Chemistry Reference
In-Depth Information
high, you actually have more gas molecules in the sample than you would if
you collected 2.50 L of the same gas when the temperature was high and the
atmospheric pressure was low. Reporting the volume of the gas alone is never
enough, so the practice is to calculate the volume that your gas sample
would occupy at “standard temperature and pressure.” Standard tempera-
ture and pressure (STP) has been set at 273 K and 101.3 kPa.
Lesson 8-1 Review
1.
A _______________ is an instrument that is used to measure
atmospheric pressure.
2.
________________ is a measure of the force exerted over a given area.
3.
STP stands for standard ___________ and ___________.
Make the following conversions:
4. 2.0 atm = _____ kPa 5. 107.5 kPa = _____ mm of Hg
6. 790 torr = _____ atm 7. 1.04 atm = ______ mm of Hg
8. 33.2 inches of Hg = _____ atm 9. 754 Torr = ______ mm of Hg
10. Which of the following is equivalent to standard temperature?
a) 0
o
C
c) 273
o
C
e) Both A and D are correct
b) 0 K
d) 273 K
Lesson 8-2: Boyle's Law
Did you ever squeeze a balloon and see bulges appear in a different
area of it? Did you ever climb onto an inflatable float or air mattress and
notice that as you sunk into it, it started to get firmer beneath you? If you
did either of these two things, you were unknowingly experimenting with
Boyle's Law. Boyle's Law states that the pressure and volume of a gas at
constant temperature are inversely proportional. This means that if you
change the volume of a gas, without changing the temperature or number
of particles of the gas, you get an inversely proportional change in the gas
sample's pressure. The relationship between the volume and pressure of a
gas will be made clearer by looking at the formula and some examples of
Boyle's Law.
Boyle's Law
P
1
V
1
= P
2
V
2
where P is the pressure and V is the volume
