DOWNLOAD HSEB NOTES ON THERMAL PROPERTIES AND IDEAL GASES | CHEMISTRY
CLASS : 11
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Boyle's Law :
Pressure and volume
of an enclosed sample of gas
If you have
ever tried to
force in the
plunger of a
syringe or a
bicycle pump while sealing the opening with a
finger you will
know that there
is some sort
of inverse relationship between the force you apply and how far
in you can push it. Greater and greater
forces are needed
to push the
plunger further and
further in. In other
words, the smaller
you make the
volume of the
enclosed air, the
bigger the pressure
of that enclosed
air. Scientific progress is closely related to technological
development : they feed and support each
other. No real
progress could be
made in the
study of gases until the 17th
century when the
first efective vacuum
pumps were developed. An Englishman named
Robert Boyle designed
some excellent vacuum
pumps which allowed him
to take very
accurate measurements over
a good range
of pressures and volumes.
He discovered the
startlingly simple fact
that the pressure and volume are not just vaguely inversely related, but
are exactly inversely proportional.
Definition:
Boyle's Law:
The
pressure of a
fixed quantity of gas is inversely proportional
to the volume
it occupies so
long as the temperature
remains constant. The standard modern
laboratory version of
his apparatus consists
of a vertical glass tube
sealed at the
top end, with
the other end
filled up to
a certain point with oil.
This end is
attached to an
oil reservoir, which
in turn has a layer of air
above it (which
the oil keeps
separate from the
trapped air.) The air trapped in
the tube by
oil is then
subjected to various
pressures (usually a bicycle pump
is used to
pump in air
through a non-return
valve) which are registered by a
Bourdon gauge. As
the air pressure
above the oil
inside the reservoir is increased,
the pressure of
the oil on
the trapped air
increases. The change in volume
of the air
in the tube
can be read
of on a
scale next to it. (NOTE TO SELF:
Include a diagram
here!!!)
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