Dalton's Law of Partial Pressure

A container holds four times as many moles of CO₂ as O₂. If the total pressure in the container is 20 atm, what is the pressure exerted by carbon dioxide?

Given that a vessel contains 0.672 mol O₂, 0.128 mol CO₂, and 0.200 mol N₂. If the total pressure of the vessel is 100 atm, what are the partial pressure of O₂, CO₂, and N₂ respectively. _{(That means, in that order).}

• 67.2 atm, 12.8 atm, 20.0 atm

• 67.2 atm, 20.0 atm, 12.8 atm

• 20.0 atm, 67.2 atm, 12.8 atm

• 12.8 atm, 20.0 atm, 67.2 atm

The pressure of a mixture of nitrogen, carbon dioxide, and oxygen is 300 kPa.
What is the partial pressure of oxygen is the partial pressures of the nitrogen and carbon dioxide are 200 kPa and 48 kPa, respectively. _{(That means, in that order)}

• 52 kPa

• 218 kPa

• 26 kPa

• 148 kPa

In a mixture of gases, each gas exerts pressure independently of the others.

• TRUE

• FALSE

Which statement best describes the relationship between gas mixtures and partial pressures according to Dalton's Law?

• The partial pressure of each gas in a mixture is independent of the presence of other gases.

• The partial pressure of a gas decreases as more gases are added to the mixture.

• The partial pressure of a gas is directly proportional to its molecular weight.

• The partial pressure of each gas is determined by the total volume of the gas mixture.

What does Dalton's Law of Partial Pressures state?

• The total pressure of a gas mixture is equal to the sum of the pressures each gas would exert if it occupied the whole volume alone.

• The pressure of a gas mixture is less than the sum of the pressures of each individual gas.

• The pressure of a gas mixture is greater than the sum of the pressures of each individual gas.

• The pressure of each gas in a mixture is the same.

Dalton's Law of Partial Pressures states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of individual gases. If a container holds oxygen at 2 atm and nitrogen at 3 atm, what is the total pressure inside the container?

• 5 atm

• 1 atm

• 6 atm

• 4 atm

How is the partial pressure of a gas in a mixture calculated using Dalton's Law?

• By multiplying the total pressure by the volume fraction of the gas.

• By dividing the volume of the gas by the total volume of the mixture.

• By multiplying the mole fraction of the gas by the total pressure of the mixture.

• By adding the pressure of all individual gases in the mixture.

In a mixture of gases, the total pressure is 760 mmHg. If the partial pressure of oxygen is 200 mmHg and nitrogen is 500 mmHg, what is the partial pressure of the remaining gas?

• 60 mmHg

• 100 mmHg

• 160 mmHg

• 260 mmHg

If the partial pressures of hydrogen and oxygen in a container are 300 mmHg and 700 mmHg respectively, what is the total pressure in the container?

• 1000 mmHg

• 400 mmHg

• 300 mmHg

• 700 mmHg