Concept explainers
(a)
Interpretation: The following conversions should be performed using metric and U.S. conversion factors:
0.21 lb to g
Concept Introduction: Different units systems like metric and U.S systems are used to represents different units of measure values and also can convert into each other with the help of dimension analysis.
(b)
Interpretation: The following conversions should be performed using metric and U.S. conversion factors:
11.6 in to cm
Concept Introduction: Different units systems like metric and U.S systems are used to represents different units of measure values and also can convert into each other with the help of dimension analysis.
(c)
Interpretation: The following conversions should be performed using metric and U.S. conversion factors:
0.15 qt to mL
Concept Introduction: Different units systems like metric and U.S systems are used to represents different units of measure values and also can convert into each other with the help of dimension analysis.
(d)
Interpretation: The following conversions should be performed using metric and U.S. conversion factors:
35.41 kg to pounds
Concept Introduction: Different units systems like metric and U.S systems are used to represents different units of measure values and also can convert into each other with the help of dimension analysis.
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EP BASIC CHEMISTRY-STANDALONE ACCESS
- Determine whether each statement that follows is true or false: a The SI system includes metric units. b If two quantities are expressed in an equivalency, they are directly proportional to each other. c The scientific notation form of a number smaller than 1 has a positive exponent. d In changing a number in scientific notation whose coefficient is not between 1 and 10 to standard scientific notation, the exponent becomes smaller if the decimal in the coefficient is moved to the right. e There are 1000 kilounits in a unit. f There are 10 milliunits in a centiunit g There are 1000 milliliters in a cubic centimeter. h The mass of an object is independent of its location in the universe. i Celsius degrees are smaller than Fahrenheit degrees. j The uncertain digit is the last digit written when a number is expressed properly in significant figures. k The quantity 76.2 g means the same as 76.200 g. l The number of significant figures in a sum may be more than the number of significant figures in any of the quantities added. m The number of significant figures in a difference may be fewer than the number of significant figures in any of the quantities subtracted. n The number of significant figures in a product may be more than the number of significant figures in any of the quantities multiplied. o The process of analysis of a problem statement includes describing the properties of the given and wanted quantities. p If the quantity in the answer to a problem is familiar, it is not necessary to check to make sure the answer is reasonable. q Conversion factors can be used to change from one unit to another only when the quantities are directly proportional. r When you are learning chemistry, you should check the solution to each problem you solve at two levels: 1 is the value reasonable? 2 what new knowledge or skill did I obtain or improve? s There is no advantage to using units in a problem that is solved by algebra. t A Fahrenheit temperature can be changed to a Celsius temperature by multiplying by a conversion factor.arrow_forwardIn which of the following pairs do both numbers contain the same number of significant figures?a. 0.068 90 m3 and 6.89 m3b. 0.420 00 kg and 42 kgc. 10 m/s and 100 m/sd. 3.14 L and 3.14 * 10-3 Larrow_forwardConvert the following measurements.a. 5.70 g to milligrams d. 45.3 mm to metersb. 4.37 cm to meters e. 10 m to centimetersc. 783 kg to grams f. 37.5 g/mL to kg/Larrow_forward
- Convert 234.0 x10^-4 to the proper exponential notation following thr rules of significant figures. A. 2.340x10^2 B. 2.340x10^ 0 C. 2.340x10^-2 D. 2.34x10 ^ 3 E. 2.340x10^ 3 F. 2.340x10^-1 G. 2.34x10^-2 H. 2.34x10^2 I. 2.34x10 ^-3 J. 2.340x10^ -3 K. 2. 349x10^1 L. 2.340arrow_forwardConversions: include the correct number of significant digits and follow the format included in the image. a. 0.20 m to mm b. 2.23 ks to s c. 78.9 mg to garrow_forward1B 1. Perform the following metric-metric conversions: a. 52.1 kg to g b. 6.22 km to nm (must convert back to the base unit first) c. 1.93 mL to dL (must convert back to the base unit first) d. 28.1 uL to mL (must convert back to the base unit first) e. 3.21 km? to dm? (must convert back to the base unit first)arrow_forward
- 1. Convert the following values into the required units. Report answers in correct number of significant figures. A. 5.15 kg/m^3 to g/L B. 9.787 dyne to N 2. The mass of a diamond is usually expressed in carats, where 5.0 carats = 1.00 g. The density of diamond is 3.51 g/mL. What is the volume (in mL) of a 4.0-carat diamond?arrow_forwardUse the prefix multipliers to express each measurement without exponents. a. 1.2 x 10-9 m b. 22 x 10-1 s c. 1.5 x 10°g d. 3.5 x 10°Larrow_forwardof significant figures contained in each of the following measurements: b. 25.0 mL c. 54.7 mL3 d. 8.5090 g e. 0.0831 g 2. Perform the following calculations and report the answers with appropriate units and the correct number of significant figures: a. 53.18 g+1.014 g +0.3270 g 54.1949+ l. o14g b. 10.35 cm x 4.15 cm x 1.10 cm : 54.5619 54.52 c. 36.140 g 4.08 mL 3.2 5784319 3. A student uses a stoppered 25.0-mL volumetric flask to determine the density of a liquid. The mass of the empty flask and stopper was 25.1841 g. The mass of the stoppered flask filled with liquid up to the scratch mark was 45.0379 g. Calculate the density of the liquid in appropriate units and with the correct number of significant figures. 4. Calculate the error and percent error of a sample of water using the following data: the actual density of water at 23 °C is 0.999765 g mL"' and the experimental density (at 23 °C) is 1.097 g mL'. Show your work and watch your significant figures. -1 ost-Lab Questions Based…arrow_forward
- Write the following numbers in normal decimal notation.arrow_forward1. In which of the following pairs do both numbers contain the same number of significant figures? a. 2.0500 m and 0.0205 b. 600.0 K and 60 K c. 0.000 75 s and 75 000 s d. 6.240 L and 6.240 X 10 -² Larrow_forwardIt is known that the density of mercury is 13.54 times the density of water. What volume of this mercury in liters would weigh the same as 0.020m^3 of fuel oil, when the fuel oil weighs 9.42kN for every cubic meter? a. 71 b. 1.42 c. 1.7 d. 2.4arrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoIntroductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning