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**Zumdahl • Zumdahl • DeCoste**

World of CHEMISTRY Zumdahl • Zumdahl • DeCoste

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**Measurements and Calculations**

Chapter 5 Measurements and Calculations

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**Goals of Chapter 5: Measurement & Calculations**

Express numbers in scientific notation Learn English, metric, & SI system of measurement Use metric system to measure length, volume, and mass Significant digits Dimensional Analysis Temperature Scales Density/Specific Gravity Copyright © Houghton Mifflin Company

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**Qualitative vs. Quantitative**

Qualitative: appearance. the substance was a white powder Quantitative: Measurement The substance had a mass of 5.6 grams Copyright © Houghton Mifflin Company

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**Why are measurements important?**

Pay for gasoline by the gallon Construction: must have accurate measurements Welding: measurements must be accurate Automobiles: Most items on cars have a measurement Landscaping: Measurements important for spatial relationships Copyright © Houghton Mifflin Company

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Measurements: 2 Parts Number + Unit Number alone is meaningless If I tell you a 2 x 4 is 5 long – what does this mean: 5 feet, 5 inches, 5 meters? Unit alone is meaningless If I tell you the 2 x 4 is feet long – what does this mean: 2 ft, 4 ft, 8 ft? ALWAYS INCLUDE BOTH NUMBER AND UNIT! Copyright © Houghton Mifflin Company

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Scientific Notation Used to express very large or very small numbers Express using number between 1 & 10 multiplied by a power of 10 10 is to positive power for large numbers 10 is to a negative number for small numbers (decimals) Copyright © Houghton Mifflin Company

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Large Numbers Decimal point moved to left Power of 10 = # places moved = + number 125 = 1.25 x 100 = 1.25 x 102 Decimal point moved 2 places left 1700 = 1.7 x 1000 = 1.7 x 103 Decimal point moved 3 places left 93,000,000 = 9.3 x 107 Decimal point moved 7 places left Copyright © Houghton Mifflin Company

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**Small Numbers (Decimals < 1.0)**

Decimal point moved to the right Power of 10 = # places moved = negative number 0.010 = 1.0 x = 1.0 x 10-2 Decimal point moved right 2 places = 1.67 x 10-4 Decimal point moved right 4 places 0.089 = 8.9 x 10-2 Copyright © Houghton Mifflin Company

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Units Tell us what scale or standard is being used to represent measurement Scientists need common units to represent quantities like mass, length, time, and temperature If everyone had own set of units – chaos would result US uses English system, most of world (& scientists) use metric system, also SI system Copyright © Houghton Mifflin Company

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BASIC UNITS Physical Quantity English System Metric System Mass Pound or slug Gram or kilogram Length inch, foot, yard Centimeter or meter Volume Quart or gallon Liter, milliliter, or cm3 Time Hours, minutes, seconds Seconds Temperature Degrees Fahrenheit °C or Kelvin Copyright © Houghton Mifflin Company

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Metric Prefixes Kilo- hecto deka- UNIT deci centi- milli- k h dk d c m Move decimal point left Move decimal point right Power of 10 between each increment Copyright © Houghton Mifflin Company

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Examples 1000 meters = 1 km (decimal moved 3 places left) 1 meter = 100 cm (decimal moved 2 places right) 10 mm = 1 cm (decimal moved 1 place left) 1 Liter = 1000 mL (decimal moved 3 places to right) 600 grams = 0.6 kg (decimal moved 3 places left) Copyright © Houghton Mifflin Company

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Table 5.2 Copyright © Houghton Mifflin Company

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Table 5.3 Copyright © Houghton Mifflin Company

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**Figure 5.1: Comparison of English and metric units.**

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**Figure 5.2: Cube representations.**

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**Figure 5.3: A 100 mL graduated cylinder.**

1 mL = 1 cm3 1 milliliter = 1 cubic centimeter 100 mL = 100 cm3 Copyright © Houghton Mifflin Company

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Dimensional Analysis Copyright © Houghton Mifflin Company

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**Uncertainty of Measurement**

When using instrument to measure (such as a ruler or graduated cylinder), we visualize divisions between markings and estimate When making measurement, record all certain numbers and first uncertain number Copyright © Houghton Mifflin Company

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**Figure 5.5: Measuring a pin.**

Reading is between 2.8 cm & 2.9 cm These divisions were visualized 2.85 cm is measurement “5” is uncertain Copyright © Houghton Mifflin Company

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**Significant Figures Ex.**

Includes all numbers recorded in a measurement For pin, length = 2.85 cm: 3 significant figures All certain numbers plus first uncertain Assume to be accurate to ± 1 in last # Pin length is 2.85 ± 0.01 cm Pin is somewhere between 2.84 & 2.86 cm Copyright © Houghton Mifflin Company

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**Rules for Counting Significant Figures**

Captive zeros (between nonzero digits) Example: (4 s.f. - all numbers are significant) Trailing zeros (right end of number) Significant if bar is placed over zero or over zero to right Example: 200 (only #2 is significant = 1 s.f.) 2Ō0 (2 s.f. - 2 & Ō both significant) 20Ō (3 s.f. - 2 and both zeros are significant)

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Following decimal to right of nonzero digit = significant 5.00 = 3 s.f. Copyright © Houghton Mifflin Company

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**Non-significant zeros**

Leading zeros, precede non-zero digits Example: = 2 s.f. - zeros are non-significant Both: some numbers are sig. some are not Copyright © Houghton Mifflin Company

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**Rules for counting significant figures (continued)**

All nonzero integers are significant Example: 1457 has 4 s.f. Exact numbers have unlimited number of s.f. Determined by counting 8 apples, 21 students Not obtained from measuring devices From definitions 1 inch is exactly 2.54 cm Will not limit numbers in calculations

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Use same rules for scientific notation (10x not s.f.) Copyright © Houghton Mifflin Company

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**To give answer with correct number of significant figures – round off**

Look at number to right of last s.f. If number is <5 round down If number is ≥5 round up Do not round off until end of calculations

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**Rules for s.f. in calculations**

Multiplication & Division Answer should have same number of s.f. as measurement with smallest number of s.f. Example: 4.56 x 1.4 = → 6.4 (3 s.f.) (2 s.f.)* (2 s.f.)*

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Addition & Subtraction Limited by smallest number of decimal places Example: (2 decimal places) (1 decimal place)* (3 decimal places) → (1 decimal place)* Copyright © Houghton Mifflin Company

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**Figure 5.6: The three major temperature scales.**

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Temperature Scales Copyright © Houghton Mifflin Company

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**Converting between Kelvin & Celsius**

To convert from Kelvin to Celsius: T°C = TK – 273 Liquid Nitrogen boils at 77K, what is this in Celsius? T°C = 77 – 273 = -196 °C To convert from Celsius to Kelvin: TK = T°C The bp of water on top of Mt. Everest is 70 °C. Convert to K. TK = = 343 K

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**Figure 5.7: Converting 70 degrees Celsius to Kelvin units.**

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**Fahrenheit/Celsius Conversions**

To convert from Celsius to Fahrenheit: T°F = 1.80(T°C) + 32 If the temperature is 28°C, what is this in °F? T°F = 1.80(28) + 32 = = 82°F (2 s.f.) To convert from Fahrenheit to Celsius: T°C = (T°F – 32)/1.80 If you have a temperature of 101°F, what is this in °C? T°C = (101 – 32)/1.80 = 69/1.8 = 38°C Copyright © Houghton Mifflin Company

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**Figure 5.8: Comparison of the Celsius and Fahrenheit scales.**

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**Density: amount of matter in a given volume of substance**

Density = mass / volume Determine mass using a balance Determine volume by calculations, graduated cylinder, or water displacement Units are in g/cm3, g/mL, kg/L, lb/gal

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**Determining volume by water displacement**

Place water in graduated cylinder & record level Add object Record volume after addition of object Volume is difference between second volume and first volume Copyright © Houghton Mifflin Company

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Figure 5.9: Tank of water. Copyright © Houghton Mifflin Company

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**Figure 5.9: Person submerged in the tank.**

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Copyright©2004 by Houghton Mifflin Company. All rights reserved 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of.

Copyright©2004 by Houghton Mifflin Company. All rights reserved 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of.

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