Ideal Gas Laws; Dalton's Partial Pressure

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

A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?

• 2 atm
• 4 atm
• 3 atm
• 9 atm

What is the variable for this number 22.4 L

• P
• T
• n
• V

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

When 0.250 moles of a gas is placed in a container at 25 °C, it exerts a pressure of 700 mm Hg. What is the volume of the container?

• 0.557 Liters

• 6.57 Liters

• 8.74 Liters

• 0.0087 Liters

A 15.50 gram sample of a gas exerts a pressure of 1.40 atmospheres when held in an 8.00 liter at 22 °C. What is the molar mass (grams/mol) of the gas?

• 33.5 g/mol

• 0.0298 g/mol

• 6.57 g/mol

• 62.2 g/mol

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