Partial Pressure Calculations in Gases

The video tutorial covers Dalton's Law, explaining that the total pressure of a gas mixture is the sum of the partial pressures of its components. Through various examples, the tutorial demonstrates how to calculate partial pressures of gases like oxygen and nitrogen, convert units for pressure calculations, and use percentages to determine partial pressures. The tutorial also includes a calculation of total pressure from water vapor pressure, emphasizing the importance of consistent units.

What is the basic principle of Dalton's Law?

• The total pressure is the sum of all partial pressures.

• The total pressure is the difference between the highest and lowest partial pressures.

• The total pressure is the product of all partial pressures.

• The total pressure is the average of all partial pressures.

In Example 1, if the total pressure is 101.3 kPa and the partial pressures of other gases are given, how do you find the partial pressure of oxygen?

• Subtract the partial pressures of other gases from the total pressure.

• Add the partial pressures of other gases to the total pressure.

• Divide the total pressure by the number of gases.

• Multiply the partial pressures of other gases by the total pressure.

What is the partial pressure of oxygen in Example 1?

• 0.040 kPa

• 79.1 kPa

• 2.22 kPa

• 94 kPa

In Example 2, what is the total pressure of the gas mixture containing oxygen, nitrogen, and helium?

• 2.64 ATM

• 4.61 ATM

• 0.97 ATM

• 9.22 ATM

How do you calculate the total pressure in Example 2?

• Divide the total pressure by the number of gases.

• Multiply the partial pressures of oxygen, nitrogen, and helium.

• Subtract the partial pressures of nitrogen and helium from oxygen.

• Add the partial pressures of oxygen, nitrogen, and helium.

In Example 3, why is it necessary to convert units before calculating the partial pressure of CO2?

• To increase the total pressure.

• To decrease the total pressure.

• To ensure all pressures are in the same unit for accurate calculation.

• To make the calculation easier.

What is the partial pressure of CO2 in Example 3?

• 32.9 kPa

• 3.3 kPa

• 23.0 kPa

• 6.6 kPa

In Example 4, if the total pressure is 600 mm of mercury and nitrogen is 80%, what is the partial pressure of oxygen?

• 480 mm of mercury

• 120 mm of mercury

• 600 mm of mercury

• 80 mm of mercury

How can you calculate the partial pressure of oxygen using percentages in Example 4?

• Divide the total pressure by the percentage of nitrogen.

• Add the percentage of nitrogen to the total pressure.

• Subtract the percentage of nitrogen from 100% and multiply by the total pressure.

• Multiply the total pressure by the percentage of nitrogen.

In Example 4, if the partial pressure of water vapor is 138.6 mm of mercury and it is 18% of the total, what is the total pressure?

• 600 mm of mercury

• 18 mm of mercury

• 138.6 mm of mercury

• 770 mm of mercury