Solutions for CHEMISTRY:CENTRAL SCI.-W/ACCESS>CUSTOM<
Problem 1DE:
5.74 Using values from Appendix C, calculate the value of 24H° for each of the following...Problem 1E:
Complete combustion of 1 mol of acetone (C2H6O) liberates 1790 kJ: C3H6O(l) + 4O2(g) 3CO2(g) +...Problem 2E:
5.87 Consider the reaction 2H(g) + O2(g) 2H2O(l)
Use the bond enthalpies in Table 5.4 to...Problem 3E:
The air bags that provide protection in automobiles in the event of an accident expand because of a...Problem 4E:
5.111 From the following data for three prospective fuels, calculate which could provide the most...Problem 5E:
5.123 Consider two solutions, the first being 50.0 mL of 1.00 MCuSO4 and the second 50.0 mL of...Problem 6E:
For each of the following transitions, give the sign of E and indicate whether a photon is emitted...Problem 7E:
In this chapter, we have learned about the photoelectric effect and its impact on the formulation of...Problem 8E:
6.12 State where in the periodic table these elements appear
elements with the valence-shell...Problem 9E:
Einstein's 1905 paper on the photoelectric effect was the first important application of Planck's...Problem 10E:
5.48 Consider the decomposition of liquid benzene,C6H6(l) to gaseous acetylene, C2H2(g):
C6 H 6...Problem 11E:
Under constant-volume conditions, the heat of combustion of glucose (C6H12O6) is 15.57kJ/g. A 3...Problem 13E:
5.67
What is meant by the term standard conditions with reference to enthalpy changes?
What is...Problem 14E:
S
5.68
What is the value of the standard enthalpy of formation of an element in its most stable...Problem 15E:
For each of the following compounds, write a balanced thermochemical equation depicting the...Problem 16E:
Write balanced equations that describe the formation of the following compounds from elements in...Problem 17E:
The following is known as the thermite reaction: 2A1(s) + Fe2O3(s)Al2O3(s) + 2Fe(s) This highly...Problem 18E:
(a) What are the units usually used to express the rates of reactions occurring in solution? (b)...Problem 19E:
Using values from Appendix C , calculate the standard enthalpy change for each of the following...Problem 20E:
5.77 Gasoline is composed primarily of hydrocarbons, including many with eight carbon atoms,...Problem 22E:
Ethanol (C2H5OH) is blended with gasoline as an automobile fuel. Write a balanced equation for the...Problem 23E:
5.80 Methanol (CH3OH) is used as a fuel in race cars.
Write a balanced equation for the...Problem 25E:
5.82 Without doing any calculations, predict the sign of for each of the following reactions:
2...Problem 26E:
Use bond enthalpies in Table 5.4 Q to estimate for each of the following reactions: a. H - H(g) + Br...Problem 27E:
Use bond enthalpies in Table 5.40 to estimate for each of the following reactions: a. b.Problem 28E:
Use enthalpies of formation given in Appendix C to calculate for the reaction Br2(g) 2 Br(g), and...Problem 29E:
5.86
The nitrogen atoms in an N2 molecule are held together by a triple bond; use enthalpies of...Problem 30E:
5.89
What is meant by the term fuel value?
Which is a greater source of energy as food, 5 g of fat...Problem 31E:
5.90
Which releases the most energy when metabolized, 1 g of carbohydrates or 1 g of fat?
A...Problem 32E:
5.91
A serving of a particular ready-to-serve chicken noodle soup contains 2.5 g fat, 14 g...Problem 33E:
5.92 A pound of plain M&M® candies contains 96 g fat, 320 g carbohydrate, and 21 g protein. What...Problem 34E:
5.93 The heat of combustion of fructose, C6H12O6, is — 2812kJ/mol. If a fresh golden delicious...Problem 35E:
5.94 The heat of combustion of ethanol, C2H5OH(l), is — 1367Wmol. A batch of Sauvignon Blanc wine...Problem 36E:
5.95 The standard enthalpies of formation of gaseous propyne (C3H4), propylene (C3H6), and propane...Problem 37E:
5.98 It is interesting to compare the ‘fuel value’ of a hydrocarbon in a hypothetical world where...Problem 38E:
At the end of 2012, global population was about 7.0 billion people. What mass of glucose in kg would...Problem 40E:
(a) For a generic second-order reaction, what quantity, when graphed versus time, will yield a...Problem 41E:
A sample of gas is contained in a cylinder-and-piston arrangement it undergoes the change in state...Problem 42E:
Limestone stalactites and stalagmites are formed in caves by the following reaction: Ca2+ (aq)...Problem 43E:
Consider the systems shown in Figure 5.10. In one case the battery becomes completely discharged by...Problem 44E:
5.105 A house is designed to have passive solar energy features. Brickwork incorporated into the...Problem 45E:
5.108 A coffee-cup calorimeter of the type shown in Figure 5.18 contains 150.0 g of water at 25.1...Problem 46E:
5.107
When a 0.235-9 sample of benzoic acid is combusted in a bomb calorimeter (Figure 5.19), the...Problem 47E:
5.108 Meals-ready-to-eat (MREs) are military meals that can be heated on a flameless heater. The...Problem 48E:
5.109 Burning methane in oxygen can produce three different carbon-containing products: soot (very...Problem 50E:
Ammonia (NH3) boils at -33 °C; at this temperature it has a density of 0.81 g/cm3. The enthalpy of...Problem 53E:
5.116 TheSun supplies about 1.0 kilowatt of energy for each square meter of surface area (
1.0...Problem 54E:
5.117 Itis estimated that the net amount of carbon dioxide fixed by photosynthesis on the landmass...Problem 55E:
5.118 At 20 °C (approximately room temperature) the average velocity of N2molecules in air is 1050...Problem 56E:
Suppose an Olympic diver who weighs 52.0 kg executes a straight dive from a 10-m platform. At the...Problem 57E:
5.120 Consider the combustion of a single molecule of CH4 (g), forming H20(l) as a product.
How...Problem 58E:
5.121 Consider the following unbalanced oxidation-reduction reactions in aqueous solution:
Ag+(aq)...Problem 59E:
Consider the following acid-neutralization reactions involving the strong base NaOH(aq): HNO3(aq) +...Problem 60E:
5.125 A sample of a hydrocarbon is combusted completely in O2(g) to produce 21.83 g CO2(g), 4.47 g...Problem 61E:
5.126 The methane molecule, CH4, has the geometry shown in Figure 2.17 . Imagine a hypothetical...Problem 62E:
5.127 One of the best-selling light, or low-calorie, beers is 4.2% alcohol by volume and a 12-oz...Problem 63E:
A source of electromagnetic radiation produces infrared light. Which of the following could be the...Problem 65E:
Consider the following three statements: For any electromagnetic radiation, the product of the...Problem 68E:
A laser emits light that has a frequency of 4.69 x 1014 s 1. What is the energy of one photon of...Problem 70E:
Calculate the velocity of a neutron whose de Broglie wavelength is 505 pm. The mass of a neutron is...Problem 71E:
An orbital has n = 4 and ml = 0, 1, 2, 3 -3, - 2, - 1, 0, 1, 2, 1, 2, 3 -3, -2 1, 2, 3, 4 - 1. What...Problem 72E:
What is the designation for the subshell with = 5 and 1 = 1?
How many orbitals are in this...Problem 73E:
How many of the elements in the second row of the periodic table (Li through Ne) will have at least...Problem 74E:
Write the electron configuration for silicon, element 14, in its ground state. How many unpaired...Problem 75E:
A certain atom has an ns2np2electron configuration in its outermost occupied shell. Which of the...Problem 76E:
Which group of elements is characterized by an ns2np2 electron configuration in the outermost...Problem 80E:
6.2 A popular kitchen appliance produces electromagnetic radiation with a frequency of 2450 MHz....Problem 81E:
6.3 The following diagrams represent two electromagnetic waves. drawn on the same scale. a Which...Problem 82E:
6.4 Stars do not all have the same temperature. The color of light emitted by stars is...Problem 83E:
6 5 The familiar phenomenon of a rainbow results from the diffraction of sunlight through raindrops...Problem 84E:
6.7 A certain quantum mechanical system has the energy levels shown in the accompanying diagram....Problem 85E:
Consider the three electronic transitions in a hydrogen atom shown here, labeled A, B, and C. Three...Problem 87E:
6.9 The contour representation of one of the orbitals for the n = 3 shell of a hydrogen atom is...Problem 88E:
6.10 The accompanying drawing shows a contour plot for a dyz orbital. Consider the quantum numbers...Problem 89AE:
8.11 Four possible electron configurations for a nitrogen atom are shown below, but only one...Problem 90AE:
6.14
a What is the relationship between the wavelength and the frequency of radiant energy?
b Ozone...Problem 91AE:
Label each of the following statements as true or false. For those that are false, correct the...Problem 92AE:
Determine which of the following statements are false and correct them. The frequency of radiation...Problem 93AE:
Arrange the following kinds of electromagnetic radiation in order of increasing wavelength:...Problem 94AE:
List the following types of electromagnetic radiation in order of increasing wavelength: the gamma...Problem 95AE:
What is the frequency of radiation that has a wavelength of 10kma, about the size of a bacterium?...Problem 96AE:
What is the frequency of radiation whose wavelength is 0.86 nm? What is the wavelength of radiation...Problem 97AE:
A laser pointer used in a lecture hall emits light at 650 nm. What is the frequency of this...Problem 99AE:
If human height were quantized in 1-foot increments, what would happen to the height of a child as...Problem 100AE:
A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in Figure 6.4....Problem 101AE:
The complete combustion of ethanol, C2H5OH(l), to formH20(g) and CO2{g) at constant pressure...Problem 102AE:
The decomposition of Ca(OH)2(s) into CaO(s) and H20(g) at constant pressure requires the addition of...Problem 104AE:
5.42 Without referring to tables, predict which of the following has the higher enthalpy in each...Problem 105AE:
Consider the following reaction: 2 Mg(s) + 02(g)2 MgO(s) H-1204 kJ Is this reaction exothermic or...Problem 106AE:
544 Consider the following reaction:
2 CH3OH(g)→2CH4 (g) + 02(g) = + 252.8 kJ
a. Is this reaction...Problem 107AE:
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates Ag+...Problem 108AE:
At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat...Problem 110AE:
5.49
a What are the units of molar heat capacity?
What are the units of specific heat?
If you know...Problem 111AE:
Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of...Problem 112AE:
What is the specific heat of liquid water? What is the molar heat capacity of liquid water? What is...Problem 113AE:
5.52
a. Which substance in Table 5.2 requires the smallest amount of energy to increase the...Problem 114AE:
The specific heat of octane, C8H18(l), is 2.22 J/g-K. How many J of heat are needed to raise the...Problem 115AE:
6.54 Consider the data about gold metal in Exercise 5.26(b).
a. Based on the data, calculate the...Problem 116AE:
When a 6-50-g sample of solid sodium hydroxide dissolves in 100 0 g of water in a coffee-cup...Problem 117IE:
5.56
a. When a 4 25-g sample of solid ammonium nitrate dissolves in 60 0 g of water in a coffee-cup...Problem 118IE:
A 2.200-g sample of quinone (C5H402) is burned in a bomb calorimeter whose total heat capacity is...Problem 119IE:
8.68 A 1.800-g sample of phenol (C6H5OH) was burned in a bomb calorimeter whose total heat capacity...Problem 120IE:
5.60 Under constant-volume conditions, the heat of combustion of benzoic acid (C6H5COOH) is 26.38...Problem 121IE:
5.61 Can you use an approach similar to Hess's law to calculate the change in internal energy, E,...Problem 122IE:
5.62 Consider the following hypothetical reactions:
A B = + 30 kJ
B C = + 60 kJ
Use...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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13th Edition
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