Bell work
January 31st, 2014
 You will have to do stoichiometry again
towards the end of this unit 
 So, given the following equation,
 C3H8 + O2  CO2 + H2O if you start with 10
grams of tricarbon octahydride, how many
grams of water will you end up with?
Agenda
Pressure Conversion Factors
Review of the characteristics of gases
Objective:
You will be able to convert between
different units of pressure on your own.
Pressure Videos
Basketball:
http://www.youtube.com/watch?v=t-Iz414g-ro
Egg:
http://www.youtube.com/watch?v=28TIyWdfxx
c&list=PLCA9B7D3D7031D919
Pressure
Pressure = Force
Area
For example:
1 pascal (Pa) = 1 N/m2
Barometer
Write down the following conversion
factors:
1 atm = 760 torr
1 atm = 101.3 kPa
1 atm = 760 mmHg
1 atm = 14.7 psi
1 kPa = 7.50 mmHg
As a class…
Convert:
1)
727 mmHg into kPa
727mmHg x _1 kPa____
7.50mmHg
= 96.9 kPa
2)
52.5 kPa into atm
3)
0.729 atm into mmHg
Solutions…
Convert:
1) 727mmHg x _1 kPa____ = 96.9 kPa
7.50mmHg
2) 52.5 kPa x _1 atm___
= 0.52 atm
101.3 kPa
3) 0.729 atm x _760 mmHg = 554.0 mmHg
1 atm
On your own…
Convert:
4) 522 torr into kPa
5) 800.0 mmHg into atm
6) 495 kPa into mmHg
Solutions…
Convert:
4. 522 torr x _1 atm_ x 101.3 kPa = 69.58 kPa
760 torr
1 atm
5. 800.0 mmHg x _1 atm___ = 1.05 atm
760 mmHg
6. 495 kPa x _7.50 mmHg_ = 3712.5 mmHg
1 kPa
Practice
If a paint ball CO2 tank
is at a pressure of
2000psi and you know
that 1psi equals
51.7mmHg, how many
atm of pressure are in
the tank?
Solution
Known quantity: 2000 psi
Conversion factors: 51.7 mmHg/1 psi
1 atm/760 mmHg
Elements that exist as gases at
250C and 1 atm
Physical Characteristics of Gases
Gases assume the volume and shape of
their containers.
Gases are the most compressible state of
matter.
Gases will mix evenly and completely when
confined to the same container.
Gases have much lower densities than
liquids and solids.
Standard Temperature and
Pressure
Standard temperature and pressure, (STP),
refers to conditions in the atmosphere at sea
level.
Temperature = 0°C or 273K
Pressure = 1atm
This is essentially the freezing point of pure
water at sea level, in air, at standard pressure
Kelvin
When doing gas law problems, all
temperatures must be in Kelvin, not
Celsius!
To convert from Celsius to Kelvin, just add
273.
So, -10°C would be:
-10°C + 273= 263K
Pressure Conversion HW…
Convert:
1.
2.
3.
4.
5.
6.
258 mmHg into kPa
30.5 kPa into atm
.259 atm into mmHg
752 torr into kPa
526 mmHg into atm
125 kPa into mmHg
Bell Work
Feb. 2nd, 2014
Remember density? D = g/ml
What is the density of a 5.6 gram substance
that takes up 9.8 mL of space.
How about volume of a cylinder?
Pi*r2h What would be the volume of a
sausage link if its diameter was 4 cm and it
is 10.2 cm height?
As a class…
What is the mass in grams of a textbook
that is 10 inches long, 8 inches wide, and
3 inches thick, if it has a density of 0.382
g/cm3?
Remember…
Density=mass/volume
Volume of a cylinder=pi*r2h
1. Solve for T2:
Practice
P1V1 = P2V2
T1
T2
2. What would be the volume of a 50 gram sphere of
platinum (density of platinum = 21.50 g\cm3)
3. What would be the mass of 15.2 cm3 of water? d=1 g/cm3
4. The density of the core of the sun is = 150 g\cm3 how
many cubic centimeters would 10 g be?
5. PV = nRT; solve for n!
6. PV = nRT; P=3 atm; V= 1L; T= 273 K; R= .0821atm.L/
mol.K
Practice
1. What would be the volume of a 50 gram sphere of
platinum (density of platinum = 21.50 g\cm3) {ec find the
diameter}
2. What would be the mass of 15.2 cm3 of water?
3. What would be the mass in grams, of a solid steel
flagpole if its circumference was 20cm? (density of steel =
7.3 g\cm3) *height of 5 meters
4. The density of the core of the sun is = 150 g\cm3 how
many cubic centimeters would 10 g be?
5. What would be the mass in grams of the trunk of a tree
that had a circumference of 1 meter and was 3 meters tall
(density of pine = 600 g\m3)
6. Solve for T1:
P1V1 = P2V2
T1
T2
Bell Work
Feb. 3rd, 2014
Not so tough one:
What is the pressure of a tank of He in atm if
the pressure gauge reads 5700mmHg.
Tough one?: What would be the pressure
in atm if the pressure gauge read 4500psi
and 14.7psi is equals 1 atm?
Bell Work
Feb. 3rd, 2014
Not so tough one:
What is the pressure of a tank of He in atm if
the pressure gauge reads 5700mmHg.
Tough one?: What would be the pressure
in atm if the pressure gauge read 4500psi
and 14.7psi is equals 1 atm?
Extra Credit
From test!
Using the following equation…
HCl + NaOH  H2O + NaCl
1) How many grams of NaCl are
produced if you start with 5.5 grams of
NaOH?
2) Calculate the percent yield of NaCl if
you ended up with 6.5 grams in lab.
Agenda
Boyle’s Law Practice Problems
Objective:
You will know how to carry out basic
Boyle’s Gas Law Calculations and
visually see the out come on volume
when varying pressure.
Videos
http://www.youtube.com/watch?v=q6oyxnkZC0
http://www.youtube.com/watch?v=3yvSQu
TP4T4
10 miles
4 miles
Sea level
0.2 atm
0.5 atm
1 atm
Closed
Open
As P (h) increases
V decreases
Boyle’s Law
Boyle’s Law
P a 1/V
P x V = constant
Constant temp. Const.
amount of gas
P1 x V1 = P2 x V2
What is Boyles Law…
P1V1= P2V2
So pressure is inversely proportional to
volume:
As Pressure goes up… volume goes___
As pressure goes down… volume goes____
Examples of Boyle Law at
work
A syringe being used
to draw blood
Popping a balloon
Popping ears during
elevation change
Solve for …
 V2
 P1
 P1V1= P2V2
 P1V1= P2V2
Try this…
A sample of chlorine gas occupies a volume
of 946mL at a pressure of 726mmHg. What
is the pressure of the gas (in mmHg) if the
volume is reduced at constant temperature
to 154 mL?
A sample of chlorine gas occupies a volume of
946mL at a pressure of 726mmHg. What is the
pressure of the gas (in mmHg) if the volume is
reduced at constant temperature to 154 mL?
P1 x V1 = P2 x V2
P1 = 726 mmHg P2 = ?
V1 = 946 mL
V2 = 154 mL
P2 = P1 x V1 = 726 mmHg x 946 mL
V2
154 mL
= 4460 mmHg
From the data in the following table
calculate the missing quantity (assuming
constant temperature).
a) V1 = 22.4 L; P1= 1 atm; P2 =? atm; V2 = 2.8L
b) V1 = 60mL; P1 =? kPa; P2 = 101.3kPa; V2= 16 mL
c) V1 = ? L ; P1 = 40 kPa; P2 = 100 kPa; V2 = 1.0 L
d) V1 = 2.50 L; P1 = 7.5 atm; P2 = ?atm; V2 = 0.100L
Practice makes perfect 
A sample of hydrogen at 1.50 atm had its
pressure decreased to 0.50 atm producing
a new volume of 750 mL. What was the
sample’s original volume?
250ml
Boyle’s ppt. HW
1) If the initial volume is 3.7 L and the initial
pressure is 180.0 KPa, what is the final volume
if the final pressure is 160 KPa?
2) If volume doubles, what happens to pressure?
3) A pressure of 950.0 Kpa is required to initially
inflate a balloon 300.0 mL. What is the final
pressure when the balloon has reached its
capacity of 1.5 L?
Bellwork 2-4-14
 1) What happens to volume as pressure
increases?
 2) Convert 2.5 atm to kpa.
 3) Now convert that number to mmHg.
 4) What does STP stand for??
 Check your grades—mid quarter is Friday!
 Test back to look at—not 5th!
BELL WORK
2-5-2014
A sample of mustard gas is in a sealed vessel
that can change volume based on internal gas
pressure. If the sample of gas started at a
volume of 500mL and an unknown pressure
and then the pressure changed to 540mmHg
and a new volume of 0.75L was established,
what was the original pressure of the vessel?
(write out all the parts first…)
Bell Work
6-Feb-2014
1) Fluorine gas exerts a pressure of 900
torr. When the pressure is changed to
1.50 atm, its volume is 250 mL. What
was the original volume?
2) What is 50 degrees C in Kelvin?
3) 78 kpa is equal to how many torr?
Boyle’s Law Lab
Please do not damage the plunger/ syringe
Practice makes perfect 
1.00L of a gas at standard temperature
and pressure is compressed to 473 mL.
What is the new pressure of the gas?
2.11atm
In a thermonuclear device, the pressure of
0.050L of gas within the bomb casing
reaches 4.0 x 106 atm. When the bomb
casing is destroyed by the explosion,
the gas is released into the atmosphere
where it reaches a pressure of 1.00 atm.
What is the volume of the gas after the
explosion?
2.0x105L
Agenda
Boyles Law Practice Problems
Finish Boyle’s law lab
Objective
You will know how to recognize a Pressure
volume problem and understand the
concept of Boyle’s law
Bell Work
7-Feb-2014
1) Neon gas exerts a pressure of 2.3 atm.
When the pressure is changed to 1.50
atm, its volume is 125 mL. What was
the original volume in liters?
2) How do you go from Kelvin to Celsius?
3) One more time, what are the values at
STP?
4) Solve Boyle’s Law for P2.
Agenda
Volume vs. Temp.
Charles law
Objective:
You will understand the relationship
between volume and temperature
and how it relates to gas molecules.
By the end of the period you will be
able to compute basic volume
temperature calculations.
Recall…
With your partner convert 23,015 Kpa to
atm.
According to Boyle’s Law what happens to
Pressure as volume increases?
As T increases…
V increases
Variation of gas volume with temp.
at constant pressure.
Charles’ &
Gay-Lussac’s
Law
VaT
V = constant x T
V1 = V2
T1 T2
All temperature must be converted to
Kelvin
To convert 0C  K
T (K) = t (0C) + 273
To convert K 0C
T (0C) = t (K) - 273
Why is the Kelvin scale used
exclusively in gas law calculations?
Because there are no negative
temperatures
Try this…
A sample of carbon monoxide gas
occupies 3.20 L at 125 0C. At what
temperature will the gas occupy a volume
of 1.54 L if the pressure remains constant?
A sample of carbon monoxide gas occupies 3.20 L at
125 0C. At what temperature will the gas occupy a
volume of 1.54 L if the pressure remains constant?
V1/T1 = V2/T2
V1 = 3.20 L
V2 = 1.54 L
T2 = ?
T1 = 398 K
V2 x T1
T2 = V
1
=
1.54 L x 398 K
3.20 L
= 192 K
Practice makes perfect 
A sample of nitrogen occupies a volume of
250mL at 25 C. What volume will it occupy
at 95 C?
308.7ml
Helium occupies a volume of 3.80L at -45 C.
What volume will it occupy at 45 C?
5.3L
A 175 mL sample of neon had its pressure
changed from 75.0 kPa to 150 kPa. What is
its new volume (it’s not Charles Law)?
87.5ml
Bell Work 2-10-14
When the boom can, a volume of 500ml,
was filled with gas the temperature was
25°C. During the back draft the
temperature reached 257°C, what
volume did the gas expand to?
**P. slips
Practice makes perfect 
A sample of Ne has a volume of 1.83L at
23.5oC. At what temperature would the gas
occupy 5.00 L? Assume pressure is
constant.
810K
A sample of Ar is collected in a 5.00 x 102ml
bottle at a temp. of 12.0oC. Assuming the
pressure remains the same, what volume
would the gas occupy at 2.0 oC?
482ml
BELL WORK 2-11-14b
1. A sample of gas at a volume of
840mL is in a test tube covered by a
centimeter of mercury. If the test
tube is put in a water bath at a
temperature of 55°C and a new
volume of 1.1L is measured, what was
the original temperature (K)?
2. What are Standard Temp. & Pressure
**P. slips
Charles Law and Water
100 – (Actual/ Theoretical x100) = % error
Charles video clips
http://www.youtube.com/watch?v=j2k40Hw
3GI0
http://www.youtube.com/watch?v=0aqH1Jg
mZ_4
Recall
Synthetic diamonds can be manufactured at
pressures of 6.00 x 104atm. If we took 2.00 L
of gas at 1.00atm and compressed it to a
pressure of 6.00 x 104atm, what would the
volume of that gas be in mL?
The highest pressure ever produced in a
laboratory setting was about 2.0 x 106atm. If
we have a 1.0 x 10-5 L sample of a gas at that
pressure, then release the pressure until it is
equal to 275mmHg, what would the new
volume of that gas be?
Answer w/ your partner
Consider the following changes imposed upon a
sample of gas, assuming the variables not
mentioned remain constant:
a. What happens to the pressure if the
temperature in K is doubled?
b. What happens to the volume if the pressure
is tripled?
c. What happens to the volume if the
temperature decreases from 300K to 200K?
d. What happens to the temperature if one-half
of the gas is removed?
Kinetic Molecular Theory
Video
http://www.youtube.com/watch?v=o2viSF0
PjlY
Agenda
Kinetic molecular theory (short)
Combine Gas Law
Objective:
You will SEE how volume, pressure
and temperature are related.
Kinetic Molecular Theory of Gases
1. Gas molecules have far greater
distances between them than their
own dimensions. They possess mass
but have negligible volume.
2. Gas molecules are in constant
random motion. No Energy is lost
during collisions.
Kinetic Molecular Theory of Gases
3. Gases
exert neither attractive nor
repulsive forces on one another.
4.The average kinetic energy of the
molecules is proportional to the
temperature of the gas in Kelvin.
Any two gases at the same
temperature will have the same
average kinetic energy.
Bell Work 2-12-14
1. Solve for x: (4x)17 + 3 = 29
2. Solve Charles’s Law for V1.
3. A sample of neon gas at 50C and a
volume of 2.50 Liters is cooled to 25C.
What is the new volume in mL?
***Math Moves U!
Quick Review
Hydrogen gas was cooled from 150C to
50C. Its new volume is 75.0 mL. What was
its original volume?
Chlorine gas occupies a volume of 25.0 mL at
300 K. What volume will it occupy at 600 K?
COMBINED GAS LAW
Boyles law: P1 x V1 = P2 x V2
Charles law: V1/T1 = V2/T2
P1V1 =P2V2
T1
T2
COMBINED GAS LAW
Solve for V1
P1V1 =P2V2
T1
T2
COMBINED GAS LAW
Solve for T1
P1V1 =P2V2
T1
T2
COMBINED GAS LAW
A balloon is filled with hydrogen gas
to a volume of 0.5L , and a pressure
of 2.0atm at a temperature of 25°C. If
the balloon is then left out in the sun
at a temperature of 35°C and reaches
a new volume of 2.0L, what is the new
pressure?
A balloon is filled with hydrogen gas to a volume of 0.5L ,
and a pressure of 2.0atm at a temperature of 25°C. If the
balloon is then left out in the sun at a temperature of 35°C
and reaches a new volume of 2.0L, what is the new
pressure?
P1V1/T1 = P2V2/T2
V1 = 0.5L
P1 = 2.0atm
T1 = 298K
P1 V1T2
P2 = T V
1 2
V2 = 2.0L
P2 = ?
T2 = 308K
2.0atm x0.5L x 308K
=
298K x2.0L
= 0.52atm
Practice
A 350 cm3 sample of helium gas is
collected at 25.0 oC and 119.3
kPa. What volume would this gas
occupy at STP?
Practice
A weather balloon is filled with helium to a
volume of 31.5 L at 20oC and 1.3 atm. In the
stratosphere the temperature and pressure
are -23oC and 3.00 x 10-3atm respectively.
What will be the volume (in L) in the
stratosphere?
BELL WORK
2-14-14
A certain gas is in an elastic vessel at a
pressure of 820 torr, a volume of 0.75L and a
temperature of 27ºC. If the volume of the
vessel is doubled and the pressure becomes
101.325kPa, what is the new Temp (K)
A balloon has a volume of 1.0 L at 21.0C and
750 mmHg. What is the balloon’s volume at
STP?
BELL WORK
2-17-14
A gas is in an elastic vessel at a pressure of
670mmHg, a volume of 0.5L and a
temperature of 30ºC. If the volume of the
vessel increases by 200 mL and the pressure
decreases by 45 mmHg, what is the new
temperature in Celsius?
BELL WORK
2-26-13
1. How many moles is 123 g of H2SO4?
2. If the original temperature is 25C and volume
stays constant, but pressure increases from
760 torr to 775 torr, what is the new
temperature?
BELL WORK
2-27-13
1. How many grams is 3 moles of HNO3?
2. If the original temperature is 22C and
pressure stays constant, but volume
decreases from 10 L to 8.3 L, what is the new
temperature?
Baby Goats!
http://www.youtube.com/watch?v=5IuRzJRrRpQ
BELL WORK
2-28-13
1. Balance the following equation:
Fe + Cl2  FeCl3
2. How many moles of FeCl3 will there be if you
start with 3 moles of Cl2?
3. How many grams of FeCl3 would that be?
Agenda:
Ideal Gas law
Objective:
You will be able to solve problems using
the Ideal Gas Law.
Review
1. If the volume of a container starts out as 3 L with a pressure of
1 atm, what is the new pressure if the volume is compressed
to 2.7 L?
2. If initial pressure is 0.9 atm with a volume of 8 L at a
temperature of 25C, what is the new volume if the temperature
increases to 27C and pressure increases to 1.1 atm?
3. If the volume starts at 7 L and temperature is 28C, what is the
new volume if the temperature increases to 31C?
Ideal Gas Law
http://www.youtube.com/watch?v=Mytvt0wlZK8
Ideal Gas Equation
Boyle’s law: V a 1 (at const. n and T)
Charles’ law: V a T (at const. n and P)
Avogadro’s law: V a n (at const. P and T)
PV = nRT
R is the gas
constant
Must have these units…
n = moles
V = liters
T = Kelvin
P = atm
R = .0821 L(atm)/mol(K)
Why? Look at the units for R
At STP, 1 mol of an ideal gas
occupies 22.4 L. Experimentally
proven to give us the value of R.
PV = nRT
R = PV
nT
=
(1 atm)(22.4L)
(1mol)(273 K)
R = 0.082057 L • atm / (mol • K)
What is the volume (in liters) occupied by
1.37moles of HCl at STP?
T = 0 0C = 273 K
PV = nRT
P = 1 atm
nRT
V=
n = 1.37 moles
P
V=
1.37molx
L•atm
0.0821mol•K
1 atm
V = 30.7 L
x 273 K
Practice… Ideal Gas
0.02 moles of oxygen gas are at 0.5 L at
0.25 atm. At what temperature is the gas?
76K
A 0.334L gas cylinder contains 2.12 moles
of helium at 23oC. What is the pressure
(atm) assuming ideal gas behavior?
154 atm
Homework
A 26.9 mole sample of neon is introduced into a
4.5 L cylinder, and the cylinder is heated until
the gas pressure is 375 atm. What is the gas
temperature (in K) at this point?
The pressure in a 2.0 L container is 1.5 x 10-4 torr
at 1115K. How many moles are in the container?
Turn-In:
Boyle’s Law Lab (Textbooks Lab)
Can Crushn’ Lab
Ideal Gas Law Lab (Lighter Lab)
Lab Turn In
Gas Law Lab
Can Crushn’ Lab
R constant Lab (Lighter Lab)
Bell Work 3-1-13
1. A 500 mL metal cylinder holding 8
grams of chlroine gas is known to
rupture at a pressure of 7.6 x 103 torr.
At what temperature, in °C, will the
container fail?
Bell Work
A 500 mL metal cylinder holding 0.100 moles of helium gas is known to
rupture at a pressure of 10 atmospheres. At what temperature, in °C,
will the container fail? (when will it busrt – volume be over 500ml)
PV = nRT
T=?
V = 0.500L
n = 0.100 mol
P = 10atm
T = PV/nR
T = ___(10atm)(0.500L)__________
(0.100mol)(0.0821 L∙atm/ mol∙K)
R = 0.0821 L∙atm
mol∙K
T(ºC) = 609K – 273
= 336
ºC
Algebra Practice
Due by End of Class
Solve for x in the following problems (show all
work):
1) 3x2 – 14 = 21
2) 2x + 11x + 17 = 24
3) 7x2 + 70y = 140
4) 2(4x2 – 16) + 32 = 44
5) 3(6x2 – 18) + 6x2 – 15 = 45
Turn in to Ms. Barrow and do Ideal Gas Law
Worksheet (1-19 odds) when done.
Bell Work 3-4-13
1. How many moles is 15 g of oxygen gas?
2. The Goodyear blimp has 5.12 x 106 liters
of helium at 25oC and 1.00 atm. How many
moles of helium are in the blimp?
Sodium and Chlorine Video
http://www.youtube.com/watch?v=Mx5JJWI
2aaw
Agenda:
Gas Laws Practice Problems
Gas laws using stoichiometry
Objective:
You will continue to UNDERSTAND how to
use the ideal gas law.
Gas Law Review
What pressure will be exerted by 0.450
moles of a gas at 25oC if it is
contained in a vessel whose volume is
650 cm3?
What volume will 12.0 grams of neon
gas occupy at 25oC and a pressure of
0.520 atm?
STOICHIOMETRY: RECAP
Balance the equation first!
NH3 + O2  NO + H2O
How many grams of H2O do I have if
I started with 4 grams of O2?
More Review
According the equation below (balance first)–
_H2SO4(aq)+_NaOH(aq)_H2O(g)+_Na2SO4(aq)
What would the moles of water be if 5.0 grams
of H2SO4 was reacted with NaOH?
What would the volume of gas be in the same
reaction at 300K and 2.5atm?
STOICHIOMETRY: RECAP
4NH3 + 5O2  4NO + 6H2O
How many grams of H2O do I have if I
reacted 4 grams of O2 w/ excess NH3?
Gas Stoichiometry
What is the volume of CO2 produced
at 37 ºC and 1.00 atm when 5.60 g of
glucose are used up in the rxn:
C6H12O6(s)+6O2(g) 6CO2(g)+6H2O(l)
Practice
What volume of nitrogen can be produced by the
decomposition of 50.0 g of NH4NO2 at 25C
and 1.20 atm?
(HINT: You must write a balanced equation.
NH4NO2  N2 + H2O )
More Stoichiometry …
4NH3 + 5O2  4NO + 6H2O
Using the above equation tell me how many
grams of NO do I have if I reacted 15 grams
of O2 w/ excess NH3?
Check your grade!
BELL WORK 3-5-13
How many moles of O2 are in 20L
of oxygen at 2.1 atm and 0°C
What mass of Mg will burn in the below
reaction?
Hint: write the balanced equation and you have
moles of oxygen so now use a mole bridge to
get there!!
Mg + O2 MgO
Crushin’ Cans Lab
#3 Could you have made the air inside the
can push outward? If so how?
#4 why do you feel the wind when it blows,
and what do you think causes it?
More Practice
Many gases are available for use in
the laboratory in compressed gas
cylinders, in which they are
stored at high pressures. Let's
calculate the mass of O2 that can
be stored at 21ºC and 170 atm in a
cylinder with a volume of 60.0 L.
BELL WORK
On a new Bell Work Sheet labeled
Bell Work 2-28-11
In three sentences or more explain
how you could use your knowledge
of stoichiometry to find the volume
of H2 gas produce at STP from 20.0g
of Mg given the following rxn.
Mg(s) + HCl(aq)  MgCl2(aq) + H2(g)
STOICHIOMETRY: RECAP
Grams A  (÷ mol mass)
moles A (mol B/ mol A)
moles B  (x mol mass)
Grams of B
BELL WORK 2-21-12
What mass (think “moles
first”) of carbon dioxide
will occupy 12.5 L at 10C
and 1.75 atm?
Standard Molar Volume:
1 mol = 22.4 L
At STP an ideal gas occupies a
volume of 22.4 L/ mol.
So, what volume would 1.25 mole
of H2 gas occupy at STP
1.25mol H2 x 22.4L/mol = 28 L
Review Practice
3-7-13
1. How many grams is 2.1 mol of HCl?
2. How many moles is 3.1 grams of CH4?
3. Starting from an unbalanced equation,
write down the steps to go from grams
of A to grams of B .
Review Practice
If I have 5.6 liters of gas in a piston at a
pressure of 1.5 atm and compress the gas
until its volume is 4.8 L, what will the new
pressure inside the piston be?
I have added 15 L of air to a balloon at sea
level (1.0 atm). If I take the balloon with
me to Denver, where the air pressure is
0.85 atm, what will the new volume of the
balloon be?
Turn in the following:
 Determining the value of “R” Lab
 Ideal and Combined (white sheet) 1-20.
 Chapter 18 review pg. 43 a & b, 44-47
and page 481 1-5.
 Gas Stoichiometry (white sheet) 1-10.
 Chapter 19 review page 494-95 36a,
37a, 38, 40, 46, 47, 52.
Can
Crushn’!