Honors Chemistry Spring Exam Review 1
Process Skills
1. How many significant figures do the following numbers have? a. 3.14 - three b. 0.00831 - three c. 1000 - one d. 100.100 - six e. 3410 - three
2. How many significant figures would the following answers have? a. 13.3 x 2.4 x 13 = two b. 1200 x 12.00 x 0.00310 = two
Stoichiometry
3. Covert the following from grams to moles. a. 42.8 g F (1.0 mol F/19.00 g) = 2.3 moles b. 10.0g H2O (1.0 mol H2O/18.02 g H2O) = 0.55 moles H2O c. 34.54g H2SO4 (1.0 mol H2SO4/98.09 g H2SO4) = 0.35 moles H2SO4
4. Convert moles to grams a. 2.35 mol NH3 (17.04 g NH3/1.0 mol NH3) = 40. g NH3 b. 17.3 mol H2O (18.02 g H2O/1.0 mol H2O) = 310 g H2O c. 56.58 mol KNO3 (101.11 g KNO3/1.0 mol KNO3) = 5700 g KNO3
5. Define stoichiometry. – (p. 354) The study of quantitative relationships between the amounts of reactants used and products formed by a chemical reaction.
6. Define limiting reactant. – (p.364) A reactant that is totally consumed during a chemical reaction, limits the extent of the reaction, and determines the amount of the product.
7. What is stated in the law of conservation of mass? Mass is neither created nor destroyed during a chemical reaction but is conserved.
8. What are the molar masses of the following compounds? a. CO2 = 44.01 g/mol b. NH3 = 17.04 g/mol c. H2O = 18.02 g/mol d. CH4 = 16.05 g/mol e. H3PO4 = 98.00 g/mol
9. Where are the reactants located in an equation? Products? Reactants are located on the left side of the arrow, and products are located on the right side.
10. What do the coefficients represent in a balanced equation? In a balanced equation, coefficients represent the number of particles of the substance involved in the reaction.
11. Balance the following equations. a. Fe (s) + O2 (g)  Fe2O3 (s) - 4Fe (s) + 3O2 (g) 
2Fe2O3 (s) b. N2 (g) + H2 (g)  NH3 (g) - 1N2 (g) + 3H2 (g)  2NH3
(g) c. C3H8 (g) + O2 (g)  CO2 (g) + H2O (g) - 1C3H8 (g) + 5O2 (g)
 3CO2 (g) + 4H2O (g)
12. How many moles of H2O will be produced if 10.3 moles of O2 reacts with excess H2?
2H2 + O2  2H2O
10.3 mol O2 (2 mol H2O /1 mol O2) = 20.6 moles H2O
13. If 23.2 grams of bromine reacts with excess lead, how many moles of lead bromide would be produced?

Pb + 2Br2  PbBr4
23.2 g Br2 (1 mol Br2/159.8 g Br2)(1 mol PbBr4/2 mol Br2) = .0726 mol PbBr4
14. 4.32 moles of aluminum react with excess chlorine to produce how many grams of aluminum chloride?
2Al + 3Cl2  2AlCl3
4.32 mol Al (2 mol AlCl3/2 mol Al)(133.33 g AlCl3/1 mol AlCl3) = 576 g
AlCl3
15. How many grams of NO2 would be created if 23.45 grams of nitrogen react with excess grams of oxygen?
N2 + 2O2  2NO2
23.45 g N2 (1 mol N2/28.02 g N2)(2 mol NO2/1 mol N2)(46.01 g NO2/1 mol
NO2) = 77.01 g NO2
16. If 30.0 grams of AgCl reacts with 30.0 grams BaI2 how many grams of
AgI will be produced? Which reactant is limiting? Which reactant is excess? How much excess remains?
2AgCl + BaI2  BaCl2 + 2AgI
30.0 g AgCl (1 mol AgCl/143.32 g AgCl)(2 mol AgI/2 mol AgCl)(234.77 g
AgI/1 mol AgI) = 49.14 g AgI
30.0 g BaI2 (1 mol BaI2 /391.13 g BaI2)(2 mol AgI/1 mol BaI2)(234.77 g
AgI/1 mol AgI) = 36.01 g AgI
49.14 g AgI – 36.01 g AgI = 13.13 g AgI
Theoretically, 36.01 g AgI will be produced. Limiting reactant – BaI2.
Excess reactant – AgCl with 13.13 g remaining.
17. If 32.13g sodium reacts with 20.33g of hydrochloric acid (HCl) how many grams of sodium chloride will be produced? Which reactant is limiting? Which reactant is excess? How much excess remains?
2Na + 2HCl  2NaCl + H2
32.12 g Na (1 mol Na/22.99 g Na)(2 mol NaCl/2 mol Na)(58.44 g NaCl/1 mol
NaCl) = 81.65 g NaCl
20.33 g HCl (1 mol HCl/36.46 g HCl)(2 mol NaCl/2 mol HCl)(58.44 g NaCl/1 mol NaCl) = 32.59 g NaCl
81.65 g NaCl – 32.59 g NaCl = 49.06 g NaCl
Theoretically, 32.59 g NaCl should be produced. Limiting reactant – HCl.
Excess reactant – Na with 49.06 g remaining.
18. In an experiment, 30.00 grams NaHCO3 decomposed and produced 17.33 grams of Na2CO3. What is the percent yield of Na2CO3?
2NaHCO3  Na2CO3 + CO2 + H2O
30.00 g NaHCO3 (1 mol NaHCO3/84.01 g NaHCO3)(1 mol Na2CO3/2 mol
NaHCO3)(105.99 g Na2CO3/1 mol Na2CO3) = 18.92 g Na2CO3 percent yield = (actual/theoretical) x 100 = (17.33 g Na2CO3/18.92 g
Na2CO3) x 100 = 91.60%
19. 50.3 grams of NH3 was produced in an experiment when 10.00 grams of hydrogen reacted with excess nitrogen. What is the percent yield of NH3?
N2 + 3H2  2NH3
10.00 g H2 (1 mol H2/2.02 g H2)(2 mol NH3/3 mol H2)(17.04 g NH3/1 mol NH3)
= 56.24 g NH3
(50.30/56.24) = 89%
Solutions
Use the solubility curve provided to answer the following questions
20. Which substance’s solubility is most affected by temperature? KNO3
21. How many grams of KCl will dissolve in 100g of water at 45C? approximately 40 g KCl.
22. If 20g of KClO3 is added to 100g of water at 30C, what type

of solution is created: saturated, unsaturated, or supersaturated? saturated.
23. If 70g of NaNO3 is placed into 100g of water at 40C and all of the solute is dissolve, what type of solution is created: saturated, unsaturated, or supersaturated? unsaturated.
24. If 50g NaCl dissolves in 100g H2O, how much NaCl dissolves in 50g
H2O? 25g NaCl.
25. What is the relationship between temperature and solid solubility?
Solids are more soluble at high temperatures. Temperature and gas solubility? Gases are less soluble at high temperatures.
26. What is the formula and unit for Molarity? M = moles of solute/liters of solution. Is it regularly used in science? It is one of the most common units of solution concentration.
27. If you dissolve 52g of salt in 102g of water, what is the percent concentration?
52g NaCl(1 mol NaCl/58.44 g NaCl) = .89 mol NaCl. 102g H2O(1 mol
H2O/18.02g H2O)(22.4 L H2O/1 mol H2O) = 127L H2O
M = moles of solute(.89 moles NaCl)/liters of solution(127L H2O) = .0070M
28. What substance is known as the universal solvent? Water.
29. What do colligative properties depend on? The word colligative means “depending on the collection.”
30. Fill in the following chart using your knowledge of suspensions, colloids, and solutions:
Tyndall effect (yes or no) Settles out
(yes or no) What method can be used to separate it?
Suspensions
yes yes settling or filtration
Colloid
yes no destroying the Brownian motion (one can do this in ways such as adding an electrolyte to the colloid or heating the colloid up).
Solution no no, but they do separate in immiscible solutions in immiscible solutions, one can merely wait for the process of separation to take place.
31. Define the following terms: a. Aqueous – a solution in which a solvent is in water b. Soluble – describes a substance that can be dissolved in a given solvent c. Insoluble – describes a substance that cannot be dissolved in a given solvent d. Immiscible – describes two liquids that can be mixed together but separate shortly after you cease mixing them e. Miscible – describes two liquids that are soluble in each other f. Solvation – the process of surrounding solute particles with solvent particles to form a solution g. Saturated – contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure h. Unsaturated – contains less dissolved solute for a given temperature and pressure than a saturated solution i. Supersaturated – contains more dissolved solute than a saturated solution at the same temperature j. Solvent – the substance that dissolves a solute to form a solution k. Solute – a substance dissolved in a solution l. Electrolyte – an ionic compound whose aqueous solution conducts an electric current

Enthalpy
32. Contrast an endothermic reaction vs. exothermic reaction.
Endothermic reactions require more energy to occur than they release; exothermic reactions require less energy to occur than they release.
33. Define specific heat. The amount of heat required to raise the temperature of one gram of a gien substance by one degree Celsius. What is it for water? 4.184 J/g•˚C
34. Define each of the following three terms and describe their relationship to each other: kinetic energy, heat, and temperature.
Kinetic energy: energy of motion.
Heat: a form of energy that flows from a warmer object to a cooler object.
Temperature: a measure of the average kinetic energy of the particles in a sample of matter.
Temperature measures the kinetic energy, which is what causes the flow of heat.
35. What is entropy and how is it affected by the state of matter
(solid, liquid, or gas)? A measure of the disorder of randomness of the particles of a system. The molecules of a solid are in a rigid, orderly arrangement, causing low entropy. The molecules of a liquid have more freedom, causing higher entropy. The molecules of a gas are completely separated and free, causing an extremely high entropy.
36. How much energy in joules is required to change 48.0g of water 16ºC?
(c = 4.184 j/gºC)?
Q = c x m x T. q = 4.184 j/g•ºC x 48.0g x 16ºC = 3200 J
37. How much energy in calories is needed to raise the temperature of
10.4g of water from 22ºC to 41ºC? (c = 1.0cal/gºC) q = 1. 0cal/gºC x 10.4g x 19ºC = 197.6 calories
38. A 25g piece of metal at 225ºC is placed in a calorimeter with 100. mL of water at 22ºC. If the final temperature was 25ºC the specific heat of the metal would be 0.06 cal/g•ºC. (hint: will take 2 steps)
100 mL H2O = 50 g H2O q = c m t. q = 1.0 cal/g•ºC x 100 g x 3ºC. q of water = 1.0 cal/ g•ºC
-300 cal = c x m x t. = c x 25g x -200ºC. c of metal = 0.06 cal/g•ºC.
39. How much energy in Calories is needed to raise the temperature of
50.0g of water from 22ºC to 41ºC when a 7.5g peanut is burned? What is the heat of combustion (Cal/g)? (c = 1.0cal/gºC)
Q = cmt. Q = 1.0cal/g•ºC x 7.5 g x 19ºC = 140 Cal.
140/7.5 = 19 Cal/g.
Equilibrium/Kinetics
40. What is necessary to start a chemical reaction? (Be Specific!!)
41. Describe and explain 4 ways to speed up a chemical reaction.
42. What is a catalyst and how does it work?
Acids/Bases
43. For the properties below, identify as an acid, base, or neutral a. pH <7 - acid b. pH >7 - base c. pH 7 - neutral d. bitter - base e. sour - acid f. HCl - acid g. NaOH - base h. proton donor - acid i. OH- donor - base j. household cleaner - base

k. vinegar - acid l. turns litmus paper red - acid m. turns litmus paper blue - base
44. What are the reactants and products involved in a neutralization reaction? The reactants are a base and an acid, and the products are a salt and water.
45. Contrast the Arrhenius Theory with the Bronsted-Lowry Theory. The
Arrhenius Theory defines an acid as a substance that contains hydrogen and a base as a substance that contains a hydroxide group. The Bronsted-Lowry defines an acid as a hydrogen-ion donor and a bass as a hydrogen-ion acceptor.
46. Describe the pH of rain and how it affects the environment. Most rainwater has a pH of 5.6 to 5.8. When the value is below 5.8, the rainwater is considered acid rain. Plants, animals, and even humans experience negative effects from acid rain.
47. Define the following terms: a. endpoint – the point in which the indicator changes color b. indicator – a chemical dye whose color is affected by acidic and basic solutions c. neutralization – a reaction in which an acid and a base react in aqueous solution to produce a salt and water d. titration – the process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration e. buffer – a solution that resists changes in pH when limited amounts of acid or base are added
Gases
48. Describe the properties of gas. Fast-moving particles, assumes the shape and volume of container, compressible, flows easily, lots of free space between particles, particles move past one another.
49. Describe the make up of air. 78% nitrogen, 21% oxygen, 1% argon,
.03% carbon dioxide, and the rest is trace gases.
50. Describe what is said in the kinetic molecular theory. The particles do not attract or repel each other. The particles are much smaller than the distances between them. The particles are in constant, random motion. No kinetic energy is lost when the particles collide with each other or with the walls of their container. Al gases have the same average kinetic energy at a given temperature.
51. What is STP and the values that are represented by it? The Standard
Temperature and Pressure at sea level. It is 1.00 atm pressure, 0.00 degrees Celcius, and 22.4 L.
52. What do we call 0 Kelvin; what is going on if a substance is 0 K?
It is the coldest temperature possible, known as “absolute zero.” At this temperature, al matter has stopped.
53. List all the names and formulas of the gas laws learned in class.
Boyle’s Law: PV=K.
Charles’ Law: V/T=K.
Gay-Lussac’s Law: P/T=K.
Combined Gas Law: (P1V1)/T1=(P2V2)/T2
Ideal Gas Law: PV=nRT or N=PV/RT
54. What is the relationship between temperature and volume? They vary directly.
55. What happens to atmospheric pressure as you go up a mountain? It decreases.
56. Compare ideal gases vs. real gases.

Ideal gases have particles that take up no space and have no intermolecular attractive forces. It follows the gas laws under conditions of temperature and pressure.
Real gases have particles with volume and intermolecular interactions.
Because of this, gas laws do not always provide exact measurements in the real world.
57. At what temperature will 5.00 g of Cl2 exert a pressure of 900 torr at a volume of 750 mL?
5.00 g Cl2 (1 mol Cl2/70.90 g Cl2) = .0705 mol Cl2
PV=nRT
(900 torr)(0.750 L)=(.0705 mol)(T)(64.2)
T = 149 degrees K
58. A sample of oxygen gas occupies a volume of 250 mL at 740 torr pressure. What volume will it occupy at 800 torr pressure?
P1V1 = P2V2
.25L x 740 torr = L x 800 torr
L = .23L oxygen
59. A sample of nitrogen occupies a volume of 250 mL at 25&#61616; C.
What volume will it occupy at 95&#61616; C?
V1/T1 = V2/T2
.25L/298 = V2/368
V2 = .31L nitrogen
60. A sample of carbon dioxide occupies a volume of 3.50 liters at 125 kPa pressure. What pressure should the gas exert if the volume was decreased by 2.00 liters.
P1V1 = P2V2
(3.5L)(125kPa)=(P)(2.00L)
P = 220 kPa
61. Helium occupies a volume of 3.8 liters at -45&#61616; C. What volume will it occupy at 45&#61616; C?
V1/T1 = V2/T2
3.8/228=V2/318
V2 = 5.3L helium
62. What volume will 2.0 moles of nitrogen occupy at 720 torr and
20&#61616; C?
PV=nRT
(720)(V)=(2.0)(293)(64.2)
52L nitrogen
63. What is air pressure at sea level? 1 atm pressure.
64. Gases diffuse. What is diffusion? The movement of one material through another from an area of higher concentration to an area of lower concentration.
65. How do you find total pressure? You add each individual pressure together.