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P1 * V1=P2 * V2
14.7psi * 20 cubic inches=29.4psi * V2
Note 1: As one can see, to make the right side of the equation proportionate to the left side, one must substitute a smaller volume than V1 into the right side of the equation.
14.7psi * 20 cubic inches=29.4psi * 10 cubic
inches
294 psi per cubic inch=294 psi per cubic inch
From analyzing this formula, one can see that it will always work according to the fact that as pressure increases the volume decreases and vice versa, because the two sides of the equation must counter balance the other.
Our purpose in our experiment was not to compare
the relationship between pressure and volume, but to compare the
relationship between the interior pressure(inside a balloon) required
to overcome the pressure exerted on it and burst the balloon.
We found that the interior pressure required to burst a balloon
increased at an extremely constant rate. Due to the fact the interior
pressure needed to pop a balloon increased at a constant rate,
we knew the relationship between the two variables would be linear.
This conclusion that the relationship is linear helped us discover
a formula for the interior pressure needed to pop a balloon. This
is because we then knew that the formula would have to be a straight
line equation. Another conclusion we made from our results that
helped us to discover this formula, was that the growth in the
required bursting interior pressure increased as exterior pressure
increased. Therefore, we knew that the slope in our equation would
be positive. To find the formula, all we had to do next was plug
in our x and y coordinates into y=mx=b. Then we plugged in different
positive slopes and yintercepts into the equation, until we found
the right combination that satisfied all of the coordinates in
our results.
Boyle's Law is an extremely dependable law. However, it does not
factor in temperature. Temperature infact, changes the air density
of an object underwater. In warm waters such as in Hawaii, lungs
have a greater volume than a lung in cold water(assuming the depth
in the water is the same for both lungs). This is because air
molecules spread out more and move more freely as they become
more heated. The spreading of molecules in turn, expands the lung
itself. When molecules are cooled on the other hand, they condense
and move very little. Although the above does not mean that warm
waters are more dangerous to scuba dive in, because the regulator
adjusts to how much air is needed to sufficiently fill the lung.
Therefore as one can see, in warmer waters the regulator distributes
less air to the lungs. In colder waters however, the the regulator
has to distribute more air to the lungs to make up for the volume
lost, due to the are extreme fluctuations in the temperature in
the water. This is because the regulator will not be able to adjust
to the amount of air needed to satisfy the lungs, as one ascends
to the surface. Therefore, a diver must ascend with utmost slowness
and deliberacy inorder to give the regulator enough time to adjust
to the circumstance.