Name: ______date: ______hr ______

2016-2017Chemistry- CH 02 Study Guide, Measurements and Calculations, pages 29-57

  1. Know the basic steps of the scientific method. What is the scientific method used for?
  2. Define Scientific Law and scientific theory.
  3. What is the difference between precision and accuracy? Be able to define both.
  4. Does the percent error determine the precision or the accuracy of an experimental value?
  5. Know the equation to calculate percent error.
  6. What is the difference between a qualitative and quantitative data/observations?
  7. What are the two parts to any measurement?
  8. What measurement system do we use in the science laboratory?
  9. All measurements have a certain degree of uncertainty. What digit in a measurement is considered uncertain?
  10. What are the SI base units for: mass, length, time, and temperature?
  11. When using a graduated cylinder in class, what units are found on the graduated cylinder?
  12. What is a derived unit? ( pg 36) Give an example.
  13. What is the SI derived unit for volume? (pg 37)
  14. What is the equation used to solve for density? Know how to solve for volume and mass from this equation.
  15. What do the following prefixes mean: Giga- Mega- kilo-, hecto-, deka-, deci-, centi-, milli- micro- nano-
  16. What process do we use when converting from one unit to another?
  17. When taking a measurement with a piece of laboratory equipment, you always read with certainty off the instrument and then ______the last digit.
  18. Name two pieces or laboratory equipment you used this chapter that would not have any uncertainty in the measurement.
  19. When measuring with a centimeter ruler with millimeter marking, which decimal place would the uncertain digit be in?
  20. What is a conversion factor? What is it’s purpose?
  21. Complete the following:

  1. 1mL = ______L
  2. 1 kg = ______g
  3. 1 cm = ______m
  4. 1 dam = ______m
  5. 1mg = ______g
  6. 1 dL = _____ L

  1. Define significant figure.
  2. When writing a number in scientific notation, what numbers should the coefficient (M) be between?
  3. What number is the SI System based upon?
  4. What are each of the following physical quantities a measurement for? Grams, second, kelvin, kilogram, centigram, milliliter, deciliter, centimeters cubed, milliseconds, degree Celsius.
  5. State the rules of reporting significant figures when multiplying or dividing.
  6. State the rules of reporting significant figures when adding or subtracting.
  7. Write the following numbers in scientific notation:

  1. 0.000 673 0 km
  2. 6000 kg
  1. 55 000 000 000 mg
  2. 0.000 003 010 L

  1. How many sig figs are in the following measurements:

  1. 28.6 g
  2. 3440. cm
  3. 910 m
  4. 0.04604 L

  1. 0.006 700 0 kg
  1. Looking at each measurement circle the digit in the measurement that is ESTIMATED: 56.023g, 45.5 mg, 465.8900 mm, 46.450 cm.
  1. Round off each of the following measurements to the indicated number of significant figures:

  1. 2.685 to 3 sig figs
  2. 47.3745ml to 4 sig figs
  3. 8.352 ml to 2 sig figs
  4. 4.16578 L to 3 sig figs
  5. 24 km to 1 sig fig
  6. 0.048 51 mg to 2 sig figs
  7. 0.635 ml to 2 sig figs

  1. Do the following calculations and round to the correct number of sig figs:

  1. 5.44 mm – 2.6103 m
  2. 2.4 cm x 15.82 cm
  3. 4.07 g + 1.863 g
  4. 3127.55 cm – 784.2 cm
  5. 0.067 ml + 1.01 ml + 2.5 ml
  1. 36.427m + 12.5 m + 6.33 m
  2. 9.40 cm x 2.6 cm
  3. 8.08 dmx 5.3200 dm
  4. 1.50 g/ 2 cm3
  5. 0.084 21 g / 0.640 mL

  1. The density of silver (Ag) is 10.5 g/cm3. Find the mass of Ag that occupies 965 cm3 of space.
  2. Under certain conditions, oxygen gas (O2) has a density of 0.00134 g/mL. Find the volume occupied by 250.0 g of O2 under the same conditions.
  3. A student measures the mass of a sample as 9.67 g. Calculate the percentage error, given that the correct mass is 9.82g.
  4. The density of ethanol is 0.789 g/mL. Find the mass of a sample of ethanol that has a volume of 150.0 mL.
  5. A handbook gives the density of calcium as 1.54 g/cm3. Based on the lab measurements, what is the percentage error of a density calculation of 1.25 g/cm3?
  1. SOLVE USING DIMENSIONAL ANALYSIS
  1. How many liters are there in 13 cases of cola if each can is 12 oz and each case contains 24 cans( 1qt = 32 oz).
  2. Convert 75.0 cm to inches (1in = 2.54 cm)
  3. Convert 2300 lbs to grams ( 1 lb = 0.4536 kg)
  4. Convert 8100 mL to quarts ( 1L = 1.057 qt)
  5. Convert 37.6 knops into knips ( 4 clips = 5 blips, 1 knop = 6 bippy, 3 blip = 18 pringle, 1 clip = 10 knip, 10 bippy = 8 pringle)
  1. If you have .0092 gallons of ethyl alcohol with the density of 0.70 g/mL, what is the mass of the ethyl alcohol in grams? ( 1 qt = 946.3 mL, 1 gal = 4 qt)