Dalton's law of Partial Pressure

Partial pressure of a gas is defined as:

• The pressure that the gas would exert if it occupied the same volume alone at the same temperature.
• The pressure exerted by the gas on the particles within it.
• The pressure exerted by the gas on the container it is in.
• The pressure exerted by the gas on the surrounding environment.

According to the Dalton law of partial pressure:

• The total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.
• The total pressure exerted by a mixture of non-reacting gases is equal to the product of the partial pressures of the individual gases.
• The total pressure exerted by a mixture of non-reacting gases is equal to the difference of the partial pressures of the individual gases.
• The total pressure exerted by a mixture of non-reacting gases is equal to the average of the partial pressures of the individual gases.

The pressure of gas collected over water can be determine using formula:

• P = P_total + P_{water vapor}

• P = P_total x P_{water vapor}

• P = P_total / P_{water vapor}

• P = P_total - P_{water vapor}

SCUBA stands for:

• Self-Contained Underwater Breathing Apparatus
• Self-Contained Underwater Breathing Aid
• Self-Contained Underwater Breathing Accessory
• Self-Compressed Underwater Breathing Apparatus

With the increase in altitudes, the partial pressure of oxygen in air:

• remains constant
• decreases
• increases
• fluctuates

With the increase in depth of sea level, the partial pressure of oxygen in water:

• increases
• remains constant
• fluctuates
• decreases

Tags

NGSS.HS-ESS2-5

At the depth of 99 feet below sea level the pressure of oxygen becomes:

• 4 times the pressure at sea level

• 2 times the pressure at sea level

• 5 times the pressure at sea level

• 3 times the pressure at sea level

Which of the following is NOT a statement of Dalton's law of partial pressures?

• The total pressure of a gas mixture is equal to the sum of the partial pressures of the individual gases in the mixture.

• The partial pressure of a gas in a mixture is the pressure that the gas would exert if it were alone in the container.

• The partial pressure of a gas in a mixture is proportional to its mole fraction in the mixture.

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

A gas mixture contains 40% nitrogen and 60% oxygen by volume. The total pressure of the mixture is 760 mmHg. What is the partial pressure of oxygen in the mixture?

• 456 mmHg

• 304 mmHg

• 228 mmHg

• 152 mmHg

Answer explanation

by volume is written, equal volume of different gas have same moles.

so mole fraction is 0.6

0.6 x 760 = answer

A scuba diver is breathing a mixture of air and helium. The partial pressure of oxygen in the mixture is 160 mmHg. What is the mole fraction of oxygen in the mixture?

• 0.21

• 0.47

• 0.79

• 1.00

Answer explanation

P_A = X_A x P_total

_{mole fraction =} P_A / P_total