Ideal gas Law and Dalton's Law of Partial Pressures

Dalton's Law states...

• that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
• that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
• how gases tend to expand when heated
• that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.

Which equation represents Dalton's Law?

• e=mc2
• PV=nRT
• P1/T1=P2/T2
• Ptotal=P1, P2, P3...

Three gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?

• 483torr
• 270torr
• 1235torr

A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?

• 234 mmHg
• 1.37 mmHg
• 2.64 mmHg
• 1, 494 mmHg

What does R stand for

• Ideal gas constant

• Real gas constant

• Temperature constant

• Ideal gas law

If the pressure exerted by a gas at 25 degrees C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?

• .002766 mole
• .0069 mol
• 2.766 mol
• 9.887 mol

In order to solve gas law calculations, temperature must be measured in:

• Fahrenheit
• Celsius
• Kelvin
• It doesn't matter 

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.

• 7.18 L 
• 7.81 L
• 4.63 L
• 4.36 L

Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 

• 0 K 
• 107 K 
• 207 K 
• 307 K 

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

• 3670 atm
• 0.245 atm
• 4.08 atm
• 605 atm