Gas Laws & Stoichiometry CFA

A sample of gas is contained in a closed container under 2 atm of pressure. According to kinetic molecular theory, what causes this pressure?

• The gas molecules are colliding with the walls of the container, exerting a force on the container.

• The gas molecules are colliding with each other, exerting a force on each other.

• The gas particles are chemically reacting with each other releasing energy.

• The gas molecules are attaching to the walls of the container, pulling it inward.

Given the combustion reaction C₃H₈ + 5O₂ ​​→ 3CO₂ + 4H₂O, how many liters of carbon dioxide can be produced from 1.00 liter of O₂ at standard temperature and pressure?

• 0.600 L

• 0.825 L

• 1.21 L

• 1.67 L

Which of the following is not one of the postulates of the Kinetic Molecular Theory for ideal gases?

• The collisions between particles are elastic.

• The particles attract and then repel each other

• The particle size is very small compared to the space between the particles.

• The particles are in constant random motion.

Which graph shows the pressure-temperature relationship expected for an ideal gas?

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Two gas molecules collide together in a box container. Which reaction accurately portrays the kinetic molecular theory?

• The two molecules will stay together because they are attracted to each other.

• The two molecules will move off in opposite directions because they are repelled by each other.

• The two molecules will move in different directions without being attracted or repelled by the other.

• The two molecules will either be attracted or repelled by each other depending on the charge of each gas molecule.

Ammonia is produced from the reaction of nitrogen and hydrogen gases. What volume of hydrogen at STP is required to produce 25 g of ammonia?

N₂(g) + 3H₂(g) → 2NH₃(g)

• 33 L

• 1.1 L

• 49 L

• 25 L

Tags

NGSS.HS-PS1-7