Chapter 13 & 14 Jigsaw Topics Name:________________________________
Per:___
Kinetic-Molecular Theory and Gases
Jigsaw Topics – Focus Questions (for Conceptual Chemistry)
Overall Unit theme/understanding:
According to the Kinetic-Molecular Theory, the state of matter of a substance depends on the
kinetic energy of its particles and strength of attraction between the particles.
1. Kinetic Energy and Temperature: pg 55-56, 403, 418
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Define kinetic energy.

Define temperature. What is temperature really measuring?

Explain what determines the kinetic energy of a gas sample.

If the gases in Figure 13-3 were all at the same temperature, would their motion be identical? Why
or why not?
2. Kinetic Molecular Theory applied to gasses: pg 420-423

What are the postulates of the Kinetic-Molecular Theory?

What are the behaviors that result from each postulate? (how do gases move/interact with each other?)

How do chemists know that gases are in constant motion?
3. Boyle’s Laws: pg 431-433

Give the equation for Boyle’s Law.

Explain the relationship between temperature and volume of a gas.

Provide a specific, everyday example of when Boyle’s Law could be observed.
4. Charles’ Law: pg: 434-437

Give the equation for Charles’ Law.

Explain the relationship between pressure and volume of a gas.

Provide a specific, everyday example of when Charles’s Law could be observed.
5. Measuring Gases: pg 424 - 430

What are the measurable properties of a gas?

What units is each measured in?

What instruments and/or methods are used to measure each property?

What is STP (in oC and atm) and why is it important to consider when we are measuring gas
properties?
6. Ideal Gas Law: 441-443

Explain the formula for the ideal gas law. What does each letter represent?

If V and T are held constant, and more gas molecules (n) are added, what happens to the pressure?
Why?

If n and V are held constant, and temperature increases, what happens to the pressure? Why?

If n and T and held constant, and volume is decreased, what happens to the pressure? Why?

Explain the significance of this equation for the properties of all gases.