Gas Laws Part 2

How do you convert mmhg to ATM?

• Multiply the mmhg pressure value by 760

• No need to convert--they can be used interchangeably.

• Divide the mmhg pressure value by 760.

A weather balloon has a volume of 105L at 0.97 atm when the temperature is 318K. What is the volume at 293K and 1.05 atm?

• 89.4 L

• 0.32 L

• 93.8 L

• 3.13 L

The total pressure in a gas mixture is equal to the sum of the partial pressures of each individual gas.

• Dalton's Law of Partial Pressures
• Boyle's Law
• Combined Gas Law
• Idea Gas Law

In PV = nRT, n stands for

• Neon
• number of moles
• number of gases
• Absolute zero

What are the standard temperature and pressure conditions for gases?

• 0 K and 760 mm Hg
• 273˚C and 1.0 atm
• 273 K and 101.3 kPa
• 0˚C and 760 kPa

A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?

• 0.78 atm

• 1.65 atm

• 1.28 atm

• 0.61 atm

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

At 17 °C, a 0.80 mole sample of a gas exerts a pressure of 1.2 atmospheres. What is the volume of the container?

• 22.9 Liters

• 2355 Liters

• 0.0630 Liters

• 15.9 Liters

At what temperature does 48.5 grams of CO₂ occupy 4.56 liters and have a pressure of 2.5 atm?

• 126 K

• 213 K

• 451 K

• 955 K