Solutions for CHM 101 VOL 1 2014 >IC<
Problem 1DE:
One of the important ideas of thermodynamics is that energy can be transferred in the form of heat...Problem 1E:
Two positively charged spheres, each with a charge of 2.0x10-5 C, a mass of 1.0 kg, and separated by...Problem 2E:
SI The accompanying photo shows a pipevine swallowtail caterpillar climbing up a twig. As the...Problem 3E:
Consider the accompanying energy diagram. Does this diagram represent an increase or decrease in the...Problem 4E:
The contents of the closed box in each of the following illustrations represent a system, and the...Problem 5E:
Imagine that you are climbing a mountain. Is the distance you travel to the top a state function? Is...Problem 6E:
The diagram shows four states of a system, each with different internal energy, E. Which of the...Problem 7E:
You may have noticed that when you compress the air in a bicycle pump, the body of the pump gets...Problem 8E:
Imagine a container placed in a tub of water, as depicted in the accompanying diagram. If the...Problem 9E:
In the accompanying cylinder diagram, a chemical process occurs at constant temperature and...Problem 11E:
Consider the two diagrams that follow. Based on (i), write an equation showing how HA is related to...Problem 12E:
Consider the conversion of compound A into compound B: A-)B. For both compounds A and A and...Problem 13E:
What is the electrostatic potential energy (in joules) between an electron and a proton that we...Problem 14E:
What is the electrostatic potential energy (in joules) between two protons that are separated by 62...Problem 15E:
The electrostatic force (not energy) of attraction between two oppositely charged objects is given...Problem 16E:
Use the equations given in Problem 5.15 to calculate: The electrostatic force of repulsion for two...Problem 17E:
A sodium ion, Na+, with a charge of 1.6 x 10-19 C and a chloride ion, Cl2, with charge of - 1.6 x...Problem 18E:
A magnesium ion, Mg2+, with a charge of 3.2 x 10-19 C and an oxide ion, 02 , with a charge of - 3.2...Problem 19E:
Identify the force present and explain whether work is being performed in the following cases: You...Problem 20E:
Identify the force present and explain whether work is done when a positively charged particle moves...Problem 21E:
Which of the following cannot leave or enter a closed system: heat, work, or matter? Which cannot...Problem 23E:
According to the first law of thermodynamics, what quantity is conserved? What is meant by the...Problem 24E:
Write an equation that expresses the first law of thermodynamics in terms of heat and work. Under...Problem 25E:
Calculate AB and determine whether the process is endothermic or exothermic for the following cases:...Problem 26E:
For the following processes, calculate the change in internal energy of the system and determine...Problem 27E:
A gas is confined to a cylinder fitted with a piston and an electrical heater, as shown here:...Problem 28E:
Consider a system consisting of two oppositely charged spheres hanging by strings and separated by a...Problem 29E:
What is meant by the term state function? Give an example of a quantity that is a state function and...Problem 30E:
Indicate which of the following is independent of the path by which a change occurs: the change in...Problem 31E:
During a normal breath, our lungs expand about 0.50 L against an external pressure of 1.0 atm. How...Problem 32E:
How much work (in J) is involved in a chemical reaction if the volume decreases from 5.00 to 1.26 L...Problem 33E:
Why is the change in enthalpy usually easier to measure than the change in internal energy? H is a...Problem 34E:
Under what condition will the enthalpy change of a process equal the amount of heat transferred into...Problem 35E:
Assume that the following reaction occurs at constant pressure: 2 Al(s) + 3 Cl2(g)2 AlCl3(s) If you...Problem 36E:
Suppose that the gas-phase reaction 2NO(g) + 02(g) 2NO2(g) werecarried out in a constant-volume...Problem 37E:
A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in Figure 5.4...Problem 38E:
A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in Figure 6.4....Problem 39E:
The complete combustion of ethanol, C2H5OH(l), to formH20(g) and CO2{g) at constant pressure...Problem 40E:
The decomposition of Ca(OH)2(s) into CaO(s) and H20(g) at constant pressure requires the addition of...Problem 41E:
Ozone, 03(9), is a form of elemental oxygen that plays an important role in the absorption of...Problem 42E:
5.42 Without referring to tables, predict which of the following has the higher enthalpy in each...Problem 43E:
Consider the following reaction: 2 Mg(s) + 02(g)2 MgO(s) H-1204 kJ Is this reaction exothermic or...Problem 44E:
544 Consider the following reaction:
2 CH3OH(g)→2CH4 (g) + 02(g) = + 252.8 kJ
a. Is this reaction...Problem 45E:
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates Ag+...Problem 46E:
At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat...Problem 47E:
5.47 Consider the combustion of liquid methanol, CH3011(l):
CH3OH(l) O2(g)→ CO2(g)+ 2H2O(1)
= -...Problem 48E:
5.48 Consider the decomposition of liquid benzene,C6H6(l) to gaseous acetylene, C2H2(g):
C6 H 6...Problem 49E:
5.49
a What are the units of molar heat capacity?
What are the units of specific heat?
If you know...Problem 50E:
Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of...Problem 51E:
What is the specific heat of liquid water? What is the molar heat capacity of liquid water? What is...Problem 52E:
5.52
a. Which substance in Table 5.2 requires the smallest amount of energy to increase the...Problem 53E:
The specific heat of octane, C8H18(l), is 2.22 J/g-K. How many J of heat are needed to raise the...Problem 54E:
6.54 Consider the data about gold metal in Exercise 5.26(b).
a. Based on the data, calculate the...Problem 55E:
When a 6-50-g sample of solid sodium hydroxide dissolves in 100 0 g of water in a coffee-cup...Problem 56E:
5.56
a. When a 4 25-g sample of solid ammonium nitrate dissolves in 60 0 g of water in a coffee-cup...Problem 57E:
A 2.200-g sample of quinone (C5H402) is burned in a bomb calorimeter whose total heat capacity is...Problem 58E:
8.68 A 1.800-g sample of phenol (C6H5OH) was burned in a bomb calorimeter whose total heat capacity...Problem 59E:
Under constant-volume conditions, the heat of combustion of glucose (C6H12O6) is 15.57kJ/g. A 3...Problem 60E:
5.60 Under constant-volume conditions, the heat of combustion of benzoic acid (C6H5COOH) is 26.38...Problem 61E:
5.61 Can you use an approach similar to Hess's law to calculate the change in internal energy, E,...Problem 63E:
Calculate the enthalpy change for the reaction P4O6(s) + 2 O2(g) -P4O10(s) given the following...Problem 65E:
From the enthalpies of reaction Calculate H for the reaction of ethylene with F2: C2H4(g) + 6 F2(g)...Problem 67E:
5.67
What is meant by the term standard conditions with reference to enthalpy changes?
What is...Problem 68E:
S
5.68
What is the value of the standard enthalpy of formation of an element in its most stable...Problem 69E:
For each of the following compounds, write a balanced thermochemical equation depicting the...Problem 70E:
Write balanced equations that describe the formation of the following compounds from elements in...Problem 71E:
The following is known as the thermite reaction: 2A1(s) + Fe2O3(s)Al2O3(s) + 2Fe(s) This highly...Problem 72E:
5.72 Many portable gas heaters and grills use propane, C3H8(g), as a fuel. Using standard...Problem 73E:
Using values from Appendix C , calculate the standard enthalpy change for each of the following...Problem 74E:
5.74 Using values from Appendix C, calculate the value of 24H° for each of the following...Problem 75E:
Complete combustion of 1 mol of acetone (C2H6O) liberates 1790 kJ: C3H6O(l) + 4O2(g) 3CO2(g) +...Problem 76E:
Calcium carbide (CaC2) reacts with water to form acetylene (C2H2) and Ca(OH)2. From the following...Problem 77E:
5.77 Gasoline is composed primarily of hydrocarbons, including many with eight carbon atoms,...Problem 79E:
Ethanol (C2H5OH) is blended with gasoline as an automobile fuel. Write a balanced equation for the...Problem 80E:
5.80 Methanol (CH3OH) is used as a fuel in race cars.
Write a balanced equation for the...Problem 82E:
5.82 Without doing any calculations, predict the sign of for each of the following reactions:
2...Problem 83E:
Use bond enthalpies in Table 5.4 Q to estimate for each of the following reactions: a. H - H(g) + Br...Problem 84E:
Use bond enthalpies in Table 5.40 to estimate for each of the following reactions: a. b.Problem 85E:
Use enthalpies of formation given in Appendix C to calculate for the reaction Br2(g) 2 Br(g), and...Problem 86E:
5.86
The nitrogen atoms in an N2 molecule are held together by a triple bond; use enthalpies of...Problem 87E:
5.87 Consider the reaction 2H(g) + O2(g) 2H2O(l)
Use the bond enthalpies in Table 5.4 to...Problem 88E:
5.88 Consider the reaction H2(g) + I2(s) 2HI(g).
Use the bond enthalpies in Table 5.4 to...Problem 89E:
5.89
What is meant by the term fuel value?
Which is a greater source of energy as food, 5 g of fat...Problem 90E:
5.90
Which releases the most energy when metabolized, 1 g of carbohydrates or 1 g of fat?
A...Problem 91E:
5.91
A serving of a particular ready-to-serve chicken noodle soup contains 2.5 g fat, 14 g...Problem 92E:
5.92 A pound of plain M&M® candies contains 96 g fat, 320 g carbohydrate, and 21 g protein. What...Problem 93E:
5.93 The heat of combustion of fructose, C6H12O6, is — 2812kJ/mol. If a fresh golden delicious...Problem 94E:
5.94 The heat of combustion of ethanol, C2H5OH(l), is — 1367Wmol. A batch of Sauvignon Blanc wine...Problem 95E:
5.95 The standard enthalpies of formation of gaseous propyne (C3H4), propylene (C3H6), and propane...Problem 96E:
5.98 It is interesting to compare the ‘fuel value’ of a hydrocarbon in a hypothetical world where...Problem 97E:
At the end of 2012, global population was about 7.0 billion people. What mass of glucose in kg would...Problem 98E:
5.98 The automobile fuel called E85 consists of 85% ethanol and 15% gasoline. E85 can be used in...Problem 99AE:
The air bags that provide protection in automobiles in the event of an accident expand because of a...Problem 100AE:
5.100 An aluminum can of a soft drink is placed in a freezer. Later, you find that the can is...Problem 101AE:
5.101 Consider a system consisting of the following apparatus, in which gas is confined on one...Problem 102AE:
A sample of gas is contained in a cylinder-and-piston arrangement it undergoes the change in state...Problem 103AE:
Limestone stalactites and stalagmites are formed in caves by the following reaction: Ca2+ (aq)...Problem 104AE:
Consider the systems shown in Figure 5.10. In one case the battery becomes completely discharged by...Problem 105AE:
5.105 A house is designed to have passive solar energy features. Brickwork incorporated into the...Problem 106AE:
5.108 A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.1...Problem 107AE:
5.107
When a 0.235-9 sample of benzoic acid is combusted in a bomb calorimeter (Figure 5.19), the...Problem 108AE:
5.108 Meals-ready-to-eat (MREs) are military meals that can be heated on a flameless heater. The...Problem 109AE:
5.109 Burning methane in oxygen can produce three different carbon-containing products: soot (very...Problem 111AE:
5.111 From the following data for three prospective fuels, calculate which could provide the most...Problem 112AE:
The hydrocarbons acetylene (C2H2) and benzene (C6H6) have the sum empirical formula. Benzene is an...Problem 113AE:
Ammonia (NH3) boils at -33 °C; at this temperature it has a density of 0.81 g/cm3. The enthalpy of...Problem 114AE:
5.114 Three common hydrocarbons that contain four carbons are listed here, along with their...Problem 115AE:
5.115 A 201-lb man decides to add to his exercise routine by walking up three flights of stairs (45...Problem 116AE:
5.116 TheSun supplies about 1.0 kilowatt of energy for each square meter of surface area (
1.0...Problem 117AE:
5.117 Itis estimated that the net amount of carbon dioxide fixed by photosynthesis on the landmass...Problem 118IE:
5.118 At 20 °C (approximately room temperature) the average velocity of N2molecules in air is 1050...Problem 119IE:
Suppose an Olympic diver who weighs 52.0 kg executes a straight dive from a 10-m platform. At the...Problem 120IE:
5.120 Consider the combustion of a single molecule of CH4 (g), forming H20(l) as a product.
How...Problem 121IE:
5.121 Consider the following unbalanced oxidation-reduction reactions in aqueous solution:
Ag+(aq)...Problem 122IE:
Consider the following acid-neutralization reactions involving the strong base NaOH(aq): HNO3(aq) +...Problem 123IE:
5.123 Consider two solutions, the first being 50.0 mL of 1.00 MCuSO4 and the second 50.0 mL of...Problem 124IE:
The precipitation reaction between AgNO3(aq) and NaCl(aq) proceeds as follows: AgNO3(aq)...Problem 125IE:
5.125 A sample of a hydrocarbon is combusted completely in O2(g) to produce 21.83 g CO2(g), 4.47 g...Browse All Chapters of This Textbook
Chapter 1 - Introduction: Matter, Energy, And MeasurementChapter 1.2 - Classifications Of MatterChapter 1.5 - Units Of MeasurementChapter 1.6 - Uncertainty In MeasurementChapter 1.7 - Dimensional AnalysisChapter 2 - Atoms, Molecules, And IonsChapter 2.3 - The Modern View Of Atomic StructureChapter 2.4 - Atomic WeightsChapter 2.5 - The Periodic TableChapter 2.6 - Molecules And Molecular Compounds
Chapter 2.7 - Ions And Ionic CompoundsChapter 2.8 - Naming Inorganic CompoundsChapter 2.9 - Some Simple Organic CompoundsChapter 3 - Chemical Reactions And Reaction StoichiometryChapter 3.1 - Chemical EquationsChapter 3.2 - Simple Patterns Of Chemical ReactivityChapter 3.3 - Formula WeightsChapter 3.4 - Avogadro's Number And The MoleChapter 3.5 - Empirical Formulas From AnalysesChapter 3.6 - Quantitative Information From Balanced EquationsChapter 3.7 - Limiting ReactantsChapter 4 - Reactions In Aqueous SolutionChapter 4.1 - General Properties Of Aqueous SolutionsChapter 4.2 - Precipitation ReactionsChapter 4.3 - Acids, Bases, And Neutralization ReactionsChapter 4.4 - Oxidation-reduction ReactionsChapter 4.5 - Concentrations Of SolutionsChapter 4.6 - Solutions Stoichiometry And Chemical AnalysisChapter 5 - ThermochemistryChapter 5.2 - The First Law Of ThermodynamicsChapter 5.3 - EnthalpyChapter 5.4 - Enthalpies Of ReactionChapter 5.5 - CalorimetryChapter 5.6 - Hess's LawChapter 5.7 - Enthalpies Of FormationChapter 5.8 - Bond EnthalpiesChapter 5.9 - Foods And FuelsChapter 6 - Electronic Structure Of AtomsChapter 6.1 - The Wave Nature Of LightChapter 6.2 - Quantized Energy And PhotonsChapter 6.3 - Line Spectra And The Bohr ModelChapter 6.4 - The Wave Behavior Of MatterChapter 6.5 - Quantum Mechanics And Atomic OrbitalsChapter 6.8 - Electron ConfigurationsChapter 6.9 - Electron Configurations And The Periodic TableChapter 7 - Periodic Properties Of The ElementsChapter 7.3 - Sizes Of Atoms And IonsChapter 7.4 - Ionization EnergyChapter 7.6 - Metals, Nonmetals, And MetalloidsChapter 7.7 - Trends Of Group 1a And Group 2a MetalsChapter 8 - Basic Concepts Of Chemical BondingChapter 8.2 - Ionic BondingChapter 8.3 - Covalent BondingChapter 8.4 - Bond Polarity And ElectronegativityChapter 8.5 - Drawing Lewis StructuresChapter 8.6 - Resonance StructuresChapter 8.7 - Exceptions Of The Octet RuleChapter 9 - Molecular Geometry And Bonding TheoriesChapter 9.2 - The Vsepr ModelChapter 9.3 - Molecular Shape And Molecular PolarityChapter 9.5 - Hybrid OrbitalsChapter 9.6 - Multiple BondsChapter 9.7 - Molecular OrbitalsChapter 9.8 - Bonding In Period 2 Diatomic MoleculesChapter 10 - GasesChapter 10.2 - PressureChapter 10.3 - The Gas LawsChapter 10.4 - The Ideal-gas EquationChapter 10.5 - Further Applications Of The Ideal-gas EquationChapter 10.6 - Gas Mixtures And Partial PressuresChapter 10.7 - The Kinetic-molecular Theory Of GasesChapter 10.8 - Molecular Effusion And DiffusionChapter 10.9 - Real Gases: Deviations From Ideal BehaviorChapter 11 - Liquids And Intermolecular ForcesChapter 11.2 - Intermolecular ForcesChapter 11.3 - Select Properties Of LiquidsChapter 11.4 - Phase ChangesChapter 11.5 - Vapor PressureChapter 11.6 - Phase DiagramChapter 11.7 - Liquid CrystalsChapter 12 - Solids And Modern MaterialsChapter 12.3 - Metallic SolidsChapter 12.5 - Ionic SolidChapter 12.7 - Covalent-network SolidsChapter 13 - Properties Of SolutionsChapter 13.3 - Factor Affecting SolubilityChapter 13.4 - Expressing Solution ConcentrationChapter 13.5 - Colligative PropertiesChapter 14 - Chemical KineticsChapter 14.2 - Reaction RatesChapter 14.3 - Concentration And Rate LawsChapter 14.4 - The Change Of Concentration With TimeChapter 14.5 - Temperature And RateChapter 14.6 - Reaction MechanismsChapter 15 - Chemical EquilibriumChapter 15.2 - The Equilibrium ConstantChapter 15.3 - Understanding And Working With Equilibrium ConstantChapter 15.4 - Heterogeneous EquilibriumChapter 15.5 - Calculating Equilibrium ConstantsChapter 15.6 - Applications Equilibrium ConstantsChapter 15.7 - Le Chatelier's PrincipleChapter 16 - Acid—base EquilibriumChapter 16.2 - Bronsted-lowery Acids And BasesChapter 16.3 - The Autoionization Of WaterChapter 16.4 - The Ph ScaleChapter 16.5 - Strong Acids And BasesChapter 16.6 - Weak AcidsChapter 16.7 - Weak BasesChapter 16.8 - Relation Between Ka And KbChapter 16.9 - Acid-base Properties Of Salt SolutionChapter 16.10 - Acid-base Behavior And Chemical StructureChapter 17 - Additional Aspects Of Aqueous EquilibriumChapter 17.1 - The Common Ion EffectChapter 17.2 - BuffersChapter 17.3 - Acid-base TitrationsChapter 17.4 - Solubility EquilibriaChapter 17.5 - Factor That Affect SolubilityChapter 17.6 - Precipitation And Separation Of IonsChapter 18 - Chemistry Of The EnvironmentChapter 18.1 - Earth's AtmosphereChapter 18.2 - Human Activities And Earth AtmosphereChapter 19 - Chemical ThermodynamicsChapter 19.1 - Spontaneous ProcessesChapter 19.2 - Entropy And Second Law Of ThermodynamicsChapter 19.3 - The Molecular Interpretation Of Entropy And The Third Law Of ThermodynamicsChapter 19.4 - Entropy Changes In Chemical ReactionsChapter 19.5 - Gibbs Free EnergyChapter 19.6 - Free Energy And TemperatureChapter 19.7 - Free Energy And Equilibrium ConstantChapter 20 - ElectrochemistryChapter 20.1 - Oxidation States And Oxidation-reduction ReactionsChapter 20.2 - Balancing Redox EquationsChapter 20.3 - Voltaic CellsChapter 20.4 - Cell Potentials Under Standard ConditionsChapter 20.5 - Free Energy And Redox ReactionsChapter 20.6 - Cell Potentials Under Nonstandard ConditionsChapter 20.9 - ElectrolysisChapter 21 - Nuclear ChemistryChapter 21.1 - Radioactivity And Nuclear EquationsChapter 21.2 - Patterns Of Nuclear StabilityChapter 21.3 - Nuclear TransmutationsChapter 21.4 - Rates Of Radioactive DecayChapter 21.6 - Energy Changes In Nuclear ReactionsChapter 22 - Chemistry Of The NonmetalsChapter 22.1 - Periodic Trends And Chemical ReactionsChapter 22.3 - Group 8a:the Noble GasesChapter 22.4 - Group 7a:the HalogensChapter 22.7 - NitrogenChapter 22.10 - The Other Group 4a:elements:si,ge,sn And PbChapter 23 - Transition Metals And Coordination ChemistryChapter 23.2 - Transition-metals ComplexesChapter 23.4 - Nomenclature And Isomerism In Coordination ChemistryChapter 23.5 - Color And Magnetism In Coordination ChemistryChapter 23.6 - Crystal-field TheoryChapter 24 - The Chemistry Of Life: Organic And Biological ChemistryChapter 24.2 - Introduction To HydrocarbonsChapter 24.3 - Alkenes,alkynes,and Aromatic HydrocarbonsChapter 24.4 - Organic Functional GroupsChapter 24.7 - Proteins
Sample Solutions for this Textbook
We offer sample solutions for CHM 101 VOL 1 2014 >IC< homework problems. See examples below:
The figure (i) represents the space filling molecular models of two spheres attached to each other...The sign of the electric charge on the particle is negative in the given diagram. This experiment...Chapter 3, Problem 1EGiven The three salts are named as sodium sulfide, sodium bicarbonate and sodium chloride. The...Chapter 5, Problem 1DEChapter 6, Problem 1DEThe alkali metals such as rubidium and cesium which has lower first ionization energies can be used...The heat of hydrogenation of acetylene is −1299.53 kJ/mol and the fuel value of 3.0 mol acetylene is...The energy absorbed by the given compound is calculated by the formula, Energy=Plank's...
The given unknown gas is a noble gas and the difference in molar masses of noble gases is much...The force of attraction between the hydrogen and an electronegative atom is called hydrogen bonding....Explanation: The given polymer is first dissolved in the buffer solution. The experiment is...According to Raoult’s law, the vapor pressure of a solution is equal to the product of the mole...Given The chemical equation for the given hypothetical reaction is, aA+bB→cC+dD The reactants...Explanation: The spectrometer is a device which splits light into the array of separate colors which...If the solution is acidic, it changes blue litmus paper into red and there is no change in color for...Explanation: The concentration of NaOH solution is calculated by considering the small volume of the...Explanation: The chemicals involved in fracking operations are hydrochloric acid, sodium chloride,...The relation between the standard free energy change, standard entropy change and standard enthalpy...GivenThe electrical potential output of the cell is 1.50 V . The external device draws the current...Explanation: Pitchblende is a uranium ore with excess amount of UO2 , on oxidation UO2 leads to the...The physical state of the substance depends upon the size of the substance. The size of the atoms...The reaction of the given coordination compound with the solution of AgNO3 solution gives the...Explanation: The buffer solution of hemoglobin is prepared first. This buffer solution of hemoglobin...
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18th Edition
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17th Edition
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14th Edition
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17th Edition
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14th Edition
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17th Edition
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14th Edition
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14th Edition
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14th Edition
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14th Edition
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14th Edition
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14th Edition
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14th Edition
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14th Edition
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Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: The Central Science (14th Edition)
14th Edition
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Student Solutions Manual to Red Exercises for Chemistry: The Central Science
14th Edition
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Chemistry The Central Science
14th Edition
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CHEMISTRY: THE CENTRAL SCIENCE
14th Edition
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Pearson eText Chemistry: The Central Science -- Access Card
14th Edition
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CHEMISTRY: W/MASTERING CHEMISTRY
13th Edition
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19th Edition
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14th Edition
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14th Edition
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AP* Chemistry: The Central Science (NASTA Edition)
14th Edition
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MASTERING CHEMISTRY ACCESS W/ETEXT
18th Edition
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MASTERING CHEMISTRY NEW DESIGN FOR CHE
1st Edition
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14th Edition
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13th Edition
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Laboratory Experiments for Chemistry: The Central Science (14th Edition)
14th Edition
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CHEMISTRY:CENTRAL..-MOD.MASTERING (18W)
14th Edition
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19th Edition
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Solutions To Exercises To Accompany Chemistry: The Central Science, 11th Edition. 9780136003250, 0136003257.
11th Edition
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Chemistry: The Central Science
11th Edition
ISBN: 9780136006176
Chemistry: The Central Science: AP Edition
11th Edition
ISBN: 9780136018797
Chemistry: The Central Science : Study Guide
6th Edition
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LAB EXPERIMENTS FOR CHEM >C<
6th Edition
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EBK CHEMISTRY
15th Edition
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Chemistry: The Central Science (chart)
9th Edition
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Chemistry The Central Science Volume 2 For Chem 112
9th Edition
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Chemistry: The Central Science
9th Edition
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Chemistry: The Central Science - Black
9th Edition
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Ap Chemistry: The Central Science
9th Edition
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Chemistry (spanish Translation) (9th Edition)
9th Edition
ISBN: 9789702604686
Chemistry: The Central Science
9th Edition
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