General
one goes up, the other goes up
direct
P1V1 = P2V2
Boyle's law
A sample of oxygen had an initial volume of 4.0L and was at a standard pressure of 1atm, what would the new volume be if the pressure was increased to 25.00atm?
Boyle's law (P1V1 = P2V2)
0.16 atm
My car tires are filled to 32psi at 20°C, when the first frost happens and the temperature drops to 15°C, what could my tire pressure drop to?
G-L's law (P1 / T1 = P2 / T2)
31.45 psi
If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 L, what is the temperature?
Ideal Gas (PV = nRT)
*R = .0821
204.6K
one goes down, the other goes up
inverse
P1 + P2 + (etc) = Ptotal
Dalton's
4.40 L of a gas is collected at 50.0 °C. What will be its volume upon cooling to 25.0 °C?
Charles's law (V1 / T1 = V2 / T2)
4.06 L
What is the atmospheric pressure if the partial pressures of nitrogen, oxygen, and argon are 604.5 mmHg, 162.8 mmHg, and 0.5 mmHg, respectively?
Dalton's law (add them up!)
767.8 mmHg
2 L of hydrogen gas are stored at a pressure of 100kPa. If the temperature does not change, what will the volume of the gas be when the pressure is decreased to 25 kPa?
Combined gas law
2 L x 100 kPa / 25 kPa = 8L
Pressure increases, volumes ___
decreases
PV= nRT
Ideal Gas law
A 2.50-L volume of hydrogen measured at -100 degrees Celsius is warmed to 100 degrees Celsius. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.
Charles's law (V1 / T1 = V2 / T2)
5.39 L
Container A contains a gas with a pressure of 3.24 mmHg. Container B contains a gas under 2.82 atm of pressure. Container C contains a gas under 1.21 atm of pressure. If all these gases are combined into container D, what is the pressure in container D?
Dalton's law (add them up once all in same units!)
Container A: 3.24 mmHg --> .004 atm
4.0343 atm
If I have 2.4 moles of gas held at a temperature of 97oC and in a container with a volume of 45 L, what is the pressure of the gas?
1.62 atm (164 kPa)
Temperature increases, volume ___
increases
P1V1 / T1 = P2V2 / T2
Combined Gas law
A sample of helium gas in a balloon is compressed from 4.0 L to 2.5 L at constant temperature. If the initial pressure was 3.0 atm at 4.0L, what is the new pressure at 2.5 L?
Boyle's law (P1V1 = P2V2)
4.8 atm
The pressure in an automobile tire is 1.88 atm at 25.0oC. What will be the pressure if the temperature warms up to 37.0oC?
G-L's law (P1 / T1 = P2 / T2)
1.96 atm
A cylinder that contains air at a pressure of 100 kPa has a volume of 0.75 L. The pressure is increased to 300 kPa. If the temperature does not change, what is the new volume of air?
Combined Gas Law
100 kPa x 0.75 L / 300 kPa =0.25 L
Temperature increases, pressure ___
increases
V1 / T1 = V2 /T2
Charles's law
If I have 45L of helium in a balloon at 300K and increase the temperature of the balloon to 350K, what will the new volume of the balloon be?
Charles's law (V1 / T1 = V2 / T2)
52.5 L
At 95ºC, the pressure of a sample of chlorine is 1.15 atm. What will the pressure be at 105ºC, assuming constant volume?
G-L's (P1 / T1 = P2 / T2)
1.18 atm
If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 L and a temperature of 87oC, how many moles of gas do I have?
1.26 mol