Unit 1 - Data Analysis

4,304 views
4,210 views

Published on

Published in: Business, Technology
0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total views
4,304
On SlideShare
0
From Embeds
0
Number of Embeds
3,913
Actions
Shares
0
Downloads
2
Comments
0
Likes
0
Embeds 0
No embeds

No notes for slide

Unit 1 - Data Analysis

  1. 1. Chapter 2
  2. 2. 30°C 30°F
  3. 3. SI unit
  4. 4. Measuring Volume We will be using graduated cylinders to find the volume of liquids and other objects. Read the measurement based on the bottom of the meniscus or curve. When using a real cylinder, make sure you are eye-level with the level of the water. What is the volume of water in the cylinder? _____mL What causes the meniscus? A concave meniscus occurs when the molecules of the liquid attract those of the container. The glass attracts the water on the sides.
  5. 5. Measuring Liquid Volume Imagescreatedathttp://www.standards.dfes.gov.uk/primaryframework/downloads/SWF/measuring_cylinder.swf What is the volume of water in each cylinder? Pay attention to the scales for each cylinder.
  6. 6. Measuring Solid Volume 10 cm 9 cm 8 cm We can measure the volume of regular object using the formula length x width x height. _____ X _____ X _____ = _____ http://resources.edb.gov.hk/~s1sci/R_S1Science/sp/e n/syllabus/unit14/new/testingmain1.htm We can measure the volume of irregular object using water displacement. Amount of H2O with object = ______ About of H2O without object = ______ Difference = Volume = ______
  7. 7.  How hot? How cold?  direction of Heat Transfer  Celsius – 0 0 C Freezing Point of Water 100 0 C Boiling Point of Water  Kelvin = C° + 273  No degree signs are used  O Kelvin = -273.150 C ▪ coldest possible temperature
  8. 8.  Length – size  meter (m)  Mass – amount of matter  Kilogram (kg) or gram (g)  Volume – space something takes up  Liter (l) or centimeters cubed (cm3 )  Temperature – amount of heat  Kelvin (K) = celsius + 273
  9. 9.  Measure of how much matter is squeezed into a given space  density = mass volume
  10. 10.  A block of wood and a block of steel have the same volume
  11. 11.  What happens to the density of an object if it is cut into pieces?  Which has the greater density, a single uranium atom or Earth?
  12. 12.  coefficient x 10 raised to a power  Single gram of hydrogen  602,000,000,000,000,000,000,000 molecules =  6.02 x 1023 molecules  Mass of an atom of gold  0.000000000000000000000327 grams =  3.27 x 10-22 grams
  13. 13.  36,000  3.6 x 104  503,000,000  5.03 x 108  0.00076  7.6 x 10-4
  14. 14. The valid digits of a number In measurement: includes all of the digits that are known, plus a last digit that is estimated
  15. 15.  Significant:  nonzero digits  final zeros after the decimal points  zeros between two other significant digits  Not significant  zeros used solely for spacing the decimal point are not significant.
  16. 16.  each have only two sig figs  0.0071 meter  0.42 meter  0.000099 meter  7.1 x 10-3 meter  4.2 x 10-1 meter  9.9 x 10-5 meter
  17. 17. ValueValue 5.605.60 5.65.6 0.0120.012 0.00120030.0012003 0.01200.0120 0.00120.0012 # of significant figures# of significant figures 33 22 22 55 33 22
  18. 18. If the digit immediately to the right of the last significant digit is less than 5, it is dropped  5 or greater - last significant digit increased by 1  41.58 square meters  41.6 square meters
  19. 19.  Round 65.145 meters to 4 sig figs  65.15m  Round 100.1°C to 1 sig fig  100°C  Round 154 cm to 2 sig figs  150  Round 0.000718 kilograms to 2 sig figs  0.00072
  20. 20.  Counting  Example: 23 people in the classroom ▪ (Not 22.9 or 23.1) 23.00000000……………….  Exactly defined quantities  Example: 60 minutes = 1 hour ▪ 60.00000000……………………..
  21. 21.  calculated answer cannot be too precise  not more precise than the least precise measurement  Multiplication and Division  same number of sig figs as the measurement with the least number of sig figs  Addition and Subtraction  same number of decimal places as the measurement with the least number of decimal places
  22. 22.  Accuracy  How close a measurement comes to the actual value of what is being measured  Precision  How close a series of measurements are to one another
  23. 23.  Difference between accepted value and experimental value  error = experimental value – accepted value  % error = x 100%error accepted value
  24. 24.  % error = x 100% 99.1°C – 100.0°C x 100% 100.0°C 0.9°C x 100% 100.0°C 0.9% error accepted value = = =

×