Honors Chemistry: Chapter 1- Problem Set
Classify the following as always true (AT), sometimes true (ST), or never true (NT) 1. Organic Chemistry is the study of substance that do not contain carbon.
2. The goal of chemistry is to accumulate knowledge.
3. Biochemistry is the study of the chemistry of living organisms.
4. Organic chemistry overlaps with physical chemistry.
5. Applied chemistry is used to attain specific goals.
6. All plastics are polymers.
7. World energy demand is staying at a constant level.
8. Nitrogen oxide emissions are a major contribute to smog.
9. A theory can be easily proved.
10. Scientific laws explain natural phenomena.
11. A well-planned experiment will disprove a hypothesis.
Match each description in Column B with the correct term in Column A
Column A Column B
12. chemistry a. study of essentially all compounds that contain 13. organic chemistry carbon
14. inorganic chemistry b. study of the composition of substances
15. physical chemistry c. study of essentially all compounds that do not 16. analytical chemistry contain carbon
17. biochemistry d. study of the chemistry of living organisms
e. study of the composition of matter and the changes it undergoes f. study of the behavior of chemicals
18. Match each activity below to one of the five branches of chemistry a. determining the boiling point of a liquid
b. finding out how much nitrogen is in a sample of a substance c. learning about the chemistry of iron ore
d. studying the process of photosynthesis
e. synthesizing (making) sucrose, a substance that contains carbon
19. List two advantages of producing electricity from solar energy instead of fossil fuels.
20. Classify each step in the following application of the scientific method as an observation, hypothesis, experiment, or theory.
a. An iron bass falls to Earth when you drop it.
b. Earth is a giant magnet.
c. An iron ball and a piece of wood are dropped at the same time from the same height.
d. The iron ball and wood fall at the same rate.
e. The large mass of Earth caused it to exert the same gravitational attraction on any object, regardless of the object’s composition.
Honors Chemistry: Problem Set Chapter 2
1. Classify the following as pure substances or mixtures. If a pure substance, classify as compound or element. If a mixture classify as homogeneous or heterogeneous.
a. sodium chloride g. chlorine b. sugar-water h. steam
c. club soda i. homogenized milk
d. iron j. water
e. steel k. salad
f. carbon dioxide l. calcium
2. Identify the following as physical properties or chemical properties.
a. state (solid, liquid, gas) b. color
c. flammability d. melting point e. freezing point
f. reacts with acid to form H2 gas
3. Identify the changes as physical changes or chemical changes.
a. rusting
b. carving a figure out of a block of wood c. dissolving salt in water
d. putting food coloring in water.
e. Cooking an egg f. Milk souring
4. What is an alloy? List 2 common alloys and the components of the alloy.
5. For the following reaction: 2H2 + O2 2H2O a. What are the reactants?
b. What are the products?
c. If 26.40g of oxygen produced 79.24g of water, how much hydrogen would have reacted? (don’t forget sig figs)
Honors Chemistry Problem Set – Chapter 3A Scientific Measurement
1. Classify each of these statements as always true (AT), sometimes true (ST) or never true (NT).
a. Qualitative measurements give results in a definite form, usually as numbers.
b. Scientific notation is used to express large numbers in a convenient format.
c. Units are used to express quantitative measurements.
d. In standard scientific notation, the coefficient is 1 and 10.
e. The SI base unit of mass is the milliliter.
f. A decigram is 100 times smaller than a gram.
g. The SI unit of volume is derived from the unit of length.
h. There are six basic SI units of measurement.
i. The density of a substance decreases as its temperature is increased.
2. Classify each of the following terms as qualitative or quantitative.
a. a cold shower b. a dozen roses
c. nine innings d. a tall building
3. For each of the following numbers
i. Write the measurement in scientific notation ii. Count the number of significant figures
iii. Identify the quantity measured (ex 32m = length)
a. 10 cm3 e. 0.00000982 mL
b. 450000 mg f. six
c. 0.2 g/mL g. 0.0031 mm
d. 37C h. 2300 mol
4. Perform the following operations and write the answers with the correct units and the correct number of significant figures.
a. 37.2 mL + 18.0mL + 380mL = b. 37.2 cm x 18.0cm x 380cm = c. 8.13 x 104cm3 3.8 x 102 cm = d. 4.552 kg + 3.14kg=
e. 30.44 kg +39422 kg=
f. 750. cm – 677.4 cm = g. 10000m – 940 m =
h. (4.5 x 105 km)(3.00 x 103km) i. 2.005 cm x 5.0 cm =
j. 120km2 8.56 km =
k. 0.005600mm3 0.200 mm2=
5. Round the following number to the indicated number of significant figures: 604.503792
a. 5 ________ e. 1 ________
b. 3 ________ f. 4 ________
c. 2 ________ g. 6 ________
d. 7________ h. 8 ________
6. Which students’ data is more precise? Explain your answer.
Student 1: 72.75g, 73.34g, 73.02g, 73.25g Student 2: 72.01g, 71.99g, 72.00g 71.98g
7. What is the volume of a board that measures 1.8cm by 8.8 cm by 30.5 cm?
Honors Chemistry Problem Set – Chapter 3B Scientific Measurement
Use dimensional analysis to convert all of the following units. Show your work and make sure your answer has the correct number of significant figures.
Prefix conversions:
1. 750 x 103 ng to g 6. 15.0 mm to km
2. 65 g to kg 7. 13455 mg to kg
3. 14 mm to m 8. 7.5 x 104 nm to km
4. 57.0 mL to L 9. 0.0982 dg to cg
5. 88.0 m/sec to cm/sec
Complex Units (converting top and bottom) and Squared or Cubed Units
1. 0.06 m2 to cm2 6. 4.52 g/mL to kg/L
2. 1.467 km3 to m3 7. 64.8 m/s to km/hr
3. 23.6 ft2 to cm2 8. 88 m/sec to mm/cs
4. 952 g/L to g/mm3 9. 35.8 mi/hr to m/s
5. 0.02580 km2 to m2 10. 0.024kg/cm3 to mg/mL
Mixed Conversions, Word Problems - The following table of densities may useful for the following problems.
1. What is the mass of 3.55 mL of mercury?
2. What is the mass of 0.045L of lead?
3. A particle moving through a gas at a speed of 45.8 m/s strikes one wall of a container, bounces off and hits the other wall 25.0 cm away. How long did it take to go from one wall to the other?
4. Which of the following has the greater volume.: 25.0g of copper or 25.0 g of lead?
5. Which has the greater mass: 25cm3 of copper or 25cm3Al?
6. Which of the following has the greater volume: 15.0g of copper or 15.0g of gold?
7. A rock has a mass of 127 g and displaces 32.1 mL of water. What is the density of the rock in g/cm3?
8. A block measures 0.52 cm by 1.67 cm by 0.30cm. It has a mass of 0.469g. What is the density of the block? Will it float in water?
9. What is the volume of 42.00g of gold?
10. What is the density of a piece of concrete that has a mass of 8.76g and a volume of 3.07 cm3?
11. Illegal ivory is sometimes detected on the basis of density. What is the density of a sample of ivory whose volume is 14.5cm3 and whose mass is 26.8 g?
12. What is the minimum volume of a tank that can hold 795kg of methanol?
13. What is the volume of 7.62g of ammonium magnesium chromate?
14. Which would be heavier a ball of lead or iron, assume equal volumes.
15. A solid block of aluminum, with a mass of 200.0g is placed in a a beaker of water that is full to the brim. How much water will overflow out of the beaker?
16. How many moles of NaNO3 are in 35.6g of a 25.0% solution of NaNO3? The molar mass of NaNO3 is 85.0g/mol.
17. The heat of solution for NaOH is 50.6 kJ/mol. How much heat is released when 50.0g of NaOH are dissolved in water. The molar mass of NaOH is 40.0g/mol.
18. A solution of BaCl2 has a concentration of 3.2 mol/L. How many liters of solution are needed to obtain 0.42 mol of BaCl2?
Answers to problems:
Prefix Conversions:
1. 7.5 x 10-4g 2. 0.065 kg 3. 0.014 m 4. 0.0570 L
5. 8.80 x 103 cm/sec 6. 1.50 x 10-5 km 7. 0.013455 kg 8. 7.5 x 10-8 km 9. 0.982 cg
Complex Units:
1. 600 cm2 2. 1.467 x 109 m3 3. 21900 cm2
4. 9.52 x 10-4 g/mm3 5. 2.580 x 104 m2 6. 4.52 kg/L 7. 233 km/hr 8. 880 mm/cs
9. 16.0 m/s Mixed Conversions, Word Problems:
1. 48.3 g Hg
2. 510 g
3. 0.00552sec
7. 3.96 g/cm3 8. 1.8 g/cm3 9. 2.18 mL 10. 2.85 g/cm3 11. 1.85 g/cm3 12. 1.01 x 106 cm3
Substance Denstiy
g/cm3 Substance Densityg/cm3
Aluminum 2.70 Water 1.00
Copper 8.96 Limestone 2.72
Gold 19.3 Calcium chloride 2.50
Lead 11.4 Methanol 0.788
Mercury 13.6 Ammonium Magnesium Chromate 1.84
Iron 7.87
13. 4.14 cm3 14. see me 15. 74.1 mL 16. .105 mol 17. 63.3 kJ 18. 0.13 L or 130 mL
Honors Chemistry: Unit 1 Review
1. Describe each of the following statements as qualitative or quantitative.
a. The time is now 7:00 p.m.
b. It is cold outside.
c. It’s getting late.
d. The temperature is four degrees Fahrenheit.
2. Jim has 2.00 x 103 marbles. Bill has 3.00 x 102 marbles. Who has more marbles, Jim or Bill?
3. One mile equals 1609 meters. Express this measurement using scientific notation.
4. An oval track is 400 meters long. Express this measurement using scientific notation.
5. Add the answers to problems 3 and 4 and express the product using scientific notation.
6. Multiply the answers to problems 3 and 4 and express the product using scientific notation.
7. a. Bruce’s three measurements are 19 cm, 20 cm, and 22 cm. Calculate the average value of his measurements and express the answer with the correct number of significant figures.
b. Pete’s there measurements are 20.9 cm, 21.0 cm and 21.0 cm. Calculate the average value of his measurements and express the answer with the correct number of significant figures.
c. Whose measurements are more precise?
d. The actual length of the object is 20 cm. Whose measurements are more accurate.
e. What is the percent error of Pete’s average measurement?
Use the density chart from your book to answer the following questions 9,10, &11.
8. What is the mass at 20.0C of five liters of air?
9. What is the mass of a bar of aluminum measuring 1.0cm by 1.0 cm by 10.0cm?
10. An object measuring 4.0 cm by 2.5 cm by 5.0 cm has a mass of 110 g. What is the density of the object?
11. Which of the following is not a physical change?
a. dissolving sugar in water c. evaporating sea water to obtain salt b. burning gasoline in an engine d. slicing a piece of bread 12. Which of the following is not a property of a gas?
a. has a definite shape c. assumes the shape of its container b. has no definite volume d. easily compressible
13. Which of the following is not a physical property of sucrose?
a. solid at room temperature c. dissolves in water b. decomposes when heated d. tastes sweet
14. Which of the following is typically in a different physical state than the other three at room temperature?
a. salt b. sugar c. flour d. water
15. Complete the following table:
Physical state Definite shape? Definite volume? Readily compressible?
Gas
No no
Yes 16. What is a homogeneous mixture?
17. Label each of the following mixtures as homogeneous or heterogeneous.
a. gasoline b. chunky peanut butter
c. oil and vinegar salad dressing d. orange soda 18. Label each at a pure substance or a mixture.
a. ethanol b. vinegar
c. motor oil d. helium
19. What elements make up chloroform (CHCl3) and how many atoms of each element are present?
20. Classify the following as elements, compounds or mixtures.
a. salt b. water c. iron d. sterling silver
21. A liquid is allowed to evaporate and leaves no residue. Is it possible to determine whether it was an element, compound or mixture?
22. Which of the following in not an element?
a. copper b. sulfur c. ammonia d. helium 23. Which of the following is a chemical change?
a. gasoline boils c. gasoline burns
b. lead is added to gasoline d. gasoline is poured into a tank 24. Classify each of the following changes as physical or chemical.
a. dew is dried by the sun c. grape juice is converted to wine b. a dark cloth is faded by the sunlight d. soap is dissolved in water
25. In the chemical reaction carbon dioxide plus water carbonic acid.
a. what does the arrow stand for b. name the products
c. name the reactants
d. If 44g of carbon dioxide react completely with 18g of water, what is the mass of carbonic acid formed?
26. In an engine, octane combines with oxygen to form carbon dioxide and water. If 22.8g of octane combine completely with 80 g of oxygen to form 70.4 g of carbon dioxide, what mass of water is formed?
27. Which chemical law allows you to answer questions 25d and 26?
28. A liquid is allowed to evaporate and leaves no residue. Is it possible to determine whether it was an element, compound or mixture?
29. A typical freezer keeps food at 277K. What is this temperature in degrees Celsius?
30. Use dimensional analysis to make the following conversions. Show all work!!!
a) 157 cs to sec b) 42.7 L to mL c) 261 nm to mm d) 642 cg to kg
e) 8.25 x 102 cg to ng f) 0.44 mL/min to L /sec g) 7386 g /cm2 to mg/ mm2 h) 1.53 kg/ L to g/cm3 i) 1.00 min to nsec
31. Match the project to one of the 5 branches of chemistry.
___________a. Determine the composition of a moon rock sample.
___________b. Do research on making a new medicine for high blood pressure.
___________c. Investigate chemical methods for regulating the rate of gasoline burning in an automobile engine.
___________d. Develop a biodegradable plastic.
___________e. Work on improving the method for making stainless steel.
32. A student performs an experiment and fine that the results do not agree with theory. Is something wrong with the students experiment? Explain.
33. Criticize the statement, “Theories are proven by experiments.”
34. Use dimensional analysis to solve the following problems:
a. The heat of fusion of water is 46.0 KJ per mole and the molar mass of water is 18.0 g per mole. How much water can be melted with 893.5KJ of heat?
b. The enthalpy of combustion of octane( C8H18) is 1245.7 KJ/mole how much energy(KJ) will be released when 0.200g of octane is combusted? The density of octane is 0.840 g/mL and the molecular weight of octane is 146.0 g/mole.
c. How many grams of KCl are in 47.0mL of a solution that is 5.2molesKCl/L? The molar mass of KCl is 66.60g/mol.
d. What is the mass of 2.3L of nitrogen? The density of nitrogen is 0.00125g/mL.
Honors Chemistry Lecture Notes: Calculations with Significant Figures Determining the number of Sig figs in a measurement
Pacific Atlantic Method for Significant Figures
** If the decimal is Present….approach the number from the Pacific. Go to the first non-zero digit; that and every number to the right of it is significant.
** If the decimal is Absent…approach the number from the Atlantic. Go to the first non-zero digit;
that and every number to the left of it is significant.
Together:
a) 40.7L b) 97.00kg c) 32,006 m
You Try!
a) 1200.00 cm3
b) 1200 cm3 c) 0.0572m2 d) 3400 g e) .00002 g f) 4000. mL Counting Sig Figs
a. 30,040g ______ b. 0.0008m ______ c. 20.900cm ______
d. 1500mg ______ e. 640 cm3 ______ f. 1500.mg ______
g. 10,000L ______ h. 20.05mL ______ i. 0.05200g ______
j. 0.663 g ______ k. 0.000056g/L ______ l. 5.6 M ______
Rounding to correct sig figs
50,600.0675 mL
Calculations made with Significant Figures:
Perform the following operations on your calculator, report the answer to the correct number of sig figs.
a. 11.075 g / 12.7 mL = e. 5.430 g / 1.82 L =
b. 140 cm x 35 cm= f. 47.0 m /2.2 s =
c. 22.0 cm + 5.28 cm +15.5 cm = g. 50.0 cm x 2.0 cm=
d. 2450 dl + 4.30 dL +10.2 dL = h. 0.003L +0.0045 L + 0.100 Rules for Sig Fig’s in Calculations:
When multiplying and dividing: The answer can only have the number of significant figures as the measurement with the least number of sig figs
When adding and subtracting: The answer can only have the number of significant decimal places as the measurement with the least number of significant decimal places.
a. 1 __________ e. 5 __________
b. 2 __________ f. 6 __________
c. 3 __________ g. 7 __________
d. 4 __________ h. 8 __________
Factor Label Method/ Dimensional Analysis Practice
Conversion Factors:
Equivalent measures:
Problems:
1-Step Conversions - base unit is either what you are starting with or ending with 1. Convert 3500.0 mg to g
2. Convert 0.649L to kL 3. Convert 84345.6 m to m 4. Convert 57 mL to L
5. Convert 88 m/sec to cm/sec 6. Convert 4.52 g/mL into kg/L
2-Step Conversions- base unit is not present in answer or given …. Given Base unknown 1. Convert 0.462mg to kg
2. Convert 880000 dm to Mm 3. Convert 0.00674 kL to mL 4. Convert 62.80km/hr into cm/hr
Squared or cubed Units - Conversion factors must be squared or cubed as well 1. Convert 800.4 m3 to cm3
2. Convert 88.46 m2 to km2
Complex Units: converting top and bottom of fraction …Given Convert top (1 or more steps) Convert bottom (1 or more steps)
1. Convert 74 m/s into km/hr 2. Convert 4.06 cm/hr into mm/sec 3. Convert 0.470 kg/L into mg/mL
4. Convert 8.24 dollars/ yd2 to cents/ft2 Mixed-
1. Convert mm2 to m2 5. Convert 88 km/hr to m/s
2. Convert 420 mg to kg 6. Convert 0.0456 m2/sec to dm2/min 3. Convert 0.0000910 g to g 7. Convert 0.0056 kcal to cal
4. Convert 56.03 dL to L 8. Convert 450 g/cm3 to g/m3
10. The density of lead is 11.3 g/ml. What is the mass of 45 mL of the metal?
11. A particle moves through a gas at a speed of 15 km/s. How far will it move in 5.5 s?
12. A sample of seawater contains 6.277 g of sodium chloride per liter of solution. How many mg of sodium chloride would be contained in 15.0 mL of this solution?
13. A sample of seawater contains 0.00245 g of sodium chloride per ml of solution. How much sodium chloride is contained in 50.0 mL of this solution?
14. Amount of heat given off when water condenses is 254kJ/mol. The molecular weight of water is 18.0g/mol. How much heat (kJ) is given off when 15.0 grams of water condenses?
15. A photon of visible light has a wavelength of 4000.0 Å. How many wavelengths will pass a point in 3.0 seconds? ( 1 Å = 1 x 10-10m ; speed of light 3.00 x 108 m/s )
