Boyle’s Law
1.
2.
3.
4.
5.
6.
7.
8.
A sample of oxygen gas occupies a volume of 250 mL at 740 torr pressure. What volume will it
occupy at 800 torr pressure?
A sample of carbon dioxide occupies a volume of 3.50 L at 125 kPa. What pressure would the
gas exert if the volume was decreased to 2.00 L?
A 2.00 L container of nitrogen had a pressure of 3.20 atm. What volume would be necessary to
decrease the pressure to 1.00 atm?
Ammonia gas occupies a volume of 450 mL at a pressure of 720 mmHg. What volume will it
occupy at standard pressure (760 mmHg)?
A 175 mL sample of neon had its pressure changed from 75.0 kPa to 150 kPa. What is the
new volume?
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?
Chlorine gas occupies a volume of 1.20 liters at 720 torr pressure. What volume will it occupy
at 1 atm?
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?
Charles’ Law
1. A sample of nitrogen occupies a volume of 250 mL at 25°C. What volume will it occupy at 95°C?
2. Oxygen gas is at a temperature of 40°C when it occupies a volume of 2.30 L. To what
temperature should it be raised to occupy a volume of 6.50 L?
3. Hydrogen gas was cooled from 150°C to 50°C. Its new volume is 75.0 mL. What was its
original volume?
4. Chlorine gas occupies a volume of 25.0 mL at 300 K. What volume will it occupy at 600 K?
5. A sample of neon gas at 50°C and volume of 2.50 L is cooled from 25°C. What is the new
volume?
6. Fluorine gas at 300 K occupies a volume of 500 mL. To what temperature should it be lowered
to bring the volume to 300 mL?
7. Helium occupies a volume of 3.80 L at -45°C. What volume will it occupy at 45°C?
8. A sample of argon gas is cooled and its volume went from 380 mL to 250 mL. If its final
temperature was -55°C, what was its original temperature?
Gay-Lussac’s Law
1.
2.
3.
4.
5.
6.
P1 = 450 mmHg
P2 = 600 mmHg
T1= 27°C
T2 = ?
P1 = 1.75 atm
P2 = ?
T1= 77°C
T2 = 154°C
P1 = ?
P2 = 1.00 atm
T1= 10°C
T2 = -123°C
P1 = ?
P2 = 18.9 psi
T1= 48°C
T2 = -20°C
P1 = 14.5 psi
P2 = 56 psi
T1= 34°C
T2 = ?
To what temperature must a sample of nitrogen gas at 27°C and 0.625 atm be heated so that
its pressure becomes doubled at a constant volume?
7. Hydrogen gas is collected at 30°C and 29 inHg and then raised to 58°C at constant volume.
What is the new pressure?
8. If a sample of iodine gas is currently 78°C and 4 atm but was originally collected at 50°C, what
was the original pressure assuming constant volume?
9. If a sample of mercury gas is currently 90°C and 813 mmHg but was originally collected at 750
mmHg, what was the original temperature assuming constant volume?
Combined Gas Law
1. If 1000 mL of a gas are at 40°C and 756 mmHg, what is the pressure of the gas if the volume
is changed to 250 mL and the temperature is changed to 89°C?
2. If a gas is collected at a temperature of 65°C and a pressure of 20 psi and then the
temperature is changed to 90°C and the pressure is changed to 88 inHg, the new volume
becomes 76 mL. What was the original volume?
3. If 675 mL of a gas at 90°C becomes 25 mL of gas at 35°C and 2 atm, what was the original
pressure?
4. If 45 mL of a gas is collected at 565 mmHg and becomes 50 mL of gas at 50°C and 800
mmHg, what was the original temperature?
5. If 18 mL of gas is collected at 30 inHg and becomes 30 mL of gas at 50°C and 800 mmHg,
what was the original temperature?
6. If a gas is collected at a temperature of 12°C and a pressure of 15 psi and then when the
temperature is changed to 15°C and the pressure is changed to 1 atm, the new volume
becomes 38 mL. What was the original volume?
7. If 568 mL of a gas are at 68°C and 4 atm, what is the pressure of the gas if the volume is
changed to 987 mL and the temperature is changed to 80°C?
8. If a gas is collected at a temperature of 46°C and a pressure of 38 inHg and then when the
temperature is changed to 50°C and the pressure is changed to 45 inHg, the new volume
becomes 75 mL. What was the original volume?
9. If 60 mL of gas is collected at 1 atm and becomes 50 mL of gas at 100°C and 6 atm, what was
the original temperature?
10. If 240 mL of gas is collected at 2 atm and becomes 50 mL of gas at 20°C and 4 atm, what was
the original temperature?
Ideal Gas Law
1.
2.
3.
4.
5.
What is the pressure in atm exerted by 2.4 moles of hydrogen gas in a 30 L container at 325 K?
What is the volume of a container holding 6.5 moles of fluorine gas at 775 mmHg and 300 K?
How many moles of oxygen gas are present in a 15 liter container at 30°C and 102 kPa?
What is the temperature of a 12 L container of 45 g of chlorine gas at 745 mmHg?
What is the pressure in atm exerted by 260 g of Br2 at 330K in a 1.5 L container?
Dalton’s Law of Partial Pressure
1. Three of the primary components of air are carbon dioxide, nitrogen, and oxygen. In a sample
containing a mixture of these gases at 39.5 inHg, the partial pressure of the carbon dioxide
and nitrogen are given as P(CO2) = 0.285 mmHg and P(N2) = 593.25 mmHg. What is the
partial pressure of the oxygen gas (in mmHg)?
2. If the air pressure today is 1.4 atm and nitrogen gas makes up 78% of the air, what is the
partial pressure of the nitrogen gas (in atm)?
3. If the air pressure today is 16.78 psi and oxygen gas makes up 19% of the air, what is the
partial pressure of the oxygen gas (in psi)?
4. Sulfur dioxide (SO2) is made of sulfur and oxygen. If the total pressure of the gas is 2.4 atm
and the partial pressure of the sulfur is 567 mmHg, what is the partial pressure of the oxygen
(in mmHg)?
5. Ammonia (NH3) is made of nitrogen and hydrogen. If the total pressure of the gas is 35 inHg
and the partial pressure of the hydrogen is 688 mmHg, what is the partial pressure of the
nitrogen (in inHg)?
6. Carbon monoxide (CO) is made of carbon and oxygen. If the total pressure of the gas is 900
torr and the partial pressure of the carbon is 800 mmHg, what is the partial pressure of the
oxygen (in torr)?
7. Sulfate is made of sulfur and oxygen. If the partial pressure of the sulfur is 450 mmHg and the
total pressure o the gas is 500 torr, what is the partial pressure?
8. Boron trioxide (BO3) is made of boron and oxygen. The partial pressure of the oxygen is 24
inHg and the total pressure of the gas is 34 inHg, what is the partial pressure of the boron (in
inHg)?
Graham’s Law
1. A container holds Ar2 (g) and HCl (g). If the container is kept constant at 15 degrees Celsius
and the argon moves at a speed of 34 m/s, what is the speed of HCl?
2. A container hold CO2 (g) and C3H8 (g) If the container is kept constant at 25 degrees Celsius
and the CO2 moves at a speed of 18 m/s, what is the speed of C3H8?
3. What gas moves fastest in each of the following pairs?
a. BF3 and Kr2
b. NH4 and O3
c. BH2 and SO3
d. SiO3 and CF4
4. If KCl (g) and H2O (g) are both kept in a container at 10 degrees Celsius and KCl moves at a
speed of 10 km/hr, what is the speed of H2O?
5. What is the relative rate of diffusion of KI (g) if it is kept in a container at constant temperature
with NaI (g) moving at a speed of 25 km/s?