Gas Laws Equations

Charles' law describes the relationship between which two quantities?

• pressure and volume
• moles and pressure
• volume and temperature
• temperature and moles

The pressure of a sample of dry air is held constant 2.25 atm while the temperature is decreased from 100. C to 7.0 C. The original volume of the sample is 43 L. Which of the following is closest to the final volume of the sample?

• 3.0 L
• 32 L
• 57 L
• 610 L

The volume of gas in a balloon is 1.90 L at  21.0 C. The balloon is heated, causing it to expand to a volume of 5.70 L. What is the new temperature of the gas inside the balloon?

• 7.00 C
• 63.0 C
• 120. C
• 609. C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-2

A 3.00-liter sample of gas is at 288 K and 1.00 atm. If the pressure of the gas is increased to 2.00 atm and its volume is decreased to 1.50 liters, what will be the Kelvin temperature of the sample?

• 144 K
• 432 K
• 576 K
• 288 K

The temperature of a 2.0-liter sample of helium gas at STP is increased to 27C, and the pressure is decreased to 80 kPa. What is the new volume of the helium sample?

• 4.0 L
• 1.4 L
• 2.0 L
• 2.8 L

The pressure on a 200-milliliter sample of CO₂(g) at constant temperature is increased from 60 kPa to 120 kPa. What is the new volume of the gas?

• 100 mL
• 400 mL
• 300 mL
• 600 mL

A gas has a volume of 1400 milliliters at a temperature of 20 K and a pressure of 1.0 atm. What will be the new volume when the temperature is changed to 40 K and the pressure is changed to 0.50 atm?

• 5600 mL
• 1400 mL
• 750 mL
• 350 mL

Which is the pressure of the gas after it is compressed and cooled?

• 4P/3
• 6P/4
• 9P/4
• 12P/3

A gas has a pressure of 120 kPa, a temperature of 400 K, and a volume of 50.0 milliliters. What volume will the gas have at a pressure of 60 kPa and a temperature of 200 K?

• 50.0 mL
• 100 mL
• 12.5 mL
• 200 mL

The volume of a sample of a gas at 273 C is 200 liters. If the volume is decreased to 100 liters at constant pressure, what will be the new temperature of the gas?

• 0 K
• 546 K
• 273 K
• 100 K