General Chemistry11th EditionEbbing, Darrell D., Gammon, Steven D. Publisher: Cengage Learning,ISBN: 9781305859142
General Chemistry
Solutions for General Chemistry
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Chapter 1 - Chemistry And MeasurementChapter 1.3 - Law Of Conservation Of MassChapter 1.4 - Matter: Physical State And Chemical CompositionChapter 1.5 - Measurement And Significant FiguresChapter 1.6 - Si UnitsChapter 1.7 - Derived UnitsChapter 1.8 - Units And Dimensional Analysis (factor-label Method)Chapter 2 - Atoms, Molescules, And IonsChapter 2.1 - Atomic Theory Of MatterChapter 2.2 - The Structure Of The Atom
Chapter 2.3 - Nuclear Structure; IsotopesChapter 2.4 - Atomic WeightsChapter 2.5 - Periodic Table Of The ElementsChapter 2.6 - Chemical Formulas; Molecular And Ionic SubstancesChapter 2.8 - Naming Simple CompoundsChapter 2.10 - Balancing Chemical EquationsChapter 3 - Calculations With Chemical Formulas And EquaitonsChapter 3.1 - Molecular Weight And Formula WeightChapter 3.2 - The Mole ConceptChapter 3.3 - Mass Percentages From The FormulaChapter 3.4 - Elemental Analysis: Percentages Of Carbon, Hydrogen And OxygenChapter 3.5 - Determining FormulasChapter 3.6 - Molar Interpretation Of A Chemical EquationChapter 3.7 - Amounts Of Substances In A Chemical ReactionChapter 3.8 - Limiting Reactant; Theoretical And Percentage YieldsChapter 4 - Chemical ReactionsChapter 4.1 - Ionic Theory Of Solutions And Solubility RulesChapter 4.2 - Molecular And Ionic EquationsChapter 4.3 - Precipitation ReactionsChapter 4.4 - Acid-base ReactionsChapter 4.5 - Oxidation-reduction ReactionsChapter 4.6 - Balancing Simple Oxidation-reduction EquationsChapter 4.7 - Molar ConcentrationChapter 4.8 - Diluting SolutionsChapter 4.9 - Gravimetric AnalysisChapter 4.10 - Volumetric AnalysisChapter 5 - The Gaseous StateChapter 5.1 - Gas Pressure And Its MeasurementChapter 5.2 - Empirical Gas LawsChapter 5.3 - The Ideal Gas LawChapter 5.4 - Stoichiometry Problems Involving Gas VolumesChapter 5.5 - Gas Mixtures; Law Of Partial PressuresChapter 5.6 - Kinetic Theory Of An Ideal GasChapter 5.7 - Moleculat Speeds; Diffusion And EffusionChapter 5.8 - Real GasesChapter 6 - ThermochemistyChapter 6.1 - Energy And Its UnitsChapter 6.2 - First Law Of Thermodynamics; Work And HeatChapter 6.3 - Heat Of Reaction; Enthalpy Of ReactionChapter 6.4 - Thermochemical EquaitonsChapter 6.5 - Applying Stoichiometry To Heats Of ReactionChapter 6.6 - Measuring Heats Of ReactionChapter 6.7 - Hess's LawChapter 6.8 - Standard Enthalpies Of FormationChapter 7 - Quantum Theory Of The AtomChapter 7.1 - The Wave Nature Of LightChapter 7.2 - Quantum Effects And PhotonsChapter 7.3 - The Bohr Theory Of The Hydrogen AtomChapter 7.4 - Quantum MechanicsChapter 7.5 - Quantum Numbers And Atomic OrbitalsChapter 8 - Electron Configurations And PeriodicityChapter 8.1 - Electron Spin And The Pauli Exclusion PrincipleChapter 8.2 - Building-up Principle And The Periodic TableChapter 8.3 - Writing Electron Configurations Using The Periodic TableChapter 8.4 - Orbital Diagrams Of Atoms; Hund's RuleChapter 8.6 - Some Periodic PropertiesChapter 8.7 - Periodicity In The Main-group ElementsChapter 9 - Ionic And Covalent BondingChapter 9.1 - Describing Ionic BondsChapter 9.2 - Electron Configurations Of IonsChapter 9.3 - Ionic RadiiChapter 9.5 - Polar Covalent Bonds; ElectronegativityChapter 9.6 - Writing Lewis Electron-dot FormulasChapter 9.7 - Delocalized Bonding: ResonanceChapter 9.8 - Exceptions To The Octet RuleChapter 9.9 - Formal Charge And Lewis FormulasChapter 9.10 - Bond Length And Bond OrderChapter 9.11 - Bond EnthalpyChapter 10 - Molecular Geometry And Chemical Bonding TheoryChapter 10.1 - The Valence-shell Electron-pair Repulsion (vsepr) ModelChapter 10.2 - Dipole Moment And Molecular GeometryChapter 10.3 - Valence Bond TheoryChapter 10.4 - Description Of Multiple BondingChapter 10.6 - Electron Configurations Of Diatomic Moleucles Of The Second-period ElementsChapter 11 - States Of Matter; Liquids And SolidsChapter 11.2 - Phase TransitionsChapter 11.3 - Phase DiagramsChapter 11.5 - Intermolecular Forces; Explaining Liquid PropertiesChapter 11.6 - Classification Of Solids By Type Of Attraction Of UnitsChapter 11.7 - Crystalline Solids; Crystal Lattices And Unit CellsChapter 11.8 - Structures Of Some Crystalline SolidsChapter 11.9 - Calculations Involving Unit-cell DimensionsChapter 12 - SolutionsChapter 12.1 - Types Of SolutionsChapter 12.2 - Solubility And The Solution ProcessChapter 12.3 - Effects Of Temperature And Pressure On SolubilityChapter 12.4 - Ways Of Expressing ConcentrationChapter 12.5 - Vapor Pressure Of A SolutionChapter 12.6 - Boiling-point Elevation And Freezing-point DepressionChapter 12.7 - OsmosisChapter 12.8 - Colligative Properites Of Ionic SolutoinsChapter 12.9 - ColloidsChapter 13 - Rates Of ReactionChapter 13.1 - Definition Of Reaction RateChapter 13.3 - Dependence Of Rate On ConcentrationChapter 13.4 - Change Of Concentration With TimeChapter 13.5 - Temperature And Rate; Collision And Transisiton-state TheoriesChapter 13.6 - Arrhenius EquationChapter 13.7 - Elementary ReactionsChapter 13.8 - The Rate Law And The MechanismChapter 14 - Chemical EquilibirumChapter 14.1 - Chemical Equilbrium - A Dynamic EquilibriumChapter 14.2 - The Equilibrium ConstantChapter 14.3 - Heterogenous Equilibria; Solvents In Homogenous EquilibriaChapter 14.4 - Qualitativelys Interpreting The Equilibrium ConstantChapter 14.5 - Predicting The Direction Of ReactionChapter 14.6 - Calculating Equilibrium ConcentrationsChapter 14.7 - Removing Products Or Adding ReactantsChapter 14.8 - Changing The Pressure And TemperatureChapter 15 - Acids And BasesChapter 15.2 - Bronsted-lowry Concept Of Acids And BassesChapter 15.3 - Lewis Concept Of Acids And BasesChapter 15.4 - Relative Strengths Of Acids And BasesChapter 15.5 - Moleculat Structure And Acid StrengthChapter 15.7 - Solutions Of A Strong Acid Or BaseChapter 15.8 - The Ph Of A SolutionChapter 16 - Acid-base EquilibriaChapter 16.1 - Acid-ionization EquilibriaChapter 16.2 - Polyprotic AcidsChapter 16.3 - Base-ionization Of EquilibriaChapter 16.4 - Acid-base Properties Of Salt SolutionsChapter 16.5 - Common-ion EffectChapter 16.6 - BuffersChapter 16.7 - Acid-base Titration CurvesChapter 17 - Solubility And Complex-ion EquilibriaChapter 17.1 - The Solubility Product ConstantChapter 17.2 - Solubility And The Common-ion EffectChapter 17.3 - Precipitation CalculationsChapter 17.4 - Effect Of Ph On SolubilityChapter 17.5 - Complex-ion FormationChapter 17.6 - Complex Ions And SolubilityChapter 18 - Thermodynamics And EquilibriumChapter 18.2 - Entropy And The Second Law Of ThermodynamicsChapter 18.3 - Strandard Entropies And The Third Law Of ThermodynamicsChapter 18.4 - Free Energy And SpontaneityChapter 18.6 - Relating ?g° To The Equilibrium ConstantChapter 18.7 - Change Of Free Energy With TemperatureChapter 19 - ElectrochemistryChapter 19.1 - Balancing Oxidation-reduction Reactions In Acidic And Basic SolutionsChapter 19.2 - Construction Of Voltaic CellsChapter 19.3 - Notation For Voltaic CellsChapter 19.4 - Cell PotentialChapter 19.5 - Standard Cell Potentials And Standard Electrode PotentialsChapter 19.6 - Equilibrium Constants From Cell PotentialsChapter 19.7 - Dependence Of Cell Potential On ConcentrationChapter 19.8 - Some Commercial Voltaic CellsChapter 19.9 - Electrolysis Of Molten SaltsChapter 19.10 - Aquesous ElectrolysisChapter 19.11 - Stiochiometry Of ElectrolysisChapter 20 - Nuclear ChemistryChapter 20.1 - RadioactivityChapter 20.2 - Nuclear Bombardment ReactionsChapter 20.3 - Radations And Matter: Detection And Biological EffectsChapter 20.4 - Rate Of Radioactive DecayChapter 20.6 - Mass-energy CalculationsChapter 21 - Chemistry Of The Main-group ElementsChapter 21.9 - Group 5a: Nitrogen And The Phosphorus FamilyChapter 21.10 - Group 6a: Oxygen And The Sulfur FamilyChapter 22 - The Transition Elements And Coordination CompoundsChapter 22.3 - Formation And Structure Of ComplexesChapter 22.4 - Naming Coordination CompoundsChapter 22.5 - Structure And Isomerism In Coordination CompoundsChapter 22.7 - Crystal Field TheoryChapter 23 - Organic ChemistryChapter 23.2 - Alkanes And CycloalkanesChapter 23.3 - Alkenes And AlkynesChapter 23.5 - Naming HydrocarbonsChapter 23.6 - Organic Compounds Containing OxygenChapter 24 - Polymer Materials: Synthetic And BiologicalChapter 24.1 - Synthesis Of Organic PolymersChapter 24.3 - ProteinsChapter 24.4 - Nucleic AcidsChapter A.1 - Scientific (exponential) NotationChapter A.2 - LogarithmsChapter A.3 - Algebraic Operations And Graphing
Book Details
Darrell Ebbing's GENERAL CHEMISTRY is recognized for its signature clear explanations, macro to micro orientation, and enhanced problem-solving strategies that have made it a best seller. The eleventh edition incorporates nomenclature changes and the adoption of IUPAC periodic table conventions, along with changes to the discussion of d orbitals. Reformatted examples facilitate learning, reinforced by new end-of-chapter questions as well as new capstone problems added to a number of chapters. Also available: the OWLv2 interactive online learning system for chemistry.
Sample Solutions for this Textbook
We offer sample solutions for General Chemistry homework problems. See examples below:
Chapter 1, Problem 1.1QPChapter 1, Problem 1.57QPChapter 1, Problem 1.58QPChapter 1, Problem 1.65QPChapter 1, Problem 1.66QPChapter 1, Problem 1.67QPChapter 1, Problem 1.68QPChapter 1, Problem 1.69QPChapter 1, Problem 1.70QP
Chapter 1, Problem 1.109QPChapter 1, Problem 1.113QPChapter 1, Problem 1.114QPExplanation: Given mass in problem statement is 8.45 kg . Since, 1 kg = 103 g and 1 μg = 10-6 g , we...Explanation: Given distance in problem statement is 127 Å . Since, 1 Å = 10−10 m and 1 mg = 10-3 g ,...Chapter 1, Problem 1.135QPChapter 1, Problem 1.136QPChapter 1, Problem 1.169QPChapter 1, Problem 1.170QPChapter 2, Problem 2.1QPChapter 2, Problem 2.25QPChapter 2, Problem 2.26QPExplanation: The product in the given chemical equation is Lithium chloride. Hence, the starting...Chapter 2, Problem 2.97QPChapter 2, Problem 2.98QPExplanation: The given reaction in the problem statement is ammonium chloride and barium hydroxide...Explanation: The raw chemical equation given in the problem statement is, C2H6 + O2 → CO2 + H2O The...Chapter 2, Problem 2.126QPExplanation: Molecule is the term that is used for compounds which contain only covalent bonding...Chapter 3, Problem 3.1QPExplanation: To calculate the number of candy pieces in 0.2 kg of candy. Given, 1.0 kg of candy has...Chapter 3, Problem 3.18QPChapter 3, Problem 3.33QPChapter 3, Problem 3.37QPChapter 3, Problem 3.41QPChapter 3, Problem 3.42QPChapter 3, Problem 3.45QPChapter 3, Problem 3.46QPChapter 3, Problem 3.57QPChapter 3, Problem 3.58QPChapter 3, Problem 3.63QPExplanation: To calculate the masses of Carbon, Hydrogen and Oxygen. Molar mass of Carbon is 12.01 g...Explanation: To determine the produced mass of K2SO4 The given reaction is, 2 KOH+ H2SO4→K2SO4 +...Chapter 3, Problem 3.141QPChapter 4, Problem 4.1QPChapter 4, Problem 4.33QPChapter 4, Problem 4.34QPChapter 4, Problem 4.38QPChapter 4, Problem 4.39QPChapter 4, Problem 4.40QPChapter 4, Problem 4.43QPChapter 4, Problem 4.44QPChapter 4, Problem 4.45QPChapter 4, Problem 4.46QPExplanation: The complete molecular equation for the reaction between potassium hydroxide and...Chapter 4, Problem 4.48QPExplanation: The molecular equation for the reaction between HCN and lithium hydroxide is given...Chapter 4, Problem 4.100QPChapter 4, Problem 4.101QPChapter 4, Problem 4.103QPExplanation: Assume that both hydrogen atoms of H2SO4 ionize completely. H2SO4(aq) + Ba(OH)2(aq) →...Explanation: When an object having one kilogram of mass and it is placed in one square meter area...Explanation: Figure 1 According to kinetic theory of gases the molecules in a container are...Explanation: From Ideal gas equation, PV = nRT we can observe that pressure is directly proportional...Explanation: Figure 1 From Ideal gas law, PV = nRT Pressure and volume are inversely proportional to...Chapter 5, Problem 5.32QPExplanation: From the ideal gas equation and density formula, Both the density and pressure are...Explanation: To Calculate: The partial pressure of each of the gases from a certain volcano whose...Explanation: To Calculate: The rms speed (in m/s) of nitrogen (N2) molecules at 25∘C and at 125∘C...Chapter 5, Problem 5.136QPExplanation: Given data: A container is filled with 16.0 g of O2 and 14.0 g of N2 Moles of oxygen:...Chapter 5, Problem 5.147QPChapter 5, Problem 5.153QPExplanation: Given, A sample of Zinc with pressure 751 mmHg and temperature 170C . The level of...Chapter 5, Problem 5.158QPChapter 5, Problem 5.159QPExplanation: Given, An ideal gas with RMS of a gas is 5.00×102m/s and pressure of 2.5 atm and...Explanation: Given, Power plant driven by fossil fuel combustion generate substantial greenhouse...Chapter 6, Problem 6.1QPChapter 6, Problem 6.32QPChapter 6, Problem 6.36QPChapter 6, Problem 6.75QPChapter 6, Problem 6.76QPChapter 6, Problem 6.80QPChapter 6, Problem 6.81QPChapter 6, Problem 6.82QPChapter 6, Problem 6.115QPChapter 6, Problem 6.125QPExplanation: Given information, 2Al(s) + Fe2O3(s) → 2Fe(l) + Al2O3(s)ΔHf : 2 × 0 - 825.5 2 × 12.40...Explanation: Given information, 4KO2(s) + 2H2O(l) → 4KOH(s) + 3O2(g)ΔHof : 4 × - 284.5 2 × -285.8 4...Explanation: Given information, 2Na(s) + 2H2O(l) → 2Na+(aq) + 2OH-(aq) + H2(g)ΔHf : 0 2 × -285.8 2 ×...Explanation: Given information Total mass of hydrogen and oxygen gas is 2.500 g.Temperature is 25 oC...Chapter 6, Problem 6.151QPChapter 6, Problem 6.152QPExplanation: Figure 1 Calculate the HHV for propane by using the trend line equation, Molar mass for...Chapter 7, Problem 7.1QPChapter 7, Problem 7.23QPChapter 7, Problem 7.24QPChapter 7, Problem 7.67QPChapter 7, Problem 7.69QPChapter 7, Problem 7.70QPChapter 7, Problem 7.82QPChapter 7, Problem 7.83QPExplanation: To calculate: The wavelength of emitted light when an electron from hydrogen atom...Chapter 7, Problem 7.105QPChapter 7, Problem 7.106QPChapter 7, Problem 7.108QPChapter 7, Problem 7.112QPChapter 8, Problem 8.1QPExplanation: Bohr formula is ΔE=-RH[22∞2−2212]=-RH[-4]= 4 RH 4 × 2.179×10-18J1 He+ ion I.E= 4 ×...Chapter 9, Problem 9.1QPChapter 9, Problem 9.24QPChapter 9, Problem 9.71QPChapter 9, Problem 9.72QPChapter 9, Problem 9.75QPChapter 9, Problem 9.81QPChapter 9, Problem 9.118QPExplanation: The electronic configuration of Cl atom is Cl17:[Ne]3s2 3p5 But the Chlorine atom gain...Chapter 9, Problem 9.137QPChapter 9, Problem 9.138QPChapter 10, Problem 10.1QPChapter 10, Problem 10.37QPChapter 10, Problem 10.38QPChapter 11, Problem 11.1QPChapter 11, Problem 11.25QPChapter 11, Problem 11.28QPChapter 11, Problem 11.63QPChapter 11, Problem 11.74QPExplanation: Intermolecular force in each compound In a 1-Pentanol, the intermolecular forces are...Explanation: Intermolecular force in each compound CH3CHO is found to be polar molecule, therefore...Chapter 11, Problem 11.157QPExplanation: Gaseous solution is made of gases. One best example for gaseous solution is air – it is...Chapter 12, Problem 12.25QPChapter 12, Problem 12.26QPChapter 12, Problem 12.70QPExplanation: Assume that volume of solution is 1.000 L which is equivalent to 1.040 kg as density of...Explanation: Assume that volume of solution is 1.000 L which is equivalent to 1.127 kg as density of...Chapter 12, Problem 12.95QPChapter 12, Problem 12.96QPChapter 12, Problem 12.107QPChapter 12, Problem 12.108QPExplanation: Parts per million is expressed as, ppm = mass of solutemass of solution × 106 The term...Explanation: Determine the number of moles of each ion present in the solution. Totally five types...Explanation: Determine the number of moles of each ion present in the solution. Totally five types...Chapter 12, Problem 12.141QPChapter 12, Problem 12.142QPChapter 13, Problem 13.1QPChapter 13, Problem 13.27QPExplanation: The reaction follows first order with presence of half-life of ten seconds. There are...Chapter 13, Problem 13.65QPChapter 13, Problem 13.95QPChapter 13, Problem 13.96QPExplanation: Given, Time[CH3NNCH3]0.0min1.50×10-2 M 1.0min1.26×10-2 M2.0min1.10×10-2 M3.0...Explanation: Given, Time[NO2]0.0min0.1103 M 1.0min0.1076 M2.0min0.1050 M3.0 min0.1026 M Time Average...Chapter 13, Problem 13.105QPExplanation: To calculate the concentration of NO2 after 2.5×102 sec The integrated rate law for...Chapter 13, Problem 13.132QPChapter 13, Problem 13.140QPChapter 13, Problem 13.141QPChapter 13, Problem 13.145QPExplanation: The plot of 1[A] (vs) time gives a straight line and the reaction is said to be second...Chapter 13, Problem 13.150QPChapter 14, Problem 14.1QPChapter 14, Problem 14.45QPChapter 14, Problem 14.71QPChapter 14, Problem 14.72QPExplanation: Given, The equilibrium constant Kc =3.92 The initial amount of CO = 1.00 mol The...Explanation: Given, The equilibrium constant Kc =0.153 The initial amount of N2 = 1.00 mol The...Chapter 14, Problem 14.101QPChapter 14, Problem 14.103QPChapter 14, Problem 14.107QPChapter 14, Problem 14.108QPExplanation: Given, Volume of the flask =2.00 L Pressure = 1.00atm Partial pressure of N2=0.781 atm...Explanation: Given, The initial amount of I2 = 0.500 mol The initial amount of Br2 = 0.500 mol The...Chapter 14, Problem 14.137QPChapter 14, Problem 14.138QPChapter 15, Problem 15.1QPChapter 15, Problem 15.20QPChapter 15, Problem 15.35QPChapter 15, Problem 15.36QPChapter 15, Problem 15.53QPChapter 15, Problem 15.54QPChapter 15, Problem 15.85QPChapter 15, Problem 15.99QPChapter 15, Problem 15.100QPExplanation: Illustration of amphiprotic behavior of bicarbonate ion with water by writing...Chapter 15, Problem 15.102QPExplanation: The hydrated aluminum ion acts as Bronsted-Lowry acid and it can react with ammonia a...Chapter 15, Problem 15.119QPExplanation: The equilibrium of the given reaction can be represented as follows. Conc. (M) H3O+(aq)...Chapter 16, Problem 16.1QPChapter 16, Problem 16.21QPChapter 16, Problem 16.22QPChapter 16, Problem 16.47QPChapter 16, Problem 16.91QPChapter 16, Problem 16.92QPChapter 16, Problem 16.113QPChapter 16, Problem 16.114QPChapter 16, Problem 16.116QPChapter 16, Problem 16.119QPChapter 16, Problem 16.120QPChapter 16, Problem 16.129QPChapter 16, Problem 16.130QPChapter 16, Problem 16.135QPExplanation: To Calculate: The pH prior to the addition of any HCl Given data: A 0.150 M solution of...Chapter 16, Problem 16.157QPChapter 17, Problem 17.1QPChapter 17, Problem 17.31QPChapter 17, Problem 17.33QPChapter 17, Problem 17.34QPChapter 17, Problem 17.41QPChapter 17, Problem 17.42QPChapter 17, Problem 17.43QPChapter 17, Problem 17.67QPChapter 17, Problem 17.68QPChapter 17, Problem 17.91QPExplanation: To calculate: The molar solubility of AgI in 2.2 M NH3 . Given, The strength of NH3 is...Explanation: To calculate: The concentration of calcium ion, sodium ion, chloride ion and fluoride...Explanation: To calculate: The quantity of water and ammonia required to dissolve silver chloride....Chapter 17, Problem 17.128QPChapter 18, Problem 18.1QPExplanation: To give: The change in the water sample Given information, temperature of the water is...Explanation: To explain: The change in standard free energy for the given reaction Given reaction...Chapter 18, Problem 18.50QPExplanation: To calculate: the value of ΔHo Given reaction and information ΔHo (kJ)CO2(g) + 2H2(g) →...Chapter 18, Problem 18.88QPExplanation: To calculate: The value of ΔHo and ΔSo for the given reactions For the first reaction,...Chapter 18, Problem 18.92QPChapter 18, Problem 18.97QPChapter 18, Problem 18.98QPExplanation: To calculate: The value of ΔHof The value of standard enthalpy change of formation...Explanation: Given reaction and information 2NH3(g) → 3H2(g) + N2(g)ΔHfo: 2 × -45.90 0 0 kJ So: 2 ×...Explanation: Given reaction and information CO(g) + 3H2(g) → CH4(g) + H2O(g)ΔHfo: -110.5 0 -74.87...Chapter 19, Problem 19.1QPChapter 19, Problem 19.23QPChapter 19, Problem 19.32QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: C2O42- →2CO2 +...Explanation: To write the equations for two half-reactions, Oxidation half reaction: Mn2+ →MnO4- +...Chapter 19, Problem 19.37QPChapter 19, Problem 19.38QPChapter 19, Problem 19.39QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: 8H2S → S8 +...Chapter 19, Problem 19.41QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: H2O2 →O2 + 2e-...Chapter 19, Problem 19.101QPExplanation: To write the equations for two half-reactions, Oxidation half reaction: S2-→ S8...Chapter 19, Problem 19.113QPExplanation: Given: Reduction of 2.0 mol Fe3+ to Fe2+ In above reduction 1 mole of electron is...Explanation: To calculate the cell potential (EMF) of given cell The standard reduction potentials...Explanation: Two types of nuclear reactions are, Radioactive decay Nuclear bombardment reactions...Explanation: Alpha emission ( α ): An unstable nucleus emits 24He nucleus or alpha particle....Explanation: Given nuclear reaction is, 4H11→H24e + 2e10 This reaction is found to be fusion...Explanation: To determine: Nuclear masses of each nucleus Nuclear mass of 12H = 2.01400 amu -...Explanation: To determine: Nuclear mass of 11H nucleus Nuclear mass of 12H = 2.01400 amu -...Explanation: Given: Mass of I-136 nuclei = 135.8401 amu Mass of Y-96 nuclei = 95.8629 amu Nuclear...Explanation: Given: Nuclear mass of 24He= 4.00260 amu-(2×0.000549amu)=4.001502amu Write the...Explanation: When Bromine-82 undergoes beta ( -10β ) decay it gives Krypton-82. This balanced...Explanation: When Tellurium-132 undergoes beta ( -10β ) decay it gives Xenon-132. This balanced...Given incomplete nuclear reaction is, 1431Si→ 1531P + ? This is written as, 1431Si→ 1531P + ZAX...Explanation: To calculate: Mass defect of Sodium Atomic mass of Na = 22.99 amu Mass of eleven...Explanation: Given Mass of electron = 0.000549 amu Temperature = 25°C 2p + 2n→ 24He Nuclear mass of...Explanation: Given Mass of electron = 0.000549 amu Temperature = 25°C 94239Pu→ 92235U + 24H...Explanation: Alloy is a mixture of one or more metals in a solid form. Examples for alloys are...Explanation: Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide...Explanation: To Write: The complete balanced equation for the given incomplete reaction. Potassium...Explanation: To Write: The complete balanced equation for the given incomplete reaction. Lithium...Explanation: To Write: The complete balanced equation for the given incomplete reaction. Barium...Explanation: Given Equation: KOH(aq) + MgCl2(aq)→ Complete Equation: A complete equation will have...Explanation: Given data: Lead(IV) oxide is prepared by oxidizing plumbite ion, Pb(OH)3- which exists...Explanation: Given Equation: Al2O3(s) + H2SO4(aq)→ Complete Equation: A complete equation will have...Explanation: Given Equation: Pb(NO3)2(aq) + Al(s)→ Complete Equation: A complete equation will have...Explanation: Given: The given molecule is ethylene and carbon is group 4A element. Carbon atom has 4...Explanation: Given data: The given cracking reaction is: CH4(g) →C(graphite) + 2H2(g) To Calculate:...Explanation: Given data: The given reaction involving synthesis of gas is: CO(g) + 2H2(g)→ CH3OH(g)...Explanation: Given Equation: CO2(g) + Ba(OH)2(aq)→ Complete Equation: A complete equation will have...Explanation: Given Equation: NaHCO3(aq) + HC2H3O2(aq)→ Complete Equation: A complete equation will...Explanation: Given data: Burning of lithium metal in oxygen. Chemical Equation: The chemical...Explanation: Given data: Burning of calcium metal in oxygen. Chemical Equation: The chemical...Explanation: Given data: Water vapor decomposes to atoms in gas phase. Hydrogen peroxide vapor...Explanation: To write: The complete and balanced equation for given combustion. P4(s) + 5O2(g) →...Explanation: To determine: The percentage of sodium acetate in a mixture of sodium acetate and...Explanation: To write: Chemical equation for given reaction Carbon burns in a air it gives Carbon...Explanation: To write: The reaction between copper and hydrochloric acid, iron and hydrochloric...Chapter 22, Problem 22.1QPExplanation: Atomic number of Vanadium is 23 and its electronic configuration is...Explanation: Atomic number of Zirconium is 40 and its electronic configuration is [Kr]4d25s2 . In...Explanation: In the complex ion [Pt(NH3)2]2+ the central metal ion Platinum is in +2 oxidation state...Explanation: In the complex ion [Pt(NH3)2(NO2)2]2+ the central metal ion Platinum is in +4 oxidation...Explanation: The reaction between Cu2+(aq) , NH3(aq) and [Cu(NH3)4]2+(aq) can be represented as,...Explanation: The reaction between Ag+(aq) , NH3(aq) and [Ag(NH3)2]+(aq) can be represented as,...Explanation: The complex ion [CoF6]3− has six fluoro ligands. Hence, the co-ordination number is six...Explanation: Oxidation state of Chromium in the complex [Cr(H2O)6]3+ , oxidation state of Cr =...Explanation: Oxidation state of Cobalt in the complex [Co(NH3)6]3+ , oxidation state of Co = charge...Chapter 23, Problem 23.1QPExplanation: By looking at the formula of the given compound we can identify that a carbonyl group...Explanation: For First structure: In the given ball-stick model, the black spheres are carbon atoms,...Chapter 23, Problem 23.24QPChapter 23, Problem 23.31QPExplanation: The given reaction in the problem statement is an combustion reaction and hence, the...Explanation: From the given name of the hydrocarbon, the parent carbon is identified as octane....Chapter 23, Problem 23.40QPExplanation: 2-methylpentane has the molecular formula of C6H14 . When this undergoes combustion...Explanation: Differentiation between condensation and addition polymer are as follows, Addition...
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11th Edition
ISBN: 9781305673939
Lms Integrated For Owlv2 With Mindtap Reader, 4 Terms (24 Months) Printed Access Card For Ebbing/gammon's General Chemistry, 11th
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Study Guide for Ebbing/Gammon's General Chemistry, 11th
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GEN CHEM(LL)+OWL+WEBASSIGN>BI<
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