Temperature Scales and Conversions

1. Temperature Scales and Conversions Boiling point of water 100°C 373.15 K 212°F freezing point of water 273.15 K 32°F 0°C 233.15 K - 40°F - 40°C Absolute zero 0 K - 459.67°F - 273.15°C Kelvin Fahrenheit °F = 9/5(°C) + 32 Celsius °C = K – 273.15 °C = 5/9(°F – 32)

2. Density = massvolume • Mass and volume are extensive, physical properties. • Density is an intensive physical property, the value of which changes with temperature. • SI units of density are kg/m3. • Commonly used units of density are g/cm3. • The density of water at 25°C is 1.00 g/cm3. • Materials with densities greater than water will sink in water (e.g. Au, density 19.32 g/cm3). • Materials with densities less than water will float on water (balsa wood, density 0.16 g/cm3).

3. massvolume Density = • I measure the mass of a chunk of metal and find it to be 26.113 g. I measure its volume by displacement and find it to be 10.0 mL. What is the density of the metal? density = 26.113g 10.0 mL = 26.113g 10.0 cm3 = 2.61 g/cm3 • I measure the mass of a cube of metal and find it to be 26.113 g. I measure one of its sides and find it to be 0.52 cm. What is the density of the metal? volume of a cube = (0.52 cm)3 = 0.14061 cm3 1 mL = 1 cm3 density = 26.113g 0.14061 cm3 = 1.9 x 102 g/cm3

4. massvolume Density = • Density is used to convert mass to volume. How many milliliters will 15.0 g of ethanol occupy when its density is 0.79 g/cm3? 15.0 g x conversion factor = volume in mL Remember: 0.79 g= 0.79 g cm3 mL 15.0 g x mL = 19 mL 0.79 g • Density is used to convert volume to mass. What is the mass of 100.0 cm3 of ethanol? 100.0 cm3 x conversion factor = mass in g 100.0 cm3 x 0.79 g = 79 gcm3

5. Density The red liquid is water with food color. What can be said about the density of the yellow liquid?

6. The Scientific Method and Measured Data • Central to the scientific method is the accumulation and study of measured data. • A measurement consists of two parts: a number and a unit. • Both must be reported correctly. • A systematic set of units (SI units and the metric prefixes) allows scientists from different areas to communicate easily. • A systematic way to report the number measured (by using the correct number of significant figures) communicates how good you think your measurements are.

7. Types of Numbers (Data) • Exact • numbers (data) obtained from counting • some conversions (e.g. 2.54 cm = 1 inch, exactly) • Inexact • most measured data Significant figures apply to inexact numbers!

8. Uncertainty in Measured Data Measured data is written to convey two (2) things! • the magnitude of the measurement • the extent of its reliability Worker #1 reports a mass of 12 g Worker #2 reports a mass of 12.0142 g 12 g means 12 ± 1 g 12.0142 g means 12.0142 ±0.0001 g 12 g has 2 significant figures. 12.0142 g has 6 significant figures. 12.0142 g is the more certain (reliable) number. The more significant figures a measurement has, the more certain it is.

9. Measured Values: Accuracy vs. Precision accurate and precise not accurate not precise precise but not accurate • Accuracy is how close your measured value is to the right value (can be shown by % error). • Precision is how well you can reproduce your measurement (can be shown by standard deviation).

10. Accuracy vs. Precision Data “symptom” precise but not accurate accurate but not precise Possible cause Poor calibration of the measuring instrument Inconsistent laboratory technique (you have control over this)

11. Recording Data to the Correct Number of Significant Figures 23°C 23°C The number of SFs in a measured value is equal to the number of known digits plus one uncertain digit. 22°C 22°C 21°C 21°C recorded value = 21.6°C recorded value = 21.68°C

12. Making Measurements in the Lab:Recording Volumetric Data to the Correct Number of Significant Figures - Glassware with Graduations Example B Example A 1. If the glassware is marked every 10 mLs, the volume you record should be in mLs.(Example A) 2. If the glassware is marked every 1 mL, the volume you record should be in tenths of mLs. 3. If the glassware is marked every 0.1 mL, the volume you record should be in hundredths of mLs.(Example B) 0 mL 30 mL 20 mL 1 mL 10 mL 30-mL beaker: the volume you write in your lab report should be 13 mL 2 mL Buret marked in 0.1 mL: you record volume as 0.67 mL

13. Making Measurements in the Lab:Recording Volumetric Data to the Correct Number of Significant Figures - Volumetric Glassware Look on the glassware for written indication of the precision of the volumetric flask or pipet. On this volumetric flask is written 500mL ± 0.2 mL. You would record the volume of the liquid in this flask as 500.0 mL.

14. Making Measurements in the Lab:Recording Masses to the Correct Number of Significant Figures This one is easy: record EVERY number (especially zeros) that appears on the display of the electronic balance. Trailing zeros MUST be recorded.

15. How to Count Significant Figures • All nonzero digits are significant (1.23 has 3 SFs). • All zeros between nonzero digits are significant (1.003 has 4 SFs). • Leading zeros are NEVER significant (0.01 has 1 SF). • Trailing zeros when a decimal point is present are significant (0.0780 has 3 SFs and180. has 3 SFs.) • Trailing zeros when no decimal point is shown are not significant. (180 has 2 SFs.)

16. Scientific Notation • An unambiguous way to show the number of significant figures (SFs) in your data • Numbers are written as the product of a number greater than or equal to 1 and less than 10 and a power of 10. Measurement in scientific notation #SFs 1.86282 x 105 mi/s 5.1900 x 10-3 m 5.121 x 103 g 6 5 4 186282 mi/s 0.0051900 m 512.1 x 101 g

17. Maintain the Correct Number of SFs When Performing Calculations Involving Measured Data • Multiplication/Division: The answer contains the same number of SFs as the measurement with the fewest SFs. 25.2 x 6.1 = 153.72 (but only 2 SFs are allowed) = 1.5 x 102 (correct answer) 25.2 = 7.3122535 (on my calculator) 3.44627 = 7.31 (correct answer) 25.2 x 6.1 = 44.604747 (on my calculator) 3.44627 = 45 (correct answer)

18. Maintain the Correct Number of SFs When Performing Calculations Involving Measured Data • Addition/Subtraction: The answer contains the same number of digits to the right of the decimal as that of the measurement with the fewest number of decimal places. 33.14159 - 33.04 0.10159 0.10 (correct answer) 2 SFs 3.14159 + 25.2 28.34159 28.3 (correct answer) 3 SFs • Calculators do NOT know these rules. It’s up to you to apply them!

19. Maintain the Correct Number of SFs When Performing Calculations Involving Measured Data • Addition/Subtraction: Dealing with numbers with no decimal places. Convert both numbers to exponential notation with the same power of ten, and then use the decimal place rule. 286.4 x 105 - 8.1 x 103 = ? 286.4 x 105 - 0.081 x 105 286.319 x 105 286.3 x 105(correct answer) 4 SFs

20. Maintain the Correct Number of SFs When Performing Calculations Involving Measured Data • Addition/Subtraction: Dealing with numbers with no decimal places. Write out the numbers and underline uncertain digit. 286.4 x 105 - 8.1 x 103 = ? 28,640,000 (uncertain in 10,000 place) - 8,100 (uncertain in 100 place) 28,631,900 (take the uncertain digit farthest to the left) 28,630,000 or 2.863 x 107 4 SFs

21. Maintain the Correct Number of SFs When Performing Calculations Involving Measured Data • Combined operations: Do the add/subtract first, carrying all digits, then do the multiply/divide. The only time you round is at the very end of the calculation. % difference = 100 x (your value - accepted value) accepted value an exact number…it does not affect SFs

22. Maintain the Correct Number of SFs When Performing Calculations Involving Measured Data Find the percent difference between 3.015 and an accepted value of 3.025. % difference = 100 x (3.015 - 3.025) 3.025 First, subtract 3.025 from 3.015: 3.015 - 3.025 result has 2 SFs - 0.010 Second, multiply by 100 and divide by 3.025 (4 SFs) (in either order): - 0.3305785 Finally, round to 2 SFs: - 0.33 %

23. Converting Measurements Using Dimensional Analysis • Helps ensure that the answers to problems have the proper units. • Uses conversion factorsto reach the proper units. • Aconversion factoris a fraction whose numerator and denominator are the same quantity expressed in different units. 2.54 cm = 1 inch (2.54 cm and 1 inch are the same length.) 2.54 cm 1 inch and are conversion factors. 1 inch 2.54 cm

24. Converting Measurements Using Dimensional Analysis • Convert 16.7 gallons to liters. 3.785 L 16.7 gal x = 63.2 L 1 gal • Convert 0.8474 liters to cubic meters (m3). 1000 cm3 10-2 m 10-2 m 10-2 m 0.8474 L x ----------- x ---------- x --------- x --------- = 8.474 x 10-4 m3 1 L 1 cm 1 cm 1 cm OR 3 1000 cm3 10-2 m 0.8474 L x ----------- x ---------- = 8.474 x 10-4 m3 1 L 1 cm

25. Problem The density of air at ordinary atmospheric pressure and 25°C is 1.19 g/L. What is the mass, in kilograms, of the air in a room that measures 12.5ft x 15.5ft x 8.0ft? The volume of the room is: 12.5 ft x 15.5 ft x 8.0 ft = 1550 ft3 (we worry about sig figs at the end) d = m , so volume x density = mass v The density of air is given in g/L…let’s convert it to units of kg/L: 1.19 g x 1 kg = 1.19 x 10-3 kg L 1000 g L

26. Problem density = 1.19 x 10-3 kg/L volume = 1550 ft3 volume x density = mass We can either convert L to ft3 orft3 to L…I choose the latter: 1550 ft3 x 12 in x 12 in x 12 in x 2.54 cm x 2.54 cm ft ftft in in x 2.54 cm x 1 mL x 1 L x 1.19x10-3kg in 1 cm3 1000mL L = 52 kg

27. Problem 1550 ft3 x 12 in x 12 in x 12 in ft ft ft x 2.54 cm x 2.54 cm x 2.54 cm in in in x 1 mL x 1 L = 43891 L 1 cm3 1000mL This conversion from cubic feet to L may also be written 1550 ft3 x 12 in 3 x 2.54 cm3 x 1 mL x 1 L ft in 1 cm3 1000mL = 43891 L