Matter, Measurement, & States of Matter Review Sheet

  1. Describe the difference between an extensive property and an intensive property. Then give one example of each.
  1. List one example of the following:
  1. Physical property ______
  2. Chemical property______
  3. Physical change______
  4. Chemical change______
  1. Define density and calculate the density of an unknown substance with a mass of 26.3 g and a volume of 6 cm3. If the known density of this substance were 4.9 g/cm3, calculate the percent error.
  1. Describe endothermic and exothermic REACTIONS. Make sure to state how the temperature would change as these processes occur.
  1. Using the flow chart created in class, identify the following examples. State all terms that apply, meaning there could be more than one term to describe.
  1. Italian Dressing______
  2. Water______
  3. Graphite______
  4. Salt Water______
  5. Carbon Dioxide______
  1. Give one example of a qualitative and quantitative measurement. Remember what a “good” qualitative measurement should contain.

7. Convert the following using the method of dimensional analysis. Show all work and units!!!!

16 oz = 1 lb / 1 in = 2.54 cm / 2000 lbs = 1 ton
1 oz = 28.35 g / 1 ft = 12 in / 1 cm3 = 1 ml
1 kg = 2.2 lbs / 1 mi = 1.61 km / 1 gal = 4 qts
1 L = 1.06 qts / 1 mi = 1760 yds
  1. How many inches are in 45.6 meters?
  1. How many hectograms are in 250,000 milligrams?
  1. Determine the number of gallons of water that are equivalent to 85,000 milliliters.
  1. How many square meters are equivalent to 0.243 square kilometers.
  1. Determine how fast a car is moving in meters per min if the speedometer in the car is reading 53.2 miles per hour.

8. a. Determine how many significant figures are in each of the following values.

2.001 _____0.00085 _____150,000 _____4.50 x 108 _____

b. Round the following values to two significant figures.

456 ______0.10778 ______600,000 ______180.65 ______

c. Calculate the following and express all answers in the correct number of significant figures.

6.201 cm + 7.4 cm+0.68 cm+12.0 cm= ______

1.6 km + 1.62 m +1200 cm= ______

8.264 g - 7.8 g= ______

1.31 cmx2.3 cm= ______

5.7621 mx6.201 m= ______

20.2 cm / 7.41 s=______

40.002 g / 13.000005 g= ______

  1. Identify which phase changes are endothermic and which are exothermic.

Endothermic /
Exothermic /


State whether each of the following (10-15) describe a solid, liquid, or gas

  1. Particles slide past one another. ______
  2. Kinetic energy is the lowest in this state of matter.______
  3. Particles have the ability to flow and possess definite volume. ______
  4. Highly compressible and takes the shape of its container. ______
  5. Has both a definite volume and definite shape. ______
  6. Possess very low densities. ______
  1. Describe how energy changes as a substance is being heated from a solid into a liquid and then into a gas. (Need to be able to do this for cooling a substance as well)
  1. What factors affect the equilibrium of a substance?

Use the cooling curve above to answer questions 18-25

  1. What is the temperature when condensation occurs?
  1. If the temperature of the substance is at 80°, what is its physical state?
  1. Is the curve considered an endothermic or exothermic process?
  1. Between what letters is KE decreasing?
  2. If the temperature for freezing is 20°, what temperature does this substance melt?
  1. When and at what temperature does this substance finish condensing?
  1. If analyzing this substance 9 minutes after cooling, what would one observe?
  1. If there was 1.18 moles of the unknown substance being cooled in the above curve, calculate the total amount of energy needed for this cooling process. (Hint: 1 mol = 55 g, Hfus = 3950 J/g , Specific Heat Capacities are Csolid=163.8 J/g·oC, Cliquid = 273 J/g·oC, and Cgas= 109.2 J/g·oC)

Use the phase diagram above to answer 26-32

  1. At what temperature and pressure would all three phases be present?
  1. If the substance was at a pressure of 100 atm and 150 K. What physical state would be present once the temperature rises to 400 K? Describe any phase changes that occurred.
  1. If the substance was at a pressure of 200 atm and 300 K was allowed to decrease in pressure to 50 atm, what is the phase change observed?
  2. At what approximate temperature does the critical point occur?
  3. Describe what is occurring and what would be observed at a pressure of 150 atm and a temperature of 350 K?
  1. Describe the change in the movement of particles as the substance transitions in question # 29.
  1. If this substance were held at a temperature of 100 K and it’s pressure was raised from 1 atm to 100 atm, describe what phase change occurs.