Boyle’s law & Gay lucass law

2. Boyle's law is an experimental gas law that describes
how the pressure of a gas tends to increase as the
volume of the container decreases. A modern statement
of Boyle's law is
The absolute pressure exerted by a given mass of an
ideal gas is inversely proportional to the volume it
occupies if the temperature and amount of gas remain
unchanged within a closed system.
Mathematically, Boyle's law can be stated as
where P is the pressure of the gas, V is the volume of the
gas, and k is a constant.
The equation states that the product of pressure and
volume is a constant for a given mass of confined gas as
long as the temperature is constant. For comparing the

3. same substance under two different sets of conditions,
the law can be usefully expressed as:
The equation shows that, as volume increases, the
pressure of the gas decreases in proportion. Similarly, as
volume decreases, the pressure of the gas increases. The
law was named after chemist and physicist Robert Boyle,
who published the original law in 1662

4. Boyle's law is often used as part of an explanation on
how the breathing system works in the human body. This
commonly involves explaining how the lung volume may
be increased or decreased and thereby cause a relatively
lower or higher air pressure within them (in keeping with
Boyle's law). This forms a pressure difference between
the air inside the lungs and the environmental air
pressure, which in turn precipitates either inhalation or
exhalation as air moves from high to low pressure .

5.  Paint and liquefied gas are filled inside the can of
spray paint .
 The boiling point of liquefied gas is lower than room
temperature .
 Who the hozzle goes down the propellant expands
into gas .
 Product escapes out where there is less pressure .

7. Arrange the quill tube horizontally on a stand.
The length of the air column is measured using a metre
scale.
Vertical heights at the two ends of mercury thread from
the table are also measured using a metre scale.
The difference between them gives the vertical height ‘h’
of the mercury thread. Here h=0. So pressure inside the
tube is also H, which is the atmospheric pressure.ie; 76 cm
of Hg
The quill tube is then placed in a slanting position with the
open end upwards.
The length of the air column is measured and the vertical
height, h of Mercury is noted. Now the pressure inside the
tube, P=H + h.
Quill tube is then placed in different positions, such as:
vertical position with open end upwards and with open
end downwards, slanting position with open end
downwards and measure its corresponding length of the
air column l and vertical height h.

9. 0
0.5
1
1.5
2
2.5
0 0.5 1 1.5 2 2.5 3 3.5
volume
P
0
0.5
1
1.5
2
2.5
0 10 20 30 40
p
time

10. 0.01
0.0105
0.011
0.0115
0.012
0.0125
0 1 2 3 4 5 6 7 8 9
Time
v

12. 0.01
0.0105
0.011
0.0115
0.012
0.0125
0 1 2 3 4 5 6 7 8 9
volume
p
0.01
0.0105
0.011
0.0115
0.012
0.0125
0 1 2 3 4 5 6 7 8 9
Time
p

13. 0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
time
v
0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
time
p*v

14. Gay-Lussac's law can refer to several discoveries made by
French chemist Joseph Louis Gay-Lussac (1778–1850)
and other scientists in the late 18th and early 19th
centuries pertaining to thermal expansion of gasses and
the relationship between temperature, volume, and
pressure .
Mathematically, Gay – lussac law can be stated as :
He is most often recognized for the Pressure Law which
established that the pressure of an enclosed gas is
directly proportional to its temperature and which he
was the first to formulate (c. 1808). He is also sometimes
credited , rightfully according to many modern scholars ,
with being the first to publish convincing evidence that,
in Gay-Lussac’s shows the relationship between the

15. pressure and temperature of a fixed mass of gas' kept at
a constant volume .
These laws are also known variously as the Pressure Law
or Amontons's law and Dalton's law respectively .
the law can be usefully expressed as :

16. Immerse the bulb of the Gay-Lussac apparatus in boiling water in a
2000ml beaker. Allow the system to come to equilibrium and record
the pressure and temperature.
Pour out about one-half of the boiling water and refill the beaker
with tap water. Allow the system to reach equilibrium again. Record the
pressure and temperature.
Empty the beaker and fill the beaker with tap water. Allow the
system to reach equilibrium again. Record the pressure and
temperature.
Place the bulb of the apparatus in a beaker containing a slushy
mixture of ice and water. Allow the system to reach equilibrium. Record
the pressure and temperature.
Repeat Step 4 using a mixture of dry ice (solid carbon dioxide) and
acetone (optional).
Repeat Step 4 using liquid nitrogen in a large Dewar flask (optional)..

18. 0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
temperature
p
0.01
0.0105
0.011
0.0115
0.012
0.0125
0 1 2 3 4 5 6 7 8 9
Time
p

19. 0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
time
0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
time
p/T

21. 0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
temperature
p
0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
time
p

22. 0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
time
T
0.01
0.0105
0.011
0.0115
0.012
0.0125
0 2 4 6 8 10
time

23. If the volume from 3 L to 1L, the pressure goes from 93000 Pa to
220000Pa .
If the volume from 1L to 3L, the pressure increases from 93000Pa
to 35000Pa .
I can infer that the relationship between pressure and volume is an
inverse relationship. As the volume increases, the pressure
decreases .
In this experiment, the temperature and the amount of gas is
assumed to remain constant .
in this experiment we have the gay lussac law , this is the
relationship between pressure and temperature .
in this law the volume is constant .
if the temperature is increase the pressure is increase .
if the temperature is decrease the pressure is decrease , .