Solutions for General Chemistry - Standalone book (MindTap Course List)
Problem 14.1QP:
Consider the reaction N2O4(g)2NO2(g). Draw a graph illustrating the changes of concentrations of...Problem 14.2QP:
When 1.0 mol each of H2(g) and I2(g) are mixed at a certain high temperature, they react to give a...Problem 14.4QP:
Obtain the equilibrium constant for the reaction HCN(aq)H+(aq)+CN(aq) from the following...Problem 14.5QP:
Which of the following reactions involve homogeneous equilibria and which involve heterogeneous...Problem 14.11QP:
How is it possible for a catalyst to give products from a reaction mixture that are different from...Problem 14.13QP:
A chemist put 1.18 mol of substance A and 2.85 mol of substance B into a 10.0-L flask, which she...Problem 14.14QP:
The reaction 3A(g)+B(s)2C(aq)+D(aq) occurs at 25C in a flask, which has 1.87 L available for gas....Problem 14.15QP:
A graduate student places 0.272 mol of PCl3(g) and 8.56 104 mol of PCl5(g) into a 0.718-L flask at...Problem 14.16QP:
An experimenter places the following concentrations of gases in a closed container: [NOBr] = 7.13 ...Problem 14.17QP:
Chemical Equilibrium I Part 1: You run the chemical reaction C(aq)+D(aq)2E(aq) at 25C. The...Problem 14.18QP:
Chemical Equilibrium II Magnesium hydroxide. Mg(OH)2, is a white, partially soluble solid that is...Problem 14.19QP:
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction...Problem 14.20QP:
Suppose liquid water and water vapor exist in equilibrium in a closed container. If you add a small...Problem 14.21QP:
A mixture initially consisting of 2 mol CO and 2 mol H2 comes to equilibrium with methanol, CH3OH,...Problem 14.23QP:
For the reaction 2HI(g)H2(g)+I2(g) carried out at some fixed temperature, the equilibrium constant...Problem 14.24QP:
An experimenter introduces 4.0 mol of gas A into a 1.0-L container at 200 K to form product B...Problem 14.25QP:
The following reaction is earned out at 500 K in a container equipped with a movable piston....Problem 14.26QP:
For the endothermic reaction AB(g)A(g)+B(g), the following represents a reaction container at two...Problem 14.29QP:
A 2.500-mol sample of phosphorus pentachloride, PCl5, decomposes at 160C and 1.00 atm to give 0.338...Problem 14.30QP:
You place 4.00 mol of dinitrogen trioxide, N2O3, into a flask, when: it decomposes at 25.0C and 1.00...Problem 14.31QP:
You place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C...Problem 14.32QP:
Nitrogen monoxide, NO, reacts with bromine, Br2, to give nitrosyl bromide, NOBr....Problem 14.33QP:
In the contact process, sulfuric acid is manufactured by first oxidizing SO2 to SO3, which is then...Problem 14.34QP:
Methanol, CH3OH, formerly known as wood alcohol, is manufactured commercially by the following...Problem 14.35QP:
Write equilibrium-constant expressions Kc for each of the following reactions. a N2O3(g)NO2(g)+NO(g)...Problem 14.36QP:
Write equilibrium-constant expressions Kc for each of the following reactions. a N2H4(g)N2(g)+2H2(g)...Problem 14.37QP:
The equilibrium-constant expression for a gas reaction is Kc[H2O]2[SO2]2[H2S]2[O2]3 Write the...Problem 14.39QP:
The equilibrium-constant expression for a reaction is Kc[NO2]4[O2][N2O5]2 What is the...Problem 14.41QP:
The equilibrium constant Kc, for the equation 2HI(g)H2(g)+I2(g) at 321C is 1.03 What is the value of...Problem 14.42QP:
The equilibrium constant Kc for the equation CS2(g)+4H2(g)CH4(g)+2H2S(g) at 900C is 27.8 What is the...Problem 14.43QP:
A 13.0-L reaction vessel at 499C contained 0.852mol H2, 0.361 mol I2, and 3.84 mol HI. Assuming that...Problem 14.44QP:
A 4.00-L vessel contained 0.0148 mol of phosphorus trichloride, 0.0126 mol of phosphorus...Problem 14.45QP:
Obtain the value of Kc for the following reaction at 900 K: 2SO2(g)+O2(g)2SO3(g) Use the data given...Problem 14.46QP:
Obtain the value of Kc for the following reaction at 500 K: CO(g)+2H2(g)CH3OH(g) Use the data given...Problem 14.47QP:
At 60C, 3.76 mol of nitrosyl bromide, NOBr, placed in a 1.00-L flask dissociates to the extent of...Problem 14.48QP:
A 2 00-mol sample of nitrogen dioxide was placed in an 80.0-L vessel. At 200C, the nitrogen dioxide...Problem 14.49QP:
Write equilibrium-constant expressions Kp for each of the following reactions: a H2(g)+Br2(g)2HBr(g)...Problem 14.50QP:
Write equilibrium-constant expressions Kp for each of the following reactions: a N2O4(g)2NO2(g) b...Problem 14.51QP:
The value of Kc for the following reaction at 298C is 41. C(g)A(g)+3B(g) What is Kp at this...Problem 14.52QP:
The equilibrium constant Kc equals 0.0952 for the following reaction at 227C. CH3OH(g)CO(g)+2H2(g)...Problem 14.53QP:
The reaction SO2(g)+12O2(g)SO3(g) has Kp equal to 6.55 at 627C. What is the value of Kc at this...Problem 14.54QP:
Fluorine, F2, dissociates into atoms on heating. 12F2(g)F(g) The value of Kp at 842C is 7.55 102...Problem 14.55QP:
Write the expression for the equilibrium constant Kc for each of the following equations: a...Problem 14.56QP:
For each of the following equations, give the expression for the equilibrium constant Kc: a...Problem 14.57QP:
On the basis of the value of Kc decide whether or not you expect nearly complete reaction at...Problem 14.58QP:
Would either of the following reactions go almost completely to product at equilibrium? a...Problem 14.59QP:
Hydrogen fluoride decomposes according to the following equation: 2HF(g)H2(g)+F2(g) The value of Kc...Problem 14.60QP:
Suppose sulfur dioxide reacts with oxygen at 25C. 2SO2(g)+O2(g)2SO3(g) The equilibrium constant Kc...Problem 14.63QP:
Methanol, CH3OH, is manufactured industrially by the reaction CO(g)+2H2(g)CH3OH(g) A gaseous mixture...Problem 14.64QP:
Sulfur trioxide, used to manufacture sulfuric acid, is obtained commercially from sulfur dioxide....Problem 14.65QP:
Phosgene, COCl2, used in the manufacture of polyurethane plastics, is prepared from CO and Cl2....Problem 14.66QP:
Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N2 and O2 (from air)....Problem 14.67QP:
Iodine and bromine react to give iodine monobromide, IBr. I2(g)+Br2(g)2IBr(g) What is the...Problem 14.68QP:
Initially a mixture contains 0.850 mol each of N2 and O2 in an 8.00-L vessel. Find the composition...Problem 14.69QP:
Calculate the composition of the gaseous mixture obtained when 1.25 mol of carbon dioxide is exposed...Problem 14.70QP:
The equilibrium constant Kc, for the reaction PCl3(g)+Cl2(g)PCl5(g) equals 49 at 230C. If 0.400 mol...Problem 14.71QP:
Suppose 1.000 mol CO and 3.000 mol H2 are put in a 10.00-L vessel at 1200 K. The equilibrium...Problem 14.72QP:
The equilibrium constant Kc for the reaction N2(g)+3H2(g)2NH3(g) at 450C is 0.159. Calculate the...Problem 14.73QP:
Consider the equilibrium FeO(s)+CO(g)Fe(s)+CO2(g) When carbon dioxide is removed from the...Problem 14.74QP:
a Predict the direction of reaction when chlorine gas is added to an equilibrium mixture of PCl3,...Problem 14.75QP:
What would you expect to be the effect of an increase of pressure on each of the following...Problem 14.76QP:
Indicate whether either an increase or a decrease of pressure obtained by changing the volume would...Problem 14.77QP:
Methanol is prepared industrially from synthesis gas (CO and H2). CO(g)+2H2(g)CH3OH(g);H=21.7kcal...Problem 14.78QP:
One way of preparing hydrogen is by the decomposition of water. 2H2O(g)2H2(g)+O2(g);H=484kJ Would...Problem 14.79QP:
Use thermochemical data (Appendix C) to decide whether the equilibrium constant for the following...Problem 14.80QP:
Use thermochemical data (Appendix C) to decide whether the equilibrium constant for the following...Problem 14.81QP:
What would you expect to be the general temperature and pressure conditions for an optimum yield of...Problem 14.82QP:
Predict the general temperature and pressure conditions for the optimum conversion of ethylene...Problem 14.83QP:
A mixture of carbon monoxide, hydrogen, and methanol, CH3OH, is at equilibrium according to the...Problem 14.85QP:
At 850C and 1.000 atm pressure, a gaseous mixture of carbon monoxide and carbon dioxide in...Problem 14.86QP:
An equilibrium mixture of dinitrogen tetroxide, N2O4, and nitrogen dioxide, NO2, is 65.8% NO2 by...Problem 14.87QP:
A 2.50-L vessel contains 1.75 mol N2, 1.75 mol H2, and 0.346 mol NH3. What is the direction of...Problem 14.88QP:
A vessel originally contained 0.0200 mol iodine monobromide (IBr), 0.050 mol I2, and 0.050 mol Br2....Problem 14.89QP:
A gaseous mixture containing 1.00 mol each of CO, H2O, CO2, and H2 is exposed to a zinc oxide copper...Problem 14.90QP:
A 2.0-L reaction flask initially contains 0.010 mol CO, 0.80 mol H2, and 0.50 mol CH3OH (methanol)....Problem 14.91QP:
Hydrogen bromide decomposes when heated according to the equation 2HBr(g)H2(g)+Br2(g) The...Problem 14.92QP:
Iodine monobromide, IBr, occurs as brownish-black crystals that vaporize with decomposition:...Problem 14.93QP:
Phosgene, COCl2, is a toxic gas used in the manufacture of urethane plastics. The gas dissociates at...Problem 14.94QP:
Dinitrogen tetroxide, N2O4, is a colorless gas (boiling point, 21C), which dissociates to give...Problem 14.97QP:
The amount of nitrogen dioxide formed by dissociation of dinitrogen tetroxide, N2O4(g)2NO2(g)...Problem 14.98QP:
The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at...Problem 14.99QP:
For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n...Problem 14.101QP:
At high temperatures, a dynamic equilibrium exists between carbon monoxide, carbon dioxide, and...Problem 14.102QP:
At high temperatures, a dynamic equilibrium exists between carbon monoxide, carbon dioxide, and...Problem 14.103QP:
The equilibrium constant Kc for the reaction PCl3(g)+Cl2(g)PCl3(g) equals 4.1 at 300C. a A sample of...Problem 14.104QP:
At 25C in a closed system, ammonium hydrogen sulfide exists as the following equilibrium:...Problem 14.105QP:
At moderately high temperatures, SbCl5 decomposes into SbCl3 and Cl2 as follows:...Problem 14.106QP:
The following reaction is important in the manufacture of sulfuric acid. SO2(g)+12O2(g)SO3(g) At 900...Problem 14.107QP:
Sulfuryl chloride is used in organic chemistry as a chlorinating agent. At moderately high...Problem 14.108QP:
Phosgene was used as a poisonous gas in World War I. At high temperatures it decomposes as follows:...Problem 14.109QP:
Gaseous acetic acid molecules have a certain tendency to form dimers. (A dimer is a molecule formed...Problem 14.110QP:
Gaseous acetic acid molecules have a certain tendency to form dimers. (A dimer is a molecules formed...Problem 14.111QP:
When 0.112 mol of NO and 18.22 g of bromine are placed in a 1.00-L reaction vessel and sealed, the...Problem 14.115QP:
A chemist placed a mixture of CO2(g) and CF4(g) into a flask at a particular temperature. These...Problem 14.118QP:
The equilibrium constant Kc for the equation 2HI(g)H2(g)+I2(g) is 1.84 at 425C. The equilibrium...Problem 14.119QP:
Consider the reaction N2O4(g)2NO2(g). Would you expect this reaction to be endothermic or...Problem 14.120QP:
A researcher put 0.400 mol PCl3 and 0.600 mol Cl2 into a 5.00-L vessel at a given temperature to...Problem 14.121QP:
Ammonium hydrogen sulfide. NH4HS, is unstable at room temperature and decomposes:...Problem 14.122QP:
A chemist wants to prepare phosgene, COCl2, by the following reaction: CO(g)+Cl2(g)COCl2(g) He...Problem 14.126QP:
A container with a volume of 1.500 L was evacuated and then filled at low temperature with 0.0500...Problem 14.130QP:
Sulfur dioxide reacts with oxygen to produce sulfur trioxide in the presence of a catalyst:...Problem 14.131QP:
Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br2(g)2Br(g) A...Problem 14.132QP:
Consider the production of ammonia from its elements: N2(g)+3H2(g)2NH3(g) In a pilot experiment, a...Problem 14.133QP:
A mixture of 0.0565 mol phosphorus pentachloride, PCl5, and 0.0800 mol helium gas, He, was placed in...Problem 14.134QP:
Calcium carbonate, CaCO3, decomposes when heated to give calcium oxide. CaO, and carbon dioxide,...Problem 14.135QP:
The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S...Browse All Chapters of This Textbook
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
GENERAL CHEMISTRY is better than ever with this eleventh edition. It includes essential updates--such as modern artwork, higher integration with OWLv2, revised end-of-chapter questions, added Capstone Problems, narrative revisions, and more--to help you succeed in your chemistry course.
Sample Solutions for this Textbook
We offer sample solutions for General Chemistry - Standalone book (MindTap Course List) 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...
More Editions of This Book
Corresponding editions of this textbook are also available below:
General Chemistry, Enhanced Edition [With Access Code] - 9th Edition
9th Edition
ISBN: 9781439043998
General Chemistry
10th Edition
ISBN: 9781285051376
General Chemistry, International Edition
10th Edition
ISBN: 9781111989491
General Chemistry
10th Edition
ISBN: 9788131528983
General Chemistry, Hybrid (with Owlv2 Printed Access Card)
10th Edition
ISBN: 9781285778235
Experiments In General Chemistry, Lab Manual
10th Edition
ISBN: 9781111989422
General Chemistry Student Solutions Manual, 8th Edition
8th Edition
ISBN: 9780618399451
General Chemistry
3rd Edition
ISBN: 9780395528792
General Chemistry : Conceptual Guide
7th Edition
ISBN: 9780618118380
General Chemistry
9th Edition
ISBN: 9780618945856
General Chemistry (Available Titles OWL)
9th Edition
ISBN: 9780618857487
Study Guide For Ebbing's Essentials Of General Chemistry, 2nd
2nd Edition
ISBN: 9780618491773
Media Guide For Ebbing's Essentials Of General Chemistry, 2nd
2nd Edition
ISBN: 9780618492473
Essentials of General Chemistry
2nd Edition
ISBN: 9780618578023
Essential General Chemistry Student Cd-rom 2nd Ed
2nd Edition
ISBN: 9780618577330
Student Solutions Manual For Ebbing's Essentials Of General Chemistry, 2nd
2nd Edition
ISBN: 9780618491780
Essentials of General Chemistry
2nd Edition
ISBN: 9780618491759
Bundle: General Chemistry, 11th + OWLv2, 4 terms (24 months) Printed Access Card
11th Edition
ISBN: 9781337191050
General Chemistry
11th Edition
ISBN: 9781305859142
Student Solutions Manual for Ebbing/Gammon's General Chemistry
11th Edition
ISBN: 9781305886780
EBK GENERAL CHEMISTRY
11th Edition
ISBN: 8220101425904
Owlv2, 1 Term (6 Months) Printed Access Card For Ebbing/gammon's General Chemistry, 11th
11th Edition
ISBN: 9781305674059
GENERAL CHEMISTY (REVISED PRTG)
11th Edition
ISBN: 9780357047743
GENEAL CHEMISTRY (LL) (W/ACESS CARD)
11th Edition
ISBN: 9780357047750
Bundle: General Chemistry, Loose-Leaf Version, 11th + LabSkills PreLabs v2 for Organic Chemistry (powered by OWLv2), 4 terms (24 months) Printed ... for Ebbing/Gammon's General Chemistry, 11th
11th Edition
ISBN: 9781337542630
OWLv2, 4 terms (24 months) Printed Access Card for Ebbing/Gammon's General Chemistry, 11th
11th Edition
ISBN: 9781305673892
Bundle: General Chemistry, Loose-leaf Version, 11th + Owlv2, 1 Term (6 Months) Printed Access Card
11th Edition
ISBN: 9781337128438
Bundle: General Chemistry, Loose-leaf Version, 11th + Lms Integrated For Owlv2 With Mindtap Reader, 4 Terms (24 Months) Printed Access Card
11th Edition
ISBN: 9781337128452
OWLv2 with Student Solutions Manual eBook for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 4 terms (24 months)
11th Edition
ISBN: 9781305864900
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN: 9781305887299
Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2, 4 terms (24 months) Printed Access Card
11th Edition
ISBN: 9781337128391
Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2 with Student Solutions Manual eBook, 4 terms (24 months) Printed Access Card
11th Edition
ISBN: 9781337128469
OWLV2 FOR EBBING/GAMMON'S GENERAL CHEMI
11th Edition
ISBN: 9781305673908
OWLv2 for Ebbing/Gammon's General Chemistry, 11th Edition, [Instant Access], 1 term (6 months)
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
11th Edition
ISBN: 9781305864887
Study Guide for Ebbing/Gammon's General Chemistry, 11th
11th Edition
ISBN: 9781305672864
GEN CHEM(LL)+OWL+WEBASSIGN>BI<
11th Edition
ISBN: 9780357298411
Student Solutions Manual for Ebbing/Gammon's General Chemistry, 11th
11th Edition
ISBN: 9781305673472
Lab Manual Experiments in General Chemistry
11th Edition
ISBN: 9781305944985
General Chemistry-OWL Access (24 Months)
11th Edition
ISBN: 9781305864894
General Chemistry (Instructor's)
11th Edition
ISBN: 9781305672826
Related Chemistry Textbooks with Solutions
Still sussing out bartleby
Check out a sample textbook solution.