The Ideal Gas Law

A 7.50 liter sealed jar at 18 °C contains 0.125 moles of oxygen and 0.125 moles of nitrogen gas. What is the pressure in the container?

• 7.38 atm
• 0.796 atm
• 0.684 atm
• 0.398 atm

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

How many moles of oxygen must be placed in a 3.00 liter container in order to exert a pressure of 2.00 atmospheres at 25 °C?

• 146.8 moles
• 0.245 moles
• 21778 moles
• 4.08 moles

A 4.0 liter container has two gases inside, neon and argon. It is known that at 18 °C, the total pressure of the combined gases is 0.850 atm. If it is known that there are 0.100 moles of neon in the container, how many moles of argon are in the container?

• 0.142 moles
• 6.93 moles
• 0.042 moles
• 4.98 moles

What is the variable for this number 22.4 L

• P
• T
• n
• V

PV=nRT

• Charles Law
• Boyle's Law
• Combined Gas Law
• Ideal Gas Law

Which is a correct unit for R?

• L.atm/mol.k

• L.atm

• mmHg/mol.K

• L.atom/mol

If n and T are held constant, the ideal gas law reduces to 

• Charles' law
• Boyle's law
• Avogadro's principle
• zero

At 250 k and 1.75 atm, a gas has a mass of 15.3 g and occupies 5.60 L. What is the molar mass of the gas?
M=mRT/PV

• 32.04
• 42.15
• 48.91
• 54.28

An unknown gases diffuses .25 times faster than Helium. What is the molar mass of the unknown gas?

• 1 g/mol
• 64 g/mol
• 24 g /mol
• 16 g/mol