Solutions for CHEMISTRY:CENTRAL SCI.-W/ACCESS>CUSTOM<
Problem 1DE:
Which element is oxidized, and which is reduced in the following reactions? N2(g) + 3 H2(g) 2...Problem 1E:
Which of the following are redox reactions? For those that are, indicate which element is oxidized...Problem 6E:
The solubility of Xe in water at 1 atm pressure and 20 °C is approximately 5103M . (a) Compare this...Problem 7E:
The coinage metals (Group 1B) copper, silver, and gold have specific heats of 0.385, 0.233, and...Problem 9E:
The contents of the closed box in each of the following illustrations represent a system, and the...Problem 10E:
An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The...Problem 11E:
4.42 Because the oxide ion is basic, metal oxides react readily with acids.
Write the net ionic...Problem 13E:
4.44 As K20 dissolves in water, the oxide ion reacts with water molecules to form hydroxide...Problem 14E:
True or false: If a substance is oxidized, it is gaining electrons. If an ion is oxidized, its...Problem 16E:
Which region of the periodic table shown here contains elements that are easiest to oxidize? Which...Problem 17E:
Determine the oxidation number of sulfur in each of the following substances: barium sulfate. BaSO4,...Problem 18E:
Determine the oxidation number for the indicated element in each of the following substances: Sin...Problem 19E:
Determine the oxidation number for the indicated element in each of the following compounds: Co in...Problem 20E:
Write balanced molecular and net ionic equations for the reactions of hydrochloric acid with nickel,...Problem 21E:
Using the activity series (Table 4.5), write balanced chemical equations for the following...Problem 22E:
The enthalpy of solution of KBr in water is about + 198 kJ/mol. Nevertheless, the solubility of KBr...Problem 24E:
4.58 The following reactions (note that the arrows are pointing only one direction) can be used to...Problem 25E:
Is the concentration of a solution an intensive or an extensive property? What is the difference...Problem 27E:
Calculate the molarity of a solution that contains 0.175 mol ZnC12 in exactly 150 mL of solution....Problem 28E:
4.62
Calculate the molarity of a solution made by dissolving 12.5 grams of Na2CrO4 in enough water...Problem 30E:
4.66 The average adult male has a total blood volume of 5.0 L. After drinking a few beers, he has a...Problem 31E:
4.67
How many grams of ethanol, CH2CH2OH should you dissolve in water to make 1.00 L of vodka...Problem 33E:
Which will have the highest concentration of potassium ion: 0.20 M KC1, 0.15 M K2CrO4, or 0.080 M...Problem 36E:
13.36 Explain why pressure substantially affects the solubility of O2in water but has little effect...Problem 45E:
Some sulfuric acid is spilled on a lab bench You can neutralize the acid by sprinkling sodium...Problem 46E:
4.84 The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium...Problem 47E:
A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100 0 mL of water An acid-base...Problem 48E:
4.86 An 8.65-g sample of an unknown group 2A metal hydroxide is dissolved in 85.0 mL of water. An...Problem 49E:
A solution of 100.0 mL of 0.200 M KOH is mixed with a solution of 200.0 mL of 0.150 M NiSO4. Write...Problem 50E:
A 1.248-9 sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCI...Problem 51E:
4.91 Uranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear...Problem 52E:
The accompanying photo shows the reaction between a solution of Cd(NO3)2 and one of Na2S What is the...Problem 54E:
4.94 You choose to investigate some of the solubility guidelines for two ions not listed in Table...Problem 55E:
4 95 Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers...Problem 56E:
4 96 The commercial production of nitric acid involves the following chemical reactions
4 NH3(g) +...Problem 57E:
Consider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution,...Problem 58E:
98 Bronze is a solid solution of Cu(s) and Sn(s); solutions of metals like this that are solids are...Problem 60E:
Tartaric acid. H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and a salt...Problem 62E:
A solid sample of Zn(OH)2 is added to 0.350 L of 0.500 M aqueous HBr. The solution that remains is...Problem 66E:
A fertilizer railroad car carrying 34,300 gallons of commercial aqueous ammonia (30% ammonia by...Problem 71E:
4.115 Federal regulations set an upper limit of 50 parts per million (ppm) of NH3 in the air in a...Problem 72E:
A mixture of gases A2 and B2 are introduced to a slender metal cylinder that has one end closed and...Problem 73E:
Practice Exercise 2 Calculate the change in the internal energy for a process in which a system...Problem 74E:
A solid sample of Zn(OH)2 is added to 0.350 L of 0.500 M aqueous HBr. The solution that remains is...Problem 75E:
Practice Exercise 2
Calculate the work, in J, if the volume of a system contracts from 1.55 to 0.85...Problem 76E:
Practice Exercise 1 A chemical reaction that gives off heat to its surroundings is said to be...Problem 80E:
Practice Exercise 1 When 0.243 g of Mg metal is combined with enough HCI to make 100 mL of solution...Problem 81E:
Practical exercise 2 When 50.0 mL of 0.100MAgNO3 and 50.0 mL of 0.100 M HCI are mixed in a...Problem 86E:
Calculate H for the reaction C(s)+ O2(g)CO(g)+H2(g) given the following thermochemical equations:...Problem 93AE:
Use the average bond enthalpies in Table 5.4 to estimate ∆H for the combustion of ethanol.
H...Problem 96AE:
One of the important ideas of thermodynamics is that energy can be transferred in the form of heat...Problem 97AE:
Two positively charged spheres, each with a charge of 2.0x10-5 C, a mass of 1.0 kg, and separated by...Problem 98AE:
SI The accompanying photo shows a pipevine swallowtail caterpillar climbing up a twig. As the...Problem 99AE:
Consider the accompanying energy diagram. Does this diagram represent an increase or decrease in the...Problem 100AE:
Write balanced net ionic equations for the reactions that occur in each of the following cases....Problem 101AE:
4.27 Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr,...Problem 107IE:
State whether each of the following statements is true or false. Justify your answer in each case....Problem 108IE:
State whether each of the following statements is true or false. Justify your answer in each case....Problem 109IE:
A textbook on chemical thermodynamics states, “The heat of solution represents the difference...Problem 112IE:
Complete and balance the following molecular equations, and then write the net ionic equation for...Browse All Chapters of This Textbook
Chapter 1 - Introduction: Matter, Energy, And MeasurementChapter 1.2 - Classifications Of MatterChapter 1.5 - Uncertainty In MeasurementChapter 1.6 - 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 CompoundsChapter 2.7 - Ions And Ionic Compounds
Chapter 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 - 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 - 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 EquilibriaChapter 15.5 - Calculating Equilibrium ConstantsChapter 15.6 - Applications Equilibrium ConstantsChapter 15.7 - Le Chatelier's PrincipleChapter 16 - Acid-base EquilibriaChapter 16.2 - Bronsted-lowry 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 EquilibriaChapter 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 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
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Chapter 1, Problem 1EWhen a charge particle comes in vicinity of another charge it gets either attracted or repelled by...Chapter 3, Problem 1EExplanation: It is better to use as few steps as possible because the lesser the number of steps,...Explanation: The chemical equation corresponds to the ΔGf0 means the equation in which only one mole...Explanation: A battery is a portable source of energy that contains one or more voltaic cells. They...Given The nuclear mass of B7e is 7.0147 amu . The nuclear mass of B9e is 9.0100 amu . The nuclear...The nomenclature of coordination compound is based on the certain rules which are written as, The...A molecule with weaker single bond is more reactive than a molecule with a stronger single bond...
Chapter 10, Problem 1DEThe important properties of the three isomers of hexanol are viscosity and volatility. Hydraulic...Chapter 12, Problem 1DEChapter 13, Problem 1DEChapter 14, Problem 1DEIn the designation of an orbital the number that is the principal quantum number n gives the shell...Chapter 16, Problem 1DEThe pKa of acetic acid is 4.74 and that of chloroacetic acid and trichloroacetic acid is 2.86 and...Explanation: GivenThe volume of helium inside the blimp is 5.74×106 L . The temperature of helium is...GivenThe volume of the gas is 1100.0 L . The temperature of gas is 280 °C . The mass of N2 gas is...Chapter 20, Problem 1DESolubility of any solute in a solvent depends upon the solute-solvent interaction. Greater the...Samples of five substances are given. The substances are NF3 , PF3 , PCl3 , PF5 and PCl5 . NF3 is a...The given reaction is, Cr(s)+3Ag+(aq)⇌Cr3+(aq)+3Ag(s) The equilibrium constant expression (Kc) for...Chapter 24, Problem 1DE
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