Gas Laws Practice

A sample of nitrogen gas has a volume of 32.4 L at 20°C. The gas is heated to 220ºC at constant pressure. What is the final volume of nitrogen?

• 2.94 L

• 19.3 L

• 31.4 L

• 54.5 L

Tags

NGSS.HS-PS3-4

A sample of N₂ gas occupies 2.40 L at 20°C. If the gas is in a container that can contract or expand at constant pressure, at what temperature will the N₂ occupy 4.80 L?

• 10°C

• 40°C

• 146°C

• 313°C

1. A gas evolved during the fermentation of sugar was collected. After purification its volume was found to be 25.0 L at 22.5°C and 702 mmHg. How many moles of gas were collected?

• 0.95 mol

• 1.05 mol

• 12.5 mol

• 22.4 mol

Tags

NGSS.HS-PS1-7

The gas pressure in an aerosol can is 3.5 atm at 25°C. If the gas is an ideal gas, what pressure would develop in the can if it were heated to 175°C?

• 3.5 atm

• 4.8 atm

• 5.3 atm

• 7.5 atm

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO₂ and is heated to 400°C, will it burst?

• Yes

• No

Tags

NGSS.HS-PS1-5

When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the

• air molecules hit the walls of the tire less frequently
• rubber in the tires reacts with oxygen in the atmosphere
• air molecules speed up and collide with the tire walls more often
• air molecules diffuse rapidly through the walls of the tire.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS3-2

What is 50 C in Kelvin?

• 223
• 323
• 100
• 50

You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?

• 5 L
• 20 L
• It would stay at 10L
• 1 L

A sample of a gas has a volume of 852 mL at 298 K. What temperature is necessary for the gas to have a volume of 945 mL?

• 57.5⁰C
• 57.5⁰K
• 330.5⁰K
• 330.5⁰C

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).

• 7.18 L 
• 7.81 L
• 4.63 L
• 4.36 L