Study Guide- Matter and Gas Laws

MATTER REVIEW 1. What is the kinetic theory of matter?

An explanation for how the particles in matter behave.

2. What are the 3 main ideas in the Kinetic Theory? 1) All matter is composed of small particles 2) These particles are in constant motion that has no pattern 3) The particles collide and crash into each other and the walls of their container.

3. Fill in the chart below with the correct information:

State SOLID LIQUID GAS PLASMA

Dra

win

g

Volume and shape…

Fixed volume Fixed Shape

Fixed volume NO fixed shape

NO fixed volume NO fixed shape

How much kinetic

energy? LOW kinetic energy

MEDIUM kinetic energy

HIGH kinetic energy

VERY HIGH kinetic energy

Intermolecular attraction

(high, medium, low,

very low)

HIGH Molecules have little

kinetic energy, so they can’t break free of attractive forces

MEDIUM LOW Virtually none

Describe HOW it moves…

Particles vibrate against each other

Particles slide/flow past each other

Particles bounce around randomly and hit each other and their container

4. The most common state of matter in the universe is plasma 5. Solids have a definite shape and volume. Solids have a fixed shape because there is a strong force

of intermolecular attraction.

6. Liquids have a definite volume but not a definite shape. Liquids can take the shape of their container because they have enough kinetic energy to overcome some of the intermolecular forces of attraction.

Binder Page:

6-12

7. Gases have NO definite shape & volume, they are free to move in all directions and spread throughout their containers. Gases can fill their container because they have enough kinetic energy to overcome all of the intermolecular forces of attraction.

8. Fill in the blank with the name of the phase change process: 1) Gas → liquid condensation 2) Gas → solid deposition 3) Liquid → gas evaporation 4) Liquid → solid freezing 5) Solid →liquid melting 6) Solid → gas sublimation

9. Look back at your drawings of the particles in a solid and a gas. What makes gases easier to

COMPRESS than solids? Gases are less dense, so they have more spaces between their particles, so there is more space to compress.

10. A cold glass will collect moisture on a hot, humid day. Explain this event according to the kinetic theory of matter. The low-temperature, low energy molecules in the glass will absorb thermal energy from the gas (air) around the glass. When the air loses energy it condenses to form water on the outside of the glass.

11. When a cup of coffee is steaming hot, the molecules in the coffee are moving fast. As the coffee cools off, the speed of the molecules will slow down.

12. Most substances will contract when they go cool off. For example: when muffins in a pan cool off, they pull away from the sides of the pan. Water is unusual because it expands when it goes from a liquid to a solid state. An example of this is when ice cubes get stuck in a tray once they freeze.

13. Based on the Kinetic Theory of Matter, why does water to turn it into steam when thermal energy is added? Water molecules on the water’s surface gain enough thermal energy to overcome intermolecular forces, separate from the other molecules, and change into the gas phase

14. On a heating curve (temperature vs. heat graph) why does the temperature plateau (get flat) in certain areas? The substance is changing state. All of the thermal energy is used to change state, so the temperature doesn’t change while a phase change is happening and the graph goes flat for a segment of time.

15. Using the heating curve to the right, write the state of matter for each part of the graph:

A. solid B. solid/ liquid C. liquid D. liquid/ gas E. gas

16. What is happening at parts B and D? phase changes

17. What is the melting/freezing point of this substance? _______-60_______°C

18. What is the boiling point of this substance? ____60______°C

GAS LAW REVIEW 19. Describe Boyle’s Law: When temperature is kept constant, the pressure and volume of a gas

are inversely proportional.

20. Describe Charles’ Law: When pressure is kept constant, the volume and temperature of a gas are directly proportional.

21. If the same amount of air is pumped into 2 containers. Container A has a larger volume and container B has smaller volume, describe the pressure in the containers. The pressure in container A is lower than container B.

22. Which gas law states that the volume of a gas increases when the temperature increases, as long as pressure does not change? Charles’s Law (HINT: Poor Charles is under constant pressure!)

23. Which gas law states that if you decrease the volume of a container of gas and hold the temperature constant, the pressure of the gas will increase? Boyle’s Law (HINT: Water stays the same, constant temperature when it is BOYLE-ing.)

24. Two gases are in containers. Both gases are at 1 atm of pressure and 0°C. Which of the following is true?

A. Both gases are oxygen gas. B. Both gases have particles moving with the same velocity. C. Both gases have the same average kinetic energy. D. Both gases have the same average potential energy. E. Both gases have the same mass.

25. Hot air balloons are not inflated using a pump. Instead, they are inflated using heat. If you want the air in the hot air balloon to expand and inflate the balloon, what could you do to the gas molecules? Add heat to the molecules. This will increase their thermal energy, which means they will expand and inflate the balloon

26. According to Charles’s Law what will happen to the size of a fully-inflated balloon if it is placed in a freezer? The volume (size) will decrease. Under constant pressure, if the temperature of a gas decreases, then the volume will decrease.

27. The pressure in this situation is kept constant. What happens to the volume of a gas as it is heated? It increases Which law is illustrated here? Charles’s Law

28. The temperature in this situation is kept constant. What happens to the pressure of a gas as the volume is increased? Pressure decreases. Which law is illustrated here? Boyle’s Law

29. The pressure is very high at the bottom of the ocean (up to 500 atm!), but low at sea level (1 atm). A diver exhales some air bubbles while deep in the ocean. What happens to the diameter of the bubbles as they ascend to the surface if we assume temperature stays the same? The diameter increases Will the number of bubbles change as they head to the surface? No. The bubbles expand because there is less pressure pushing on them, but the bubbles don’t disappear.

30. According to the graph, as the pressure increases, the volume decreases. Since the graph doesn’t account for temperature, we assume that temperature was kept constant. Which law is illustrated by this graph? Boyle’s Law

31. According to the graph, as the temperature increases, the volume increases. Since the graph doesn’t account for pressure, we assume that pressure was kept constant. Which law is illustrated by this graph? Charles’s Law