ONRAMPS CHEMISTRY FINAL REVIEW PART 1

What assumption does the Kinetic Molecular Theory make about gas particles' volume?

• Gas particles have significant volume.

• Gas particles' volume is directly proportional to pressure.

• Gas particles occupy no volume.

• Gas particles' volume increases with temperature.

What property of a gas is directly proportional to its temperature according to the Kinetic Molecular Theory?

• Pressure

• Kinetic energy

• Density

• Volume

According to Boyle's Law, what happens to the volume of a gas when pressure increases, assuming temperature remains constant?

• Volume increases.

• Volume decreases.

• Volume remains constant.

• Volume doubles.

Which gas law would you use to calculate the final volume of a gas when its pressure changes?

• Avogadro's Law

• Boyle's Law

• Charles' Law

• Gay-Lussac's Law

What is the primary focus of the Ideal Gas Law?

• Understanding the relationship between gas volume, pressure, temperature, and moles.

• Calculating the volume of a gas at standard temperature and pressure.

• Relating pressure and temperature of a gas.

• Determining the molecular weight of a gas.

In an ICE table, what does the 'C' stand for?

• Change

• Constant

• Completed

• Calculated

How does the rate of effusion for helium compare to that of carbon dioxide?

• Helium and carbon dioxide effuse at the same rate.

• The rate of effusion is not related to molecular mass.

• Helium effuses slower than carbon dioxide.

• Helium effuses faster than carbon dioxide.

What does the 'a' term in the Van der Waals equation account for?

• Temperature in Kelvin.

• The ideal gas constant.

• Attraction between gas particles.

• Volume occupied by gas particles.

Which intermolecular force is the strongest?

• London dispersion forces

• Dipole-dipole interactions

• Hydrogen bonding

• Ion-dipole forces

How does the presence of intermolecular forces affect the boiling point of a substance?

• Has no effect on the boiling point

• Decreases the boiling point

• Only affects the melting point

• Increases the boiling point