Chemistry and Chemical Reactivity (Inst...10th EditionKotz Publisher: CENGAGE LISBN: 9781337399180
Chemistry and Chemical Reactivity (Inst...
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Chapter 1 - Basic Concepts Of ChemistryChapter 1.5 - CompoundsChapter 1.6 - Physical PropertiesChapter 1.7 - Physical And Chemical ChangesChapter 1.8 - Energy: Some Basic PrinciplesChapter 2 - Atoms Molecules And IonsChapter 2.1 - Atomic Structure, Atomic Number, And Atomic MassChapter 2.2 - Isotopes And Atomic WeightChapter 2.5 - Ionic Compounds: Formulas, Names, And PropertiesChapter 2.6 - Atoms, Molecules, And The Mole
Chapter 2.7 - Chemical Analysis: Determining Compound FormulasChapter 2.8 - Instrumental Analysis: Determining Compound FormulasChapter 3 - Chemical ReactionsChapter 3.2 - Balancing Chemical EquationsChapter 3.4 - Aqueous SolutionsChapter 3.5 - Precipitation ReactionsChapter 3.6 - Acids And BasesChapter 3.7 - Gas-forming ReactionsChapter 3.8 - Oxidation-reduction ReactionsChapter 3.9 - Classifying Reactions In Aqueous SolutionChapter 4 - Stoichiometry: Quantitative Information About Chemical ReactionsChapter 4.1 - Mass Relationships In Chemical Reactions: StoichiometryChapter 4.2 - Reactions In Which One Reactant Is Present In Limited SupplyChapter 4.4 - Chemical Equations And Chemical AnalysisChapter 4.5 - Measuring Concentrations Of Compounds In SolutionChapter 4.6 - Ph, A Concentration Scale For Acids And BasesChapter 4.7 - Stoichiometry Of Reactions In Aqueous Solution-fundamentalsChapter 4.8 - Stoichiometry Of Reactions In Aqueous Solution-titrationsChapter 4.9 - SpectrophotometryChapter 5 - Principles Of Chemical Reactivity: Energy And Chemical ReactionsChapter 5.2 - Specific Heat Capacity: Heating And CoolingChapter 5.3 - Energy And Changes Of StateChapter 5.4 - The First Law Of ThermodynamicsChapter 5.5 - Enthalpy Changes For Chemical ReactionsChapter 5.6 - CalorimetryChapter 5.7 - Enthalpy CalculationsChapter 5.8 - Product- Or Reactant-favored Reactions And ThermodynamicsChapter 6 - The Structure Of AtomsChapter 6.1 - Electromagnetic RadiationChapter 6.2 - Quantization: Planck, Einstein, Energy, And PhotonsChapter 6.3 - Atomic Line Spectra And Niels BohrChapter 6.4 - Particle-wave Duality: Prelude To Quantum MechanicsChapter 6.7 - One More Electron Property: Electron SpinChapter 7 - The Structure Of Atoms And Periodic TrendsChapter 7.3 - Electron Configuration Of AtomsChapter 7.4 - Electron Configuration Of IonsChapter 7.5 - Atomic Properties And Periodic TrendsChapter 7.6 - Periodic Trends And Chemical PropertiesChapter 8 - Bonding And Molecular StructureChapter 8.2 - Covalent Bonding And Lewis StructuresChapter 8.3 - Atom Formal Charges In Covalent Molecules And IonsChapter 8.4 - ResonanceChapter 8.5 - Exceptions To The Octet RuleChapter 8.6 - Molecular ShapesChapter 8.7 - Electronegativity And Bond PolarityChapter 8.8 - Molecular PolarityChapter 8.9 - Bond Properties: Order, Length, And Dissociation EnthalpyChapter 8.10 - Dna, RevistedChapter 9 - Bonding And Molecular Structure: Orbital Hybridization And Molecular OrbitalsChapter 9.1 - Valence Bond TheoryChapter 9.2 - Molecular Orbital TheoryChapter 9.3 - Theories Of Chemical Bonding: A SummaryChapter 10 - Gases And Their PropertiesChapter 10.1 - Modeling A State Of Matter: Gases And Gas PressureChapter 10.2 - Gas Laws: The Experimental BasisChapter 10.3 - The Ideal Gas LawChapter 10.4 - Gas Laws And Chemical ReactionsChapter 10.5 - Gas Mixtures And Partial PressuresChapter 10.6 - The Kinetic-molecular Theory Of GasesChapter 10.7 - Diffusion And EffusionChapter 10.8 - Nonideal Behavior Of GasesChapter 11 - Intermolecular Forces And LiquidsChapter 11.2 - Interactions Between Ions And Molecules With A Permanent DipoleChapter 11.3 - Interactions Between Molecules With A Permanent DipoleChapter 11.4 - Intermolecular Forces Involving Nonpolar MoleculesChapter 11.5 - A Summary Of Van Der Waals Intermolecular ForcesChapter 11.6 - Properties Of LiquidsChapter 12 - The Solid StateChapter 12.1 - Crystal Lattices And Unit CellsChapter 12.2 - Structures And Formulas Of Ionic SolidsChapter 12.6 - Phase ChangesChapter 13 - Solutions And Their BehaviorChapter 13.1 - Units Of ConcentrationChapter 13.2 - The Solution ProcessChapter 13.3 - Factors Affecting Solubilitiy: Pressure And TemperatureChapter 13.4 - Colligative PropertiesChapter 13.5 - ColloidsChapter 14 - Chemical Kinetics: The Rates Of Chemical ReactionsChapter 14.1 - Rates Of Chemical ReactionsChapter 14.3 - Effect Of Concentration On Reaction RateChapter 14.4 - Concentration-time Relationships: Integrated Rate LawsChapter 14.5 - A Microscopic View Of Reaction RatesChapter 14.7 - Reaction MechanismsChapter 15 - Principles Of Chemical Reactivity: EquilibriaChapter 15.2 - The Equilibrium Constant And Reaction QuotientChapter 15.3 - Determining An Equilibrium ConstantChapter 15.4 - Using Equilibrium Constants In CalculationsChapter 15.5 - More About Balanced Equations And Equilibrium ConstantsChapter 15.6 - Disturbing A Chemical EquilibriumChapter 16 - Principles Of Chemical Reactivity: The Chemistry Of Acids And BasesChapter 16.2 - Water And Ph ScaleChapter 16.4 - Acid-base Properties Of SaltsChapter 16.5 - Predicting The Direction Of Acid-base ReactionsChapter 16.7 - Calculations With Equilibrium ConstantsChapter 16.8 - Polyprotic Acids And BasesChapter 16.10 - The Lewis Concept Of Acids And BasesChapter 17 - Principles Of Chemical Reactivity: Other Aspects Of Aqueous EquilibriaChapter 17.1 - The Common Ion EffectChapter 17.2 - Controlling Ph: Buffer SolutionsChapter 17.3 - Acid-base TitrationsChapter 17.4 - Solubility Of SaltsChapter 17.5 - Precipitation ReactionsChapter 17.6 - Equilibria Involving Complex IonsChapter 18 - Principles Of Chemical Reactivity: Entropy And Free EnergyChapter 18.3 - Entropy Measurement And ValuesChapter 18.4 - Entropy Changes And SpontaneityChapter 18.6 - Calculating And Using Standard Free Energies, Δfg˚Chapter 18.7 - The Interplay Of Kinetics And ThermodynamicsChapter 19 - Principles Of Chemical Reactivity: Electron Transfer ReactionsChapter 19.1 - Oxidation-reduction ReactionsChapter 19.2 - Simple Voltaic CellsChapter 19.4 - Standard Electrochemical PotentialsChapter 19.5 - Electrochemical Cells Under Nonstandard ConditionsChapter 19.6 - Electrochemistry And ThermodynamicsChapter 19.7 - Electrolysis: Chemical Change Using Electrical EnergyChapter 19.8 - Counting ElectronsChapter 19.9 - Corrosion: Redox Reactions In The EnvironmentChapter 20 - Environmental Chemistry-earth's Environment, Energy, And SustainabilityChapter 20.7 - Green Chemistry And SustainabilityChapter 21 - The Chemistry Of The Main Group ElementsChapter 21.2 - The Periodic Table: A Guide To The ElementsChapter 21.11 - The Noble Gases, Group 8aChapter 22 - The Chemistry Of The Transistion ElementsChapter 22.4 - Coordination CompoundsChapter 22.5 - Structures Of Coordination CompoundsChapter 22.6 - Bonding In Coordination CompoundsChapter 22.7 - Colors Of Coordination CompoundsChapter 23 - Carbon: Not Just Another ElementChapter 23.2 - HydrocarbonsChapter 23.3 - Alcohols, Ethers, And AminesChapter 23.4 - Compounds With A Carbonyl GroupChapter 23.5 - PolymersChapter 24 - BiochemistryChapter 24.1 - ProteinsChapter 24.3 - Nucleic AcidsChapter 24.5 - MetabolismChapter 25 - Nuclear ChemistryChapter 25.2 - Nuclear Reactions And Radioactive DecayChapter 25.3 - Stability Of Atomic NucleiChapter 25.4 - Rates Of Nuclear DecayChapter 25.5 - Artifical Nuclear ReactionsChapter 25.8 - Applications Of Nuclear Chemistry
Sample Solutions for this Textbook
We offer sample solutions for Chemistry and Chemical Reactivity (Instructor's) homework problems. See examples below:
Chapter 1, Problem 1PSChapter 1, Problem 21RPSIn 1.52, the decimal numbers with no zeroes and has only the significant numbers. So, the...In 6.25×102, can be written as 625 has no decimal numbers with no zeroes and has only the...Chapter 1, Problem 28RPSChapter 1, Problem 43RGQChapter 1, Problem 54RGQChapter 1, Problem 62RGQThe average value and the standard deviation is calculated as, SD=∑|x−μ|2Nwhere, x is values in the...
Atoms are made of three subatomic particles such as neutrons, protons and electrons. In which, the...Chapter 2, Problem 43PSChapter 2, Problem 44PSChapter 2, Problem 80PSConversion formula for number moles of an atom into mass, Number of moles ×Molar mass = Mass in...(a) 3.79×1024 atoms Fe Equation for finding number of atoms from number of moles of an atom, Number...Chapter 2, Problem 122GQThe molar mass of the given compound is as follows, Molecular formula of the given compound is...Chapter 2, Problem 124GQChapter 2, Problem 126GQChapter 2, Problem 128GQIn ClF3 compound, both elements are nonmetals, so it is a molecular compound. Electronegativity of...Chapter 2, Problem 131GQChapter 2, Problem 133GQChapter 2, Problem 153GQChapter 2, Problem 154GQChapter 2, Problem 156GQThe product of the reaction, balancing of the reaction and the type of the reaction is shown below,...Chapter 3, Problem 1PSChapter 3, Problem 20PSChapter 3, Problem 24PSThe given compound is lead nitrate and potassium bromidewhich is soluble in water. In this reaction...Chapter 3, Problem 63PSChapter 3, Problem 64PSThe soluble compound contains bromide ion is shown below NaBr, KBr or other alkali metal bromides...Chapter 3, Problem 70GQChapter 3, Problem 81GQChapter 3, Problem 83GQChapter 4, Problem 1PSChapter 4, Problem 17PSChapter 4, Problem 45PSChapter 4, Problem 46PSChapter 4, Problem 82GQBalanced chemical equation for the given reaction is, 2 NaIO3(aq) + 5 NaHSO3(aq) → 3 NaHSO4(aq) +2...Chapter 4, Problem 92GQChapter 4, Problem 103GQChapter 4, Problem 109GQChapter 4, Problem 118GQThe amount of hydrochloric acid in 50.0 mL of 0.100 M HCl can be determined as follows, Amount of...Chapter 4, Problem 125ILHerein two iron compounds are given (a) K[Fe(C2O4)2 (H2O)2] (b) K3[Fe(C2O4)3] To find which one is...Chapter 4, Problem 136SCQChapter 5, Problem 1PSChapter 5, Problem 57PSChapter 5, Problem 58PSChapter 5, Problem 81GQGiven, ΔfH0(C) = 0 KJ/mol ΔfH0(H2O) =-241.8kJ/mol ΔfH0(CO) =-110.54kJ/mol ΔfH0(H2) =0J/mol Enthalpy...For isooctane the balanced reaction is C8H18+ 25/2 O2→ 8 CO2+ 9 H2O ΔrH0=ΣnΔfH0(products) -...For N2H4 the balanced equation is: N2H4+ O2→ N2+ 2H2O ΔrH0=ΣnΔfH0(products) - ΣnΔfH0(reactants)...Chapter 5, Problem 89GQTo show the net result is the decomposition of water. Equation 1-2 =A A=CaBr2 + H2O +Hg → CaO +...Chapter 5, Problem 110SCQChapter 5, Problem 111SCQChapter 5, Problem 115SCQThe energy of a photon of line in the yellow region with wavelength 5.89 × 10−7 m and 5.8959 × 10−7...Chapter 6, Problem 1PSChapter 6, Problem 34PSChapter 6, Problem 54GQChapter 6, Problem 57GQChapter 6, Problem 62GQChapter 6, Problem 67GQChapter 6, Problem 68GQChapter 6, Problem 69GQThe atomic number of technetium is 43. The electronic configuration is [Kr]4d55s2. Here Tc has 5...Electronic configuration of Gadolinium (Gd) elements filling method is shown below. (Gd) is located...Chapter 7, Problem 1PSLet us consider the orbital filling method of Strontium (Sr) 1. The spdf and orbital box notations,...The electron configuration is, Atomic number of Plutonium (Pu) =94Complete (spdf) notation of (Pu) =...Chapter 7, Problem 21PSLet us consider the orbital filling method of Sodium (Na+) ions. Given the Sodium atom has loss of...Chapter 7, Problem 25PSChapter 7, Problem 43GQElectronic configuration for Cerium (Ce) system: Atomic number of Cerium (Ce) =58Complete (spdf)...Chapter 7, Problem 49GQChapter 8, Problem 1PSChapter 8, Problem 15PSChapter 8, Problem 16PSThe Lewis electron dot structure for given molecules are determined by first drawing the skeletal...Chapter 8, Problem 24PSChapter 8, Problem 33PSChapter 8, Problem 41PSThe structure of BCl3 is, This molecule has a trigonal planar geometry. The direction dipole in the...Chapter 8, Problem 73GQChapter 8, Problem 97SCQChapter 9, Problem 1PSChapter 9, Problem 8PSChapter 9, Problem 26PSThere are 13 valence electrons in ClO molecule. In accordance with the MO theory, the electron...Chapter 9, Problem 28PSChapter 9, Problem 42GQChapter 9, Problem 46GQMolecular orbital diagram of (CN) molecule can be drawn as σ*2pz −−−− → (Anti bonding electrons) −−...Chapter 10, Problem 1PSChapter 10, Problem 39PSChapter 10, Problem 40PSChapter 10, Problem 41PSChapter 10, Problem 57GQGiven, Before mixing He ArV 3.0 L 2.0 LP 145 mm Hg 335 mm Hg The partial pressure for the given...Chapter 10, Problem 89GQThe balanced chemical equation for the reaction of the two given gases with HCl is as follows,...Chapter 10, Problem 105ILThe given reactants C3H8(g) and O2(g) reacts in order to give set of products like CO2(g) and...Chapter 10, Problem 107SCQThe given compound ClO2 contains two oxygen atoms and one chlorine atom. The atomic number of oxygen...In water molecules the hydrogen bond in ice are linear and have strong directional property, this...Chapter 11, Problem 21PSGiven: Temperature oCVapor Pressure mm Hg2513.65045.375127.2100310.8 Temperatures and corresponding...Chapter 11, Problem 38GQThe normal boiling point of dichlorodimethylsilane is calculated Given: Temperature (K)Vapour...The major reason behind this observation is hydrogen bonding The electronegativity difference...Given: ln P 1/T 2.300.003693.690.003424.610.003255.990.002976.630.00285 From the given data we can...Number of atoms per unit is given below, It has 8 atoms in the corner, 6 atom in the face, 4 atoms...Chapter 12, Problem 1PSThe phase diagram of CO2 is given below, Figure 1 When seeing the phase diagram of CO2, the density...The energy can be calculated by using following formula, q = m × c × ΔT Mass (m) = 12.0 Kgc = 4.7...Chapter 12, Problem 50GQChapter 12, Problem 51GQGiven,partial pressure of CO2 = 4 barHenry's constant = 0.034 mol/kg.barAccording to Henry's law, Sg...Chapter 13, Problem 1PSCalculate mole fraction of NaI: Given data: Molality = 0.15 mol/ kg 0.15 moles of NaI is in 1Kg of...Calculate molality of KNO3: Given data: Weight percent = 10.0 Weight percent = 10.0 indictaes 10g of...Given, Mass of phenylalanine is 3% = 3100 × 100 g = 3 g Mass of solvent is 100 g − 3 g = 97 g =...Given, Given mass of NaCl is 1130 g Given mass of ice is 7250 g = 7.25 kg Weight percentage of NaCl...Chapter 13, Problem 57GQChapter 13, Problem 58GQChapter 13, Problem 79GQChapter 13, Problem 91ILGiven, measured ΔTfp for NaCl= −3.050Cmeasured ΔTfp for Na2SO4= −1.360C Kfp = −1.860C/m Mass of NaCl...The number of moles of any substance can be determined using the equation Number of mole =Given mass...Chapter 14, Problem 1PSChapter 14, Problem 11PSChapter 14, Problem 12PSChapter 14, Problem 13PSChapter 14, Problem 14PSChapter 14, Problem 59GQGiven information, The reaction is 2 H2O2(aq) → 2 H2O(l) + O2(aq) [H2O2](mol/L)Initial Reaction Rate...Chapter 14, Problem 82GQChapter 14, Problem 89ILChapter 14, Problem 90ILChapter 15, Problem 1PSChapter 15, Problem 40GQChapter 15, Problem 53GQChapter 15, Problem 54GQChapter 15, Problem 55GQChapter 15, Problem 56GQChapter 15, Problem 62GQChapter 15, Problem 63GQChapter 16, Problem 1PSChapter 16, Problem 8PSChapter 16, Problem 39PSChapter 16, Problem 40PSChapter 16, Problem 73PSChapter 16, Problem 75PSChapter 16, Problem 76PSChapter 16, Problem 94GQThe oxalic acid is a diprotic acid. It ionizes into two steps. H2C2O4(aq) + H2O(l)⇌HC2O4-(aq) +...An equilibrium constant (K) is the ratio of the concentration of products and reactants raised to...Chapter 16, Problem 114ILA lewis acid can accept a pair of electrons from a lewis base. The boron in BF3 is electron poor and...Chapter 16, Problem 129SCQChapter 17, Problem 1PSChapter 17, Problem 27PSChapter 17, Problem 28PSChapter 17, Problem 30PSChapter 17, Problem 33PSChapter 17, Problem 60PSSolubility product constant Ksp for AgCN is 6.0×10−17. AgCN dissociates as follows in water,...Chapter 17, Problem 82GQThe value of equilibrium constant, Knet for the given reaction is calculated below. Given: Refer to...Chapter 17, Problem 105ILChapter 17, Problem 106ILChapter 17, Problem 107ILChapter 18, Problem 1PSChapter 18, Problem 20PSChapter 18, Problem 33PSChapter 18, Problem 34PSChapter 18, Problem 39PSChapter 18, Problem 40PSChapter 18, Problem 58GQChapter 18, Problem 76GQChapter 18, Problem 90SCQThe formula for hydrazine is N2H4. It reacts with oxygen to produce water and N2. The balanced...The ΔSo (system) for the reaction is calculated below. Given: Refer to Appendix L for the values of...Chapter 19, Problem 1PSChapter 19, Problem 3PSChapter 19, Problem 4PSChapter 19, Problem 5PSThe given reaction is s follows. Fe(OH)3(s) + Cr(s) →Cr(OH)3(s) + Fe(OH)2(s) Oxidation states:...Chapter 19, Problem 19PSThe given table: Half reactionEo(V)MnO4-(aq)+ 8H+5e- →Mn2+(aq)+4H2O(l)BrO3-(aq)+ 6H+ + 6e-...Chapter 19, Problem 58GQChapter 19, Problem 63GQLet’s write the reduction potential of each of the following non-metal ions. F2+2e- →2F- ; E0= +...Chapter 19, Problem 105ILChapter 19, Problem 110ILReason for the correct answer: In atmosphere there are different types of air in different...Given, Treatment of sea water with Ca(OH)2 gives insoluble Mg(OH)2. This reacts with HCl to produce...When methyl myristate is burned the gas CO2 and H2O are produced as the products. The balanced...Given: From the table 8.8, the average bond energy of C-Cl bond is 339 kJ/mol In-order to find the...Given the combustion of ethanol and isooctane: EthanolC2H5OH (l) +3 O2 (g) → 2CO2 (g) + 3H2O (l)...If the concentration of dissolved CO2 is increased, then the pH will be decreased as a result of the...Chapter 21, Problem 1PSAcidic oxides are generally oxides of non-metals of group VAand VIAmetals. The two examples of...Sodium belongs to group 1A of periodic table and has an oxidation number of +1. Thus, it loses one...Potassium belongs to group 1A of periodic table and has an oxidation number of +1. Thus, it loses...The ΔrG°,ΔrH° and ΔrS° for the given reaction is calculated below. Given: Refer to Appendix L for...Chapter 21, Problem 45PSIf the value of standard Gibbs free energy of reaction (ΔrG∘) is positive then the reaction is...The mass of H2O and O2 produced in the decomposition of ammonium perchlorate is calculated below....Any metal M reacts with hydrogen chloride to give metal halide and hydrogen. The chemical equation...The iodine atom belongs to group 17 in the periodic table. The outer electronic configuration of...The balanced chemical equation between NH2N(CH3)2 and N2O4 is written as,...Chapter 21, Problem 107GQThe ΔrG∘ for the reaction of silver with hydrogen halide is calculated below. Given: Refer to...Probable equation for the given reaction can be written as follows, Fe(aq)2+ + [Ce(NO3)6](aq)2− →...Chapter 22, Problem 1PSThe oxidation state of central metal atom Ni is 2+. Dichloro means there are two Cl ions whereas...The oxidation state of central metal atom Cr is 2+. Di means there are two ions whereas means tri...The Ligands are arranged in an alphabetical order, followed by the metal name (nickel). There are...Chapter 22, Problem 31PSThe oxidation state of central metal atom Cr is 3+. Tetra means there are four ions or molecule...Examining the given complex shows that Fe serves as the central metal atom since it is surrounded by...Examining the given complex shows that Fe serves as the central metal atom since it is surrounded by...Examining the given complex shows that Zn serves as the central metal atom since it is surrounded by...Carbon is bonded via four single bonds to adjacent atoms. Carbon is bonded with four single four...Carbon is bonded via four single bonds to adjacent atoms. Carbon is bonded with four single four...The given isomer is 2,2-dimethylhexane From the name it is clear that: The parent name is hexane for...The given alcohol is, The longest chain has three carbon atoms so parent chain will be propane. The...The systematic name of given alcohol is 1-butanol. The longest chain will have four carbon atoms as...The molecular formula of the given amine can be written by using its given name ethylamine. The...Chapter 23, Problem 48PSCompound 1 s, It is a ketone The reaction between compound 1 and NaBH4 is the reduction reaction of...Chapter 23, Problem 85GQThe structure of the given compound is drawn below. There is longest carbon chain is five carbon...From the given data, 2-amino benzoic acid = 4.0 gMolar mass of 2-amino benzoic acid =137.14 g/mol...Let’s write the balanced equation of combustion of ethane: 2C2H6(g) + 7O2(g) → 4CO2(g) + 3H2O(l)...Assuming the molecular formula of the compound is CxHyOz. It dissociates into carbondioxide and...Chapter 24, Problem 1PSThe value of ΔrH° for the given oxidation reaction of one mole of glucose is calculated below....Chapter 24, Problem 24PSThe value of ΔrH° for the production of one mole of glucose by the process of photosynthesis at...The Ratemax for the given reaction is calculated below, Given: The substare concentration and...The alpha particle has highest mass when compared to Beta and Gamma particles because the Alpha...The radioactive isotope of iron-54 when irradiated with alpha particle forms 2856Ni by the emission...The bombardment of unknown particle with Beryllium-9, produce an Helium nuclei particle...Given incomplete nuclear reaction is, 47111 Ag → 48111 Cd + ? 47111 Ag Undergoes nuclear reaction,...Given incomplete nuclear reaction is, 1019 Ne→ +10 β + ? This reaction is completed by the emission...The radioactive decay series beginning with Th-232 and ending with Pb-208 is as follows....The radioactive isotope of manganese-54 is transmuted to iron-56 along with the emission of a...The bombardment of Deuterium nuclei with Cadmium-114, produce an unknown particle and a proton...
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