
Molar Mass 46.06844 g/mol
Appearance Colourless clear liquid
Density 0.789 g/cc
Melting Point -114.3 ⁰C (158.8 K)
Boiling point 78.4 ⁰C (351.6 K)
Solubility in Water Fully miscible
Acidity 15.9(H⁺ from OH group)
Viscosity 1.200 mPa (cP) at 20⁰C
Dipole Moment 5.64fc/f (1.69D ) (gas)

ACETALDEHYDE
IUPAC Name Ethanal
Other Names Acetaldehyde
Molecular Formula C₂H₄O
Structure

PROPERTIES
Molar Mass 44.05g/mol
Appearance Colourless liquid , fruity odour
Density 0.778 g/cc
Melting Point -123.5 ⁰C
Boiling Point 20.2 ⁰C

9. Solubility in Water Fully miscible
Viscosity 0.215 at 20 ⁰C
Dipole Moment 2.7 D

ACETONE
IUPAC Name Propanone
Other Names Dimethyl ketone
Molecular Formula CH₃COCH₃
Structure

PROPERTIES
Molar Mass 58.08 g/mol
Appearance Colourless clear liquid
Density 791 kg/m³
Melting Point -95 °C
Boiling Point 56 °C
Solubility in Water Fully miscible
Viscosity 0.316 cp
Dipole Moment 2.69 D

WATER
IUPAC Name Oxidane
Other Names Water, Dihydrogen monoxide,
Aqua
Molecular Formula H₂O
Structure

PROPERTIES
Molar Mass 18.01528 g/mol

10. Density 1 g/cc
Appearance Colourless clear liquid
Melting Point 0 ⁰C
Boiling Point 100 ⁰C
Viscosity 0.894 cp
Dipole Moment 1.85D

USES OF SOLUTION

1. USES OF ACETONE
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 litres 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 fibres.
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.

11. 2. USES OF WATER
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.

3. USES OF ACETALDEHYDE
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 catalysed by an alcohol dehydrogenase , now operating the
opposite direction.

12. 4. USES OF ETHANOL
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.

13. EXPERIMENT

AIM:- TO ANALYSE SAMPLE OF DIFFERENT LIQUIDS

PROCEDURE
1. KEEPING THE TEMPRATURE SAME
i. Take three beakers of equal volume and label them as A,B ,C,D.
Pour 10ml of each liquid in these beakers.
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.
2. BEAKERS OF DIFFERENT SURFACE AREA
Put 10ml of different liquids in beakers of different surface areas.
3. HEATING THE BEAKERS
Heat the beakers to different temperatures and note their volumes.

14. 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
OBSERVATION TABLE
Variation of volume liquids evaporate in different surface area
.
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
Variation of rate of evaporation of liquids at different temperatures
.
Temperature (In Degree Celsius )
Liquids(ml) 25
o
27
o
29
o
31
o
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

15. 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.

RESULT
This experiment clearly establishes the relation between the
rate of evaporation of different liquids and the factors on
which it depends .

16. Reference Taken From Class XII NCERT Text book and
Pradeep’s Chemistry Class XII
WEBSITES USED FOR REFERENCE:-
1. www.google.com
2. www.Wikipedia.com
3. www.encyclopedia.com
4. www.youtube.com
5. www.vectorstocks.com

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