Dalton's Law

What units will be found in the variables of a Dalton's law problem?

• kilopascals (kPa)

• liters (L)

• Kelvins (K)

• moles (mol)

Dalton's law equation is used to find what?

• the density of a pure gas

• the total pressure of a pure gas

• the total pressure of a gas mixture

• the volume of a gas mixture

What is the total pressure of the heliox gas in the diagram?

• 300 kPa

• 100 kPa

• 400 kPa

• 500 kPa

In a mixture of gases, each gas contributes to the total pressure. The individual contribution of each gas is known as the _________________.

• partial volume

• partial pressure

• molar mass

• mole ratio

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.

Dalton's Law of Partial Pressures is particularly useful in calculating the pressure of gases in:

• Chemical reactions

• Gas mixtures

• Solids

• Liquids

Which of the following is a direct application of Dalton's Law of partial pressures?

• Predicting the boiling point of a liquid mixture.

• Calculating the pressure inside a balloon filled with helium and oxygen.

• Determining the solubility of a gas in water at a given temperature.

• Measuring the speed of sound in air.

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

If a gas mixture contains 2 moles of hydrogen and 3 moles of helium, what is the partial pressure of helium if the total pressure is 5 atm?

• 2 atm

• 3 atm

• 1 atm

• 4 atm

What is the definition of partial pressure in a gas mixture?

• The pressure that each gas would exert if it occupied the entire volume alone at the same temperature.

• The total pressure exerted by the sum of all gases in a mixture.

• The pressure exerted by the gas molecules when they collide with the walls of a container.

• The decrease in pressure when a gas is mixed with another gas.