Gas Laws and Pressure Calculations

This video tutorial for Unit 9 Day 1 homework covers pages 1-3, focusing on gas molecules, kinetic molecular theory, and pressure conversions. It explains how gas molecules occupy space, the principles of kinetic theory, and how to perform pressure conversions using dimensional analysis. The tutorial also covers Dalton's Law, demonstrating how to calculate total and partial pressures in gas mixtures.

What is the primary characteristic of gas molecules that allows them to fill large volumes?

• They are very large in size.

• They are solid at room temperature.

• They are very small and diffuse easily.

• They are heavy and dense.

According to the kinetic molecular theory, how do gases behave at a given temperature?

• All gases have different energies.

• Gases become liquids.

• Gases do not move.

• All gases have the same energy.

What tool is used to measure atmospheric pressure?

• Thermometer

• Anemometer

• Barometer

• Hygrometer

What is the standard pressure in millimeters of mercury (mm Hg)?

• 22.4 mm Hg

• 180 mm Hg

• 760 mm Hg

• 101.3 mm Hg

How do you convert 1.8 atmospheres to millimeters of mercury (mm Hg)?

• Multiply by 760

• Multiply by 101.3

• Divide by 760

• Divide by 101.3

What is the total pressure if you have 1 atm, 2 atm, and 3 atm of different gases?

• 7 atm

• 6 atm

• 5 atm

• 3 atm

In Dalton's Law, what must be true for the pressures to be added directly?

• They must be measured at different temperatures.

• They must be converted to Kelvin.

• They must be in the same units.

• They must be in different units.

If a gas mixture has a total pressure of 0.98 atm, and the partial pressures of CO2 and O2 are 0.12 atm and 0.70 atm respectively, what is the partial pressure of N2?

• 0.20 atm

• 0.18 atm

• 0.16 atm

• 0.22 atm

What is the first step in solving for an unknown partial pressure in a gas mixture?

• Convert all pressures to the same unit.

• Add all given pressures together.

• Subtract the smallest pressure from the largest.

• Multiply all pressures by Avogadro's number.

In a gas mixture, if the total pressure is 111 kPa and the partial pressures of O2 and He are 11.1 kPa and 77.49 kPa respectively, what is the partial pressure of N2?

• 23.41 kPa

• 25.41 kPa

• 22.41 kPa

• 24.41 kPa