Honors Chemistry Chapter 2 Problem Handout Solve the following on separate sheets of paper. Where appropriate, show all work. 1. Convert each of the following quantities to the required unit. a. 12.75 mm to kilometers b. 277 cm to meters c. 30560 m 2 to hectares (1 ha = 10000 m 2 ) d. 3857 grams to milligrams e. 68.71 kl to liters 2. A person drinks eight glasses of water each day, and each glass contains 300 ml. How many liters of water will that person consume in a year? What is the mass of this volume of water in kilograms? (Assume one year has 365 days and the density of water is 1.00 kg/l). 3. At the equator the Earth rotates with a velocity of 465 m/s. a. What is this velocity in kilometers per hour? b. What is this velocity in kilometers per day? 4. A textbook measure 250. mm long, 224 mm wide, and 50.0 mm thick. It has a mass of 2.94 kg. a. What is the volume of the book in cubic meters? b. What is the density of the book in grams per cubic centimeter? c. What is the area of one cover in square meters? 5. Determine the number of significant figures in the following measurements: a. 0.1020 m b. 11.5 ml c. 101 g d. 360 cm 2 e. 0.97 km f. 1000 kg g. 180. mm h. 0.4936 L i. 0.020700 s 6. Perform the following calculations, and express the answer in the correct units and number of significant figures. a. 651 cm x 75 cm b. 7.835 kg 2.5 L c. 14.75 L 1.20 s d. 360 cm x 51 cm x 9.07 cm e. 7.945 J + 82.3 J 0.02 J f. 0.0012 m 0.00045 m 0.00011 m g. (0.054 kg + 1.33 kg) x 5.4 m 2 h. 690 000 m (5.022 h 4.31 h) 7. Express the following quantities in scientific notation: a. 158000 km b. 0.000009782 L c. 0.00593 g d. 1050000000 Hz
8. Perform the following calculations and express the result in scientific notation with the correct number of significant figures: a. 2.48 x 10 2 kg + 9.17 x 10 3 kg + 7.2 x 10 1 kg b. 4.07 x 10-5 mg + 3.966 x 10-4 mg + 7.1 x 10-2 mg c. 9.81 x 10 27 molecules + 3.18 x 10 25 molecules 2.09 x 10 26 molecules d. 1.54 x 10-1 L 2.36 x 10-4 s 9. 22400 ml of oxygen gas contains 6.022 x 10 23 oxygen molecules at 0 o C and standard atmospheric pressure. a. How many oxygen molecules are in 0.100 ml of gas? b. How many oxygen molecules are in 1.00 L of gas? c. What is the average space in milliliters occupied by one oxygen molecule? 10. Calculate the density (in g/ml) of a substance that has a mass of 2.80 g and a volume of 2.00 L. 11. Determine the volume that 35.2 grams of carbon tetrachloride will occupy if it has a density of 1.60 g/cm 3 (1 ml = 1 cm 3 ). 12. The density of ethanol is.789 g/ml. What is the mass of 150 ml of ethanol? 13. A block of lead measures 20.00 mm x 30.00 mm x 45.00 mm. Calculate the mass of this block, if the density of lead is 11.34 g/cm 3. 1. a. 1.275 x 10-5 km b. 2.77 m c. 3.056 ha d. 3857000 mg e. 68710 L 2. 876 L 876 kg 3. a. 1670 km/h b. 40200 km/day 4. a. 2.80 x 10-3 m 3 b. 1.05 g/cm 3 c..0560 m 2 5. a. 4 b. 3 c. 3 d. 2 e. 2 f. 1 g. 3 h. 4 i. 5 6. a. 4.9 x 10 4 cm 2 b. 3.1 kg/l c. 12.3 L/s d. 1.7 x 10 5 cm 3 e. 90.2 J f..0006 m g. 7.5 kg m 2 h. 970000 m/h 7. a. 1.58 x 10 5 km b. 9.782 x 10-6 L c. 5.93 x 10-3 g d. 1.05 x 10 9 Hz 8. a. 9.49 x 10 3 kg b. 7.1 x 10-2 mg c. 9.63 x 10 27 molecules d. 6.53x 10 2 L/s 9. a. 2.69 x 10 18 molecules b. 2.69 x 10 22 molecules c. 3.72 x 10-20 ml 10. 1.40 x 10-3 g/ml 11. 22.0 cm 3 12. 120 g 13. 306.2 g
Chap 1-2 Study Guide - MULTIPLE CHOICE 1. Chemistry is best defined as the study of a. the structure of matter. b. all substances and the changes that they can undergo. c. the substances found on the periodic table and the compounds they form. d. what happens when two elements are mixed together. 2. The capacity to do work is called a. temperature. c. force. b. energy. d. heat. 3 The energy possessed by objects because of their position or the arrangement of their particles is called a. kinetic energy. c. radiant energy. b. electrical energy. d. potential energy. 4 What kind of energy is carried by objects in motion? a. kinetic energy c. radiant energy b. electrical energy d. potential energy 5. What is the SI base unit for mass? a. kilogram c. liter b. mole d. gram 6. Which of the following is a derived unit? a. cm 3 c. kilogram b. meter d. Fahrenheit 7. The chemical energy stored in coal is an example of a. kinetic energy. c. radiant energy. b. electrical energy. d. potential energy. 8. Which of the following is a prefix that makes the unit larger? a. kilo- c. millib. deci- d. pico- 9. A milliliter is the same volume as a a. cubic centimeter. c. centimeter. b. millimeter. d. cubic meter. 10. A recorded measurement has two certain digits and one estimated digit. How many significant digits does the measurement have? a. none c. two b. one d. three 11. In which of the following is the zero not significant? a. 0.15 c. 1.50 b. 1.05 d. 1.015 12. A meter is defined as 100 cm. How many significant digits are there in the value 100? a. one c. three b. two d. an infinite number 13. In multiplication and division of measured values, the measured value that determines the number of significant digits in the answer is the one that has the a. largest number of significant digits. c. largest number of decimal places. b. smallest number of significant digits. d. smallest number of significant zeros.
14. How should you round off a number that ends with the digit 5? a. Round down. b. Round up. c. Round off so that the last digit you retain has an even value. d. Round off so that the last digit you retain has an odd value. 15.A number written in scientific notation is made up of the a. significant digits of the original number. b. significant digits of the original number and 10 written with an exponent. c. original number with all digits after the decimal place removed. d. number 10 written with an exponent equal to the number of significant digits in the original number. 16. The percent error is equal to 100 percent multiplied by a. b. c. d. 17.Density is equal to a. mass/volume. c. volume/mass. b. mass volume. d. mass + volume. 18.The amount of heat needed to raise the temperature of 1 gram of water by 1 Celsius degree is called a a. joule. c. kelvin. b. degree Fahrenheit. d. calorie. Figure 1-2 19. In Figure 1-2, how should the length indicated by the arrow along the ruler be recorded? a. 0.3 cm c. 0.35 cm b. 0.4 cm d. 0.350 cm 20. What metric unit is indicated by each of the shortest lines on the ruler in Figure 1-2? a. centimeter c. millimeter b. micrometer d. one-sixteenth inch 21.In Figure 1-2, how should the volume reading for the water be recorded? a. 7.00 cm 3 c. 8.00 cm 3 b. 7.0 cm 3 d. 8.0 cm 3 22. What metric unit is indicated by each of the lines on the graduated cylinder in Figure 1-2? a. centimeter c. liter b. cubic centimeter d. cubic milliliter
23 What is the SI unit of energy? a. joule c. kelvin b. degree Fahrenheit d. calorie MASS OF SAMPLE 4078 Team 1 Team 2 Team 3 Team 4 Reading 1 42 g 41.04 g 31.33 g 42.34 g Reading 2 42.158 g 39.77 g 31.30 g 41.12 g Reading 3 42.07 g 43.15 g 31.36 g 41.21 g Average 42.1 g 41.32 g 31.33 g 41.55 g Accepted measure from issuing lab: 41.33 g Percent error 1.9% 0.02% 24.2% 0.53% Figure 1-3 24. Which team in Figure 1-3 is most accurate? a. team 1 c. team 3 b. team 2 d. team 4 25. Which team in Figure 1-3 is most precise? a. team 1 c. team 3 b. team 2 d. team 4 26 Which of the following is a statement of the law of conservation of energy? a. Energy must be conserved in order to have enough energy for the future. b. In chemical processes, it is best to conserve as much energy as possible. c. In any process, energy is neither created nor destroyed. d. Energy cannot be transformed from one kind of energy into another kind. 27 What is the SI scale for temperature? a. Fahrenheit scale c. Celsius scale b. Kelvin scale d. none of the above PROBLEM SOLVING 28. Express 4.5 millimeters in meters. 29. Convert 12.1 kilograms to grams. 30.Express 3.56 Mg in µg. (M = 10 6 ; µ = 10-6 ) 31.Determine the number of significant digits in each of the following measured values: (a) 6.7090 (b) 0.0384 (c) 12,000 (d) 3400. (e) 100.050 32.Calculate the volume of a rectangular pan that is 27.0 cm long, 14.55 cm wide, and 9.3 cm high. (Remember to retain only significant digits in your final answer and to express your answer in the proper units.) 33.Write the following numbers in scientific notation: (a) 1450. (b) 16,300 (c) 0.002360. Write the following numbers in ordinary notation: (d) 7.72 10 3 (e) 9.14 10 5 (f) 5.391 10 7. 34.A student measures the mass of an object as 135.80 g. Calculate the percent error in the measurement, given that the accepted value for the mass is 137.23 g. 35. Calculate the density of an object that occupies 17.1 cm 3 and has a mass of 39.26 g. Will that object float in water, given that the density of water is 1.00 g/cm 3? Explain your answer. 36. Find the mass of an object with a density of 4.5 g/cm 3 and a volume of 12 cm 3.
37. Find the volume of an object with a density of 0.76 g/cm 3 and a mass of 106.4 grams. 38. Convert 73.0 seconds to weeks. Express your answer in scientific notation. 39. Convert a height of 5 feet, 6 inches to meters. (2.54 cm = 1 in.) 40. Which temperature scales have units of equal size? a. Fahrenheit and Celsius c. Celsius and Kelvin b. Kelvin and Fahrenheit d. none of the above 41. Which equation correctly relates the Celsius and Kelvin scales? a. K = C 273 c. K = C + 100 b. C = K + 273 d. C = K 273 42. What is absolute zero? a. zero degrees on the Celsius scale b. the point at which the potential energy of particles is zero c. the point at which the motion of particles ceases d. the temperature at which water freezes 43. On the Kelvin scale, the lowest possible temperature has a value of a. 0 K. c. 32 K. b. 273 K. d. 273 K. 44. Anything that has mass and volume is called a. plasma. c. weight. b. matter. d. density. 45. Which state of matter is characterized by definite shape and definite volume? a. plasma c. solid b. liquid d. gas 46. Which state of matter is characterized by definite volume but lack of definite shape? a. plasma c. solid b. liquid d. gas 47. Which of the following is not simply a change in state? a. melting c. freezing b. burning d. boiling 48. Which of the following is a physical property? a. flammability c. tendency to rust b. density d. none of the above 49. Which of the following is a physical change? a. cooking c. rusting b. burning d. crushing 50. A substance that cannot be separated into simpler substances by a chemical change is called a(n) a. compound. c. element. b. mixture. d. crystal. 51. A substance that contains two or more elements chemically combined in a fixed proportion is called a a. plasma. c. heterogeneous mixture. b. compound. d. homogeneous mixture. 52. Pure substances include a. elements only. c. compounds and mixtures. b. elements and compounds. d. elements and mixtures.
53. Which of the following is the formula of a compound? a. CO c. Mg b. Co d. K + B 54. A blend of two or more pure substances is called a(n) a. plasma. c. mixture. b. compound. d. element. 55. Which of the following is an example of a heterogeneous mixture? a. sand in water c. salt dissolved in water b. homogenized milk d. air 56. Which of the following is an example of a homogeneous mixture? a. oil and water c. sawdust and nails b. salt dissolved in water r d. sand in water 57.Which of the following techniques cannot be used to separate homogeneous mixtures? a. distillation c. chromatography b. crystallization d. filtration Figure 2-2 58. What does the Sample 1 in Figure 2-3 illustrate? a. a gas c. plasma b. a solid d. a liquid 59. What does the Sample 2 in Figure 2-3 illustrate? a. a gas. c. plasma. b. a solid. d. a liquid. Figure 2-3 60.In which of the samples shown in Figure 2-3 is the density high? a. sample 1 only c. samples 1 and 3 b. sample 2 only d. samples 2 and 3 61. Convert 450 C to the Kelvin scale. 62. Convert 58 K to the Celsius scale. 63. Identify each of the underlined phrases in the following account of a laboratory procedure as either a chemical change or a physical change. Explain your answers. The unknown substance was tested to determine its properties. First, a sample was ground up finely with a mortar and pestle. Next, samples were dissolved in water and other solvents. A Bunsen burner was lighted and some of the pure chemical was placed into a test tube and heated gently until it melted. Because the heating was too rapid, the test tube cracked and the experiment was repeated. Heating was continued this time until the substance boiled. Some fumes of the boiling substance reacted with oxygen in the air to form a white powder
1. b 2. b 3. d 4. a 5. a 6. a 7. d 8. a 9. a 10. d 11. a 12. a 13. b 14. b 15. b 16. b 17. a 18. d 19. c 20. c 21. b` 22. b 23. a. 24. b 25. c 26. c 27. b 40. c 41. d 42. c 43. a. 44. b 45. c 46. b 47. b 48. b 49. d 50. c 51. b 52. b 53. a 54. c 55. a 56. b 57. d 58. d 59. a 60. c 61. 723 K 62. -215 o C 28..0045 m 29. 12100 g 30. 3.56 x 10 12 µg 31. a. 5 b. 3 c. 2 d. 4 e. 6 32 3700 cm 3 33. a. 1.450 x 10 3 b. 1.63 x 10 4 c. 2.360 x 10-3 d..0072 e. 914000 f..0000005391 34. -1.04% 35. sink, d = 2.30 g/ml and the d H2O = 1 g/ml 36. 54 g 37. 140 cm 3 38. 1.21 x 10-4 weeks 39. 1.7 m