Chemistry: Atoms First V11st EditionBurdge Publisher: McGraw Hill CustomISBN: 9781259383120
Chemistry: Atoms First V1
Solutions for Chemistry: Atoms First V1
Problem 1.1WE:
illustrates conversions between these two temperature scales. Worked Example 1.1 Normal human body...Problem 1PPB:
According to the website of the National Aeronautics and Space Administration (NASA), the average...Problem 1PPC:
If a single degree on the Celsius scale is represented by the rectangle on the left, which of the...Problem 1.2WE:
A body temperature above 39C constitutes a high fever. Convert this temperature to the Fahrenheit...Problem 2PPA:
The average temperature at the summit of Mt. Everest ranges from 36C during the coldest month...Problem 2PPC:
If a single degree on the Fahrenheit scale is represented by the rectangle oil the left, which of...Problem 3PPA:
Given that 20.0 mL of mercury has a mass of 272 g. calculate (a) the density of mercury and (b) the...Browse All Chapters of This Textbook
Chapter 1 - Chemistry: The Science Of ChangeChapter 1.4 - Scientific MeasurementChapter 1.5 - Uncertainty In MeasurementChapter 1.6 - Using Units And Solving ProblemsChapter 2 - Atoms And The Periodic TableChapter 2.3 - Atomlc Number, Mass Number, And IsotopesChapter 2.4 - Nuclear StabilityChapter 2.5 - Average Atomlc MassChapter 2.6 - The Periodic TableChapter 2.7 - The Mole And Molar Mass
Chapter 3 - Quantum Theory And The Electronic Structure Of AtomsChapter 3.1 - Energy And Energy ChangesChapter 3.2 - The Nature Of LightChapter 3.3 - Quantum TheoryChapter 3.4 - Bohr's Theory Of The Hydrogen AtomChapter 3.5 - Wave Properties Of MatterChapter 3.6 - Quantum MechanicsChapter 3.7 - Quantum NumbersChapter 3.8 - Atomic OrbitalsChapter 3.9 - Electronic ConfigurationsChapter 3.10 - Electronic Configurations And The Periodic TableChapter 4 - Periodic Trends Of ElementsChapter 4.1 - Development Of The Periodic TableChapter 4.2 - The Modern Periodic TableChapter 4.4 - Periodic Trends In Properties Of ElementsChapter 4.5 - Electron Configuration Of IonsChapter 4.6 - Ionic RadiusChapter 5 - Ionic And Covalent CompoundsChapter 5.2 - Lewis Dot SymbolsChapter 5.3 - Ionic Compounds And BondingChapter 5.4 - Naming Ions And Ionic CompoundsChapter 5.5 - Covalent Bonding And MoleculesChapter 5.6 - Naming Molecular CompoundsChapter 5.7 - Covalent Bonding In Ionic SpeciesChapter 5.8 - Molecular And Formula MassesChapter 5.9 - Percent Composition Of CompoundsChapter 5.10 - Molar MassChapter 6 - Representing MoleculesChapter 6.2 - Electronegativity And PolarityChapter 6.3 - Drawing Lewis StructuresChapter 6.4 - Lewis Structures And Formal ChargeChapter 6.5 - ResonanceChapter 6.6 - Exceptions To The Octet RuleChapter 7 - Molecular Geometry, Intermolecular Forces, And Bonding TheoriesChapter 7.1 - Molecular GeometryChapter 7.2 - Molecular Geometry And PolarityChapter 7.3 - Intermolecular ForcesChapter 7.4 - Valence Bond TheoryChapter 7.5 - Hybridization Of Atomic OrbitalsChapter 7.6 - Hybridization In Molecules Containing Multiple BondsChapter 7.7 - Molecular Orbital TheoryChapter 7.8 - Bonding Theories And Descriptions Of Molecules With Delocalized BondingChapter 8 - Chemical ReactionsChapter 8.1 - Chemical EquationsChapter 8.2 - Combustion AnalysisChapter 8.3 - Calculations With Balanced Chemical EquationsChapter 8.4 - Limiting ReactantsChapter 9 - Chemical Reactions In Aqueous SolutionsChapter 9.1 - General Properties Of Aqueous SolutionsChapter 9.2 - Precipitation ReactionsChapter 9.3 - Acid-base ReactionsChapter 9.4 - Oxidation-reduction ReactionsChapter 9.5 - Concentration Of SolutionsChapter 9.6 - Aqueous Reactions And Chemical AnalysisChapter 10 - Energy Changes In Chemical ReactionsChapter 10.1 - Energy And Energy ChangesChapter 10.2 - Introduction To ThermodynamicsChapter 10.3 - EnthalpyChapter 10.4 - CalorimetryChapter 10.5 - Hess's LawChapter 10.6 - Standard Enthalpies Of FormationChapter 10.7 - Bond Enthalpy And The Stability Of Covalent MoleculesChapter 10.8 - Lattice Energy And The Stability Of Ionic SolidsChapter 11 - GasesChapter 11.2 - The Kinetic Molecular Theory Of GasesChapter 11.3 - Gas PressureChapter 11.4 - The Gas LawsChapter 11.5 - The Ideal Gas EquationChapter 11.6 - Real GasesChapter 11.7 - Gas MixturesChapter 11.8 - Reactions With Gaseous Reactants And ProductsChapter 12 - Liquids And SolidsChapter 12.2 - Properties Of LiquidsChapter 12.3 - The Properties Of SolidsChapter 12.4 - Types Of Crystalline SolidsChapter 12.5 - Phase ChangesChapter 12.6 - Phase DiagramsChapter 13 - Physical Properties Of SolutionsChapter 13.2 - A Molecular View Of The Solution ProcessChapter 13.3 - Concentration UnitsChapter 13.4 - Factors That Affect SolubilityChapter 13.5 - Colligative PropertiesChapter 13.6 - Calculations Using Colligative PropertiesChapter 14 - Entropy And Free EnergyChapter 14.3 - Entropy Changes In A SystemChapter 14.4 - Entropy Changes In The UniverseChapter 14.5 - Predicting SpontaneityChapter 15 - Chemical EquilibriumChapter 15.2 - The Equilibrium ConstantChapter 15.3 - Equilibrium ExpressionsChapter 15.4 - Chemical Equilibrium And Free EnergyChapter 15.5 - Calculating Equilibrium ConcentrationsChapter 15.6 - Le Chatelier's Principle: Factors That Affect EquilibriumChapter 16 - Acids, Bases, And SaltsChapter 16.1 - Bronsted Acids And BasesChapter 16.2 - Molecular Structure And Acid StrengthChapter 16.3 - The Acid-base Properties Of WaterChapter 16.4 - The Ph And Poh ScalesChapter 16.5 - Strong Acids And BasesChapter 16.6 - Weak Acids And Acid Ionization ConstantsChapter 16.7 - Weak Bases And Base Ionization ConstantsChapter 16.8 - Conjugate Acid-base PairsChapter 16.9 - Diprotic And Polyprotic AcidsChapter 16.10 - Acid-base Properties Of Salt SolutionsChapter 16.12 - Lewis Acids And BasesChapter 17 - Acid-base Equilibria And Solubility EquilibriaChapter 17.1 - The Common Ion EffectChapter 17.2 - Buffer SolutionsChapter 17.3 - Acid-base TitrationsChapter 17.4 - Solubility EquilibriaChapter 17.5 - Factors Affecting SolubilityChapter 17.6 - Separation Of Ions Using Differences In SolubilityChapter 18 - ElectrochemistryChapter 18.1 - Balancing Redox ReactionsChapter 18.3 - Standard Reduction PotentialsChapter 18.4 - Spontaneity Of Redox Reactions Under Standard-state ConditionsChapter 18.5 - Spontaneity Of Redox Reactions Under Conditions Other Than Standard-stateChapter 18.7 - ElectrolysisChapter 19 - Chemical KineticsChapter 19.3 - Measuring Reaction Progress And Expressing Reaction RateChapter 19.4 - Dependence Of Reaction Rate On Reactant ConcentrationChapter 19.5 - Dependence Of Reactant Concentration On TimeChapter 19.6 - Dependence Of Reaction Rate On TemperatureChapter 19.7 - Reaction MechanismsChapter 20 - Nuclear ChemistryChapter 20.1 - Nuclei And Nuclear ReactionsChapter 20.2 - Nuclear StabilityChapter 20.3 - Natural RadioactivityChapter 20.4 - Nuclear TransmutationChapter 21 - Metallurgy And The Chemistry Of MetalsChapter 22 - Coordination ChemistryChapter 22.1 - Coordination CompoundsChapter 22.3 - Bonding In Coordination Compounds: Crystal Field TheoryChapter 23 - Organic ChemistryChapter 23.2 - Classes Of Organic CompoundsChapter 23.3 - Representing Organic MoleculesChapter 23.5 - Organic ReactionsChapter 24 - Modern MaterialsChapter 24.1 - PolymersChapter 24.3 - Liquid CrystalsChapter 24.6 - Semiconductors
Sample Solutions for this Textbook
We offer sample solutions for Chemistry: Atoms First V1 homework problems. See examples below:
Given the coldest temperature as -128.6°F Conversion of oF into oC: oC = (oF - 32oF) × 5oC9oF =...Given that there are 100 oranges in a box and the average weight of an orange is 7.2 ounces The...Study of matter and changes which the matter undergoes is chemistry. In chemistry we study about...Chapter 1, Problem 1.9QPChapter 1, Problem 1.19QPExplanation: Convert the given temperature into degree Celsius unit Given temperature is 95 oF...Explanation: Convert the given temperature into degree Celsius unit Given temperature is 105 oF...Qualitative properties: These are the properties observed and can’t be measured with the numerical...Explanation To determine: density of the pheromone s To determine the density of the pheromone s,...
Explanation: The threshold level is given in the units of micrograms per deciliter (10μg /dL) and...Chapter 1, Problem 1.111QPExplanation The conversional formula from Celsius to Fahrenheit is Fo = (oC×9oF5oC)+ 32Fo It is...Explanation: Given, The given storage temperature of cidofovir is 680 F − 770 F Conversional...Chapter 1, Problem 1.116QPExplanation: Calculate the mass of dozen plain and jam-filled doughnuts: Given: Average Mass of...Chapter 2, Problem 2.1QPChapter 2, Problem 2.22QPChapter 2, Problem 2.38QPExplanation: The atomic mass of 24Mg is given below, Average atomic mass= ∑(Mass of isotope ×...Explanation: To Identify: The symbols for each atom to be identified. The element symbol :...Explanation: Identify the symbol of an element. The element symbol : ZAX,Z (atomic number) = no. of...Explanation: Predict the number of protons and neutrons of each atom. The element symbol :...Chapter 2, Problem 2.77QPExplanation: Every atom contains a nucleus in which all of its positive charge and most of its mass...Explanation: (i) The electrostatic energy between two charges is calculated using the formulae: Eel...Chapter 3, Problem 3.1QPTo find: Determine the kinetic energy of a 25-kg mass moving at 61.3 m/s Kinetic energy (in joule)...To find: Determine the velocity of Ne atom that has Ek= 1.12 × 10-20 J Kinetic energy (in joule) is...To find: Determine the velocity of an electron that have Ek= 3.41 × 10-21 J. Kinetic energy (in...Chapter 3, Problem 3.44QPChapter 3, Problem 3.96QPChapter 3, Problem 3.97QPChapter 3, Problem 3.98QPChapter 3, Problem 3.102QPChapter 3, Problem 3.103QPChapter 3, Problem 3.104QPChapter 3, Problem 3.116QPChapter 3, Problem 3.117QPChapter 3, Problem 3.123QPChapter 3, Problem 3.128QPChapter 3, Problem 3.133QPChapter 4.4, Problem 4.6WEChapter 4.4, Problem 6PPBChapter 4.5, Problem 7PPAChapter 4, Problem 4.1QPExplanation: Valence electron of the atom is the total number of electrons that is present in the...Explanation: Since only the valence electrons involve in bonding, electrons present in the outermost...Explanation Electronic configuration of Li atom is, 1s22s1 The electronic configuration of Li is...Explanation: Electronic configuration of Rb 1s22s22p63s23p64s23d104p65s1 The electronic...Chapter 4, Problem 4.71QPExplanation: Electronic configuration of Sc is, 1s22s22p63s23p64s23d1 The electronic configuration...Explanation: Electronic configuration of Ni is, 1s22s22p63s23p64s23d8 The electronic configuration...Chapter 4, Problem 4.74QPExplanation: Electronic configuration of Ar is, 1s22s22p63s23p6 The electronic configuration of Ar...Chapter 4, Problem 4.78QPChapter 4, Problem 4.79QPChapter 4, Problem 4.84QPChapter 4, Problem 4.85QPChapter 4, Problem 4.89QPExplanation: Predict the Formula. a) Name : Mercury(II) chloride. Cation: Mercury Anion:...Explanation: Predict the Formula. a) Name : Potassium dichromate. Cation: Potassium Anion:...Explanation: Molar mass of water is given below Molar mass of hydrogen = 1.00794 g/mol. Molar mass...Chapter 5, Problem 5.1QPChapter 5, Problem 5.6QPExplanation: The electronic configuration of Bromine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5. Lewis dot...Explanation: K3PO4 has three K+ ion and one PO43- ion. Here anion contains expected number of oxygen...Explanation: KClO has one K+ ion and one ClO- ion. Here anion contains two less oxygen than expected...Explanation: Molecular formula is given as C6H6O Molecular mass of C6H6O = 6(mass of C in amu) +...Explanation: Molecular mass of CH3Cl = 1(mass of C in amu) + 3(mass of H in amu) + 1(mass of Cl in...To calculate: Molecular mass of Li2CO3 Molecular formula is given as Li2CO3 Molecular mass of Li2CO3...To calculate: Molecular mass of CH4 Molecular formula is given as Molecular mass of CH4 = (mass of C...Explanation: Percent composition by mass: percent composition by mass of each element present in a...Explanation: Percent composition by mass: percent composition by mass of each element present in a...Explanation: Percent composition by mass: percent composition by mass of each element present in a...Explanation: Percent composition by mass: Percent composition by mass of each element present in a...Percent composition by mass: Percent composition by mass of each element present in a compound is...Chapter 5, Problem 5.79QPExplanation: Partial charges are the magnitude of charges Given, μ = 0.82 Dr = 1.41 A0 μ= Q × r The...Explanation: Given Lewis structure A formal charge (FC) is the charge assigned to an atom in a...Chapter 6.6, Problem 10PPAExplanation: Covalent Bonding In covalent bonding the atoms share electrons equally, it means both...The electronegativity difference range is used to find whether the given bond is ionic, non-polar...The electronegativity difference range is used to find whether the given bond is ionic, non-polar...The given molecule contains one nitrogen atom and two oxygen atom with it. The Nitrogen has totally...Chapter 6, Problem 6.35QPThe given atomic arrangement of diazomethane is CH2N2. Resonance structure of hydrazoic acid is...Resonance structure of PO2F2 − ion is drawn below. In the case of PO2F2 −, the chemical bonding of a...Chapter 6, Problem 6.83QPChapter 6, Problem 6.92QPExplanation: (a) Given, Q = 0.19 e −1r = 213 pm μ= Q × r The partial charges are + 0.19 e− and −...Chapter 6, Problem 6.97QPExplanation 1: Molecular geometry is the spatial arrangement of atoms on a molecule and/ or ions. It...Explanation: To predict: The geometry for the given molecule. Draw the Lewis structure for the...Chapter 7, Problem 7.7QPExplanation: To predict: The geometry for the given molecule. Draw the Lewis structure for the...Chapter 7, Problem 7.9QPChapter 7, Problem 7.10QPChapter 7, Problem 7.31QPChapter 7, Problem 7.37QPExplanation: Tetrahedral A molecule having tetrahedral geometry has the empirical formula AB4 which...Chapter 7, Problem 7.61QPExplanation: The given molecular formulas were recorded as shown above. To calculate hybridization...Chapter 7, Problem 7.103QPChapter 7, Problem 7.105QPChapter 7, Problem 7.129QPChapter 7, Problem 7.138QPChapter 7, Problem 7.143QPExplanation: The mass of nitrous oxide is given as 10 g. Equation for Number of moles of a...Chapter 8.4, Problem 8.7WEFormation of water takes place by the combination of hydrogen and oxygen. Chemical reaction is a...Explanation: List the atoms of given equation and also the number of each atoms present on both...Chapter 8, Problem 8.9QPChapter 8, Problem 8.37QPExplanation: The mass of products should be equal to mass of its starting materials this is governed...Explanation: The mass of products should be equal to mass of its starting materials this is governed...Explanation: To calculate the number of moles of O3 and NO Number of moles of NO2= 0.740g O3 × 1 mol...Chapter 8, Problem 8.66QPExplanation: In given reaction, Mixture of CH4 and C2H6 are burned in O2. Therefore, The chemical...Explanation: In the given reactions, Octane ( C8H18) undergoes complete as well incomplete...Explanation: In given reaction diagram, 2 molecules of ClF3 reacts with two molecules of NH3 to form...The given compound Ba(C2H3O2)2 contains Ba2+ ions together with acetate ions which makes the...Explanation: The give metals from top to bottom in decreasing order of oxidation. The given...Explanation: The molarity of 5.00 L solution contains 235 g of sucrose, Molar mass of the sucrose is...Explanation: To calculate the required volumes of stock solutions to prepare the final diluted...Explanation: The balanced equation is, Na2SO4→2 Na+(aq)+SO42−(aq) 1 mole SO42-in Na2SO4 [SO42-]=...Chapter 9.6, Problem 15PPBExplanation: The required volume of 0.203 M NaOH to neutralize the 25.0 mL of a 0.188 M H2SO4...Chapter 9, Problem 9.1QPExplanation: According to the solubility guideline, CaCO3 is contains carbonate ion so it is...Explanation: The balanced equation for reaction of FeCl3(aq) and LiOH(aq) is,...Explanation: The ionic compounds are dissolved in water to produced ions these ions are combined to...Explanation: The ionic compounds are dissolved in water to produced ions these ions are combined to...Explanation: The oxidation number of Sulfur in H2S In H2S there is one Sulfur, two Hydrogen atoms....Chapter 9, Problem 9.47QPChapter 9, Problem 9.48QPExplanation: The oxidation number of Cs in Cs2O According to the rules, the sum of oxidation numbers...Given, Record the given data, The molarities for solutions are 0.100 M The volumes for solution are...Chapter 9, Problem 9.89QPExplanation: Record the given data, Concentration of NaOH= 1.015 M Volume of HCl solution = 25.00 mL...Chapter 9, Problem 9.125QPExplanation: Describe the preparation of Magnesium hydroxide and predict and it solubility in water...Chapter 9, Problem 9.146QPExplanation: To record the given data, Taken mass KMnO4 of in first dilution = 0.8214 g Final Volume...Chapter 9, Problem 9.167QPChapter 9, Problem 9.168QPChapter 10.3, Problem 2PPBExplanation: The thermochemical equation can be given as, 12H2+12Cl2→HCl ΔH°reaction=-92.3 kJ...Chapter 10, Problem 10.1QPGiven, Record the given info Initial volume = 1.6 L Final volume = 5.4L Calculate the work done...Given, Record the given info Initial volume = 26.7m L Final volume = 89.3mL Calculate the work done...Explanation: To calculate the ΔH°reaction for the first equation Two moles of Graphite are needed;...Chapter 10, Problem 10.77QPExplanation: ΔH°f[Li(g)]=159.3 kJ mol-1 ΔH°f[Cl(g)]=121.7 kJ mol-1IE(1)(Li)=520 kJ...Explanation: ΔH°f[Ca(g)]=179.3 kJ mol-1 ΔH°f[Cl(g)]=121.7 kJ mol-1IE1(Ca)=590 kJ mol-1IE2(Ca)=1145...Chapter 10, Problem 10.88QPExplanation: Lithium hydroxide reacts with Carbon dioxide to give Lithium carbonate (soluble...Explanation: Record the given data Volume and Molarity of Silver Nitrate = 50.0 mL & 0.100 M...Explanation: The change in enthalpy that is associated with the formation of one mole of a substance...Chapter 10, Problem 10.130QPExplanation: The chemical equations can be given, C6H6(l)+152O2(g)→6CO2(g)+3H2O(l) ΔH°=-3267.4 kJ...Explanation: The energy that is necessary to break up the F2- into an F and an F- atom is the bond...Chapter 10, Problem 10.137QPExplanation: To calculate the moles of H2O Mass of Water = 500 g Moles of Water = 500 g×1 mol...Explanation: Calcium carbide upon reaction with Water gives Calcium hydroxide and Acetylene. The...Chapter 10, Problem 10.158QPExplanation: (a) To determine: The pressure of the gas calculated using the ideal gas equation The...Explanation: Given, The total pressure is 5.78 atm The mole fraction and partial pressure of CO2,...Explanation: To differentiate of Diffusion and Effusion. Diffusion is the dispersal of molecules of...Record the given data Mass of N2 is 14.01 g/mole Mass of O2 is 16.00 g/mole The Mass of O2 , and...Record the given data Given pressure is 375 mmHg 1 atm = 101.325 Pa Given pressure 375 mmHgis...Explanation: First, we calculate the mole fraction Methane from the mixture. Then, we can calculate...Explanation: (a) Dalton’s law states that the total pressure of the mixture is the sum of the...Explanation: (a). χN2 = 0.7808 χO2 = 0.2094 χAr = 0.0093χCO2 = 0.0005 PN2= 0.781 atm, PO2 = 0.209...To calculate the moles of the compound. n =PVRTn = (97.3 mmHg × 1 atm760 mmHg)(0.378 L)(0.0821L ....Explanation: To calculate the moles of the metal consumed in the reaction mol M = 0.225 g M × 1 mol...NH3(g) + HCl(g) → NH4Cl(s) To determine the moles of each reactant ?mol NH3 = 73.0 g NH3 × 1 mol NH3...Chapter 11, Problem 11.89QPTo calculate the moles Nitro-glycerine You can map out the following strategy to solve for the total...Explanation: To calculate the initial number of moles of O2 and NO nNO = PNOVRT = (0.500 atm) (4.00...Chapter 11, Problem 11.110QPExplanation: Calculate the moles of CO2 produced using the ideal gas equation. We carry an extra...Explanation: This is a Boyle’s law problem, pressure and volume vary. Suppose that the pressure at...Chapter 11, Problem 11.126QPExplanation: To calculate the moles of water vapour per liter using the ideal gas equation P =nRTV...Chapter 12.4, Problem 5PPCChapter 12, Problem 12.1QPExplanation: Sodium is a highly electropositive metal and Oxygen is a highly electronegative...Chapter 12, Problem 12.26QPExplanation: Record the given data: edge length of unit cell = 287 pmdensity of Iron = 7.87 g/cm3...Chapter 12, Problem 12.29QPChapter 12, Problem 12.31QPChapter 12, Problem 12.32QPExplanation: CO2 is a non-polar covalent compound. Non-polar covalent compounds have weak London...Calculate the heat required to warm ice to melting point. given data: mass of ice, m = 866 gspecific...Chapter 12, Problem 12.110QPChapter 12, Problem 12.114QPChapter 12, Problem 12.120QPChapter 12, Problem 12.123QPChapter 12, Problem 12.132QPExplanation: Calculation of number of moles of glucose solution 170.1g180.2g/mol= 0.9440 mol By...Chapter 13.5, Problem 13.6WEExplanation: To explain difference between saturated, unsaturated and supersaturated solution...Given, Amount of urea((NH2)2CO) = 5.00 gPercent by mass of soultion = 16.2 % The amount of water...Given, Strength of NaCl = 2.55 MDensity of NaCl solution = 1.08 g/mLMolecular mass of NaCl= 58.4...Given, Strength of sugar solution = 1.22 MDensity of sugar solution = 1.12g /mLMolecular weight of...For molarity of sulfuric acid: Given, Mass percent of Sulphuric acid = 98 %Density of Sulphuric acid...Given, Mass of solute(NH3) = 35.0 gMass of solvent(water) = 75.0 g = 0.075 kgDensity of the solution...The molality of ethanol (C2H5OH) solution is calculated. Given, Mass percent of ethanol in aqueous...Chapter 13, Problem 13.60QPChapter 13, Problem 13.67QPExplanation: Explanation of CaCl2 solution has higher boiling point than urea CaCl2 is an ionic...Chapter 13, Problem 13.79QPChapter 13, Problem 13.94QPChapter 13, Problem 13.106QPChapter 13, Problem 13.138QPChapter 13, Problem 13.141QPExplanation: Given data Molar mass of liquid A = 100g/mol Molar mass of liquid B = 110g/mol Vapour...Chapter 14.3, Problem 2PPBExplanation: Given, S°(Na(s))=51.05JK-1mol-1S°(Na(l))=57.56 JK-1mol-1 ΔΗf°(Na(s) )=0ΔΗf°(Na(l) )=...Chapter 14, Problem 14.1QPExplanation: To record the given data The number of particles in the system, N=10 The degeneracy of...Chapter 14, Problem 14.15QPChapter 14, Problem 14.20QPChapter 14, Problem 14.21QPChapter 14, Problem 14.22QPChapter 14, Problem 14.23QPChapter 14, Problem 14.47QPChapter 15.2, Problem 1PPAChapter 15.3, Problem 15.4WEChapter 15.3, Problem 6PPAChapter 15.4, Problem 10PPBChapter 15.5, Problem 15.12WETo Identify: Given the equilibrium reactions addition, removal of (A2and B2) should be analysed....Chapter 15, Problem 15.1QPChapter 15, Problem 15.60QPChapter 15, Problem 15.62QPChapter 15, Problem 15.89QPChapter 15, Problem 15.95QPExplanation: To find: The equilibrium reaction should be identified given the statement. Analyze the...Chapter 15, Problem 15.104QPChapter 15, Problem 15.111QPExplanation: (a) and (b) Let us consider the following standard free energy equation ΔG0 =-RTln...Chapter 15, Problem 15.121QPChapter 15, Problem 15.132QPChapter 15, Problem 15.133QPChapter 15, Problem 15.137QPChapter 15, Problem 15.145QPChapter 15, Problem 15.155QPChapter 15, Problem 15.156QPChapter 15, Problem 15.1KSPChapter 15, Problem 15.2KSPChapter 16.1, Problem 2PPAExplanation: Given data: The pOH of the given solution is 13.02 Calculation of hydroxide ion [OH-] :...Chapter 16.5, Problem 16.7WEChapter 16.5, Problem 8PPAChapter 16.6, Problem 12PPAChapter 16.7, Problem 16.15WEChapter 16.10, Problem 19PPAChapter 16, Problem 16.1QPExplanation: (a) To classify: H2O as Bronsted acid or base, or both. To identify the species as...Explanation: Given Concentration of H3O+ = 1.13 × 10−4 M Formula Kw = [H3O+][OH−] = 1.0 × 10−14...Explanation: Given Concentration of OH- = 2.50× 10−2 M Formula Kw = [H3O+][OH−] = 1.0 × 10−14 [H3O+]...Explanation: Given Concentration of H3O+ = 1.13 × 10−4 M Formula Kw = [H3O+][OH−] = 5.84 × 10−14 at...Explanation: Given Concentration of OH- = 2.50× 10−2 M Formula Kw = [H3O+][OH−] = 5.13 × 10−13 at...Chapter 16, Problem 16.54QPChapter 16, Problem 16.55QPExplanation: Record the given data A 0.10-M solution of ammonia at 25 oC . From the concentration...Explanation: A simple relationship between the ionization constant of a weak acid ( Ka ) and the...Explanation: CN- is the conjugate base of weak acid HCN , The acid ionization constant Ka of acid...Chapter 16, Problem 16.78QPExplanation: Record the given datas The concentration of H2CO3 solution is 0.025 M H2CO3 is a weak...Chapter 16, Problem 16.97QPExplanation: Record the given datas CH3COOH(aq)+NO2- → CH3COO-(aq)+HNO2(aq) From the given data, we...Chapter 16, Problem 16.147QPExplanation: Given data: The concentration of H3PO4 solution is 0.100 M Species of H3PO4 H3PO4 is a...Explanation: Given data: The concentration of Na2CO3 solution is 0.100 M Ionization of Na2CO3 Na2CO3...Chapter 16, Problem 16.166QPTo calculate: The pH of buffer solution (NaF+ HF). Given, Molarity of HF = 0.76 Mmolarity of NaF =...Chapter 17.3, Problem 4PPAExplanation: The solubility product constant of ( Ag2SO3 ) is calculated below. The equilibrium of...Chapter 17.5, Problem 10PPBChapter 17, Problem 17.1QPChapter 17, Problem 17.5QPChapter 17, Problem 17.6QPChapter 17, Problem 17.10QPChapter 17, Problem 17.16QPExplanation: Amount of monoprotic acid is 0.1276 g Concentration of NaOH is 0.0633 M Calculate the...Explanation: Concentration of acetic acid is 0.100 M Concentration of NaOH is 0.167 M Calculate the...Explanation: Concentration of NaOH is 0.10 M Concentration of HCOOH is 0.10 M Find the concentration...Chapter 17, Problem 17.35QPChapter 17, Problem 17.36QPExplanation: SrF2 = 7.3 × 10-2g/L Calculate the molar solubility = 7.3 × 10-2g SrF2 1L× 1 mol SrF2...Chapter 17, Problem 17.65QPExplanation: The given data is recorded as such. 0.100 M HCl0.100 M CH3NH2 HCl(aq) + CH3NH2(aq) →...Explanation: CacH(aq) → Cac-(aq) + H+(aq) Initial concentration (M): 0.10 0 0 Change in...Chapter 17, Problem 17.126QPExplanation: The concentration of silver ion in AgBr is determined below. Solubility product...Chapter 18.3, Problem 2PPBThere are two half-cell reactions involved At anode, 2 Au(s) → 2 Au(aq)3+ + 6e−Eanode0 = 1.50 V At...The cell reaction involved is, H2(g) + 2AgCl(s) ⇄ 2Ag(s) + 2H+ + 2Cl(aq)− Partial pressure of H2 is...Chapter 18, Problem 18.1QPChapter 18, Problem 18.24QPChapter 18, Problem 18.32QPChapter 18, Problem 18.40QPExplanation: For Magnesium Mg2++2e-→Mg 1 mole Mg2mole e-×24.31g Mg1 mole Mg×1...Chapter 18, Problem 18.50QPChapter 18, Problem 18.51QPChapter 18, Problem 18.54QPChapter 18, Problem 18.65QPExplanation: To calculate the standard electrode potential of the cell (E°cell) The standard...Explanation: The total volume of the AgNO3 solution =100mL The concentration of AgNO3 =0.100M Weight...Explanation: To find the completely balanced chemical equation The overall cell reaction can be...Explanation: To explain the how cell potential (Ecell) of Daniel cell changes when the cell equation...Explanation: To record the given data Gf°(ZnO)=-318.2KJmol-1ΔGf°(Zn)=0ΔGf°(O2)=0 To write the half...Chapter 19.3, Problem 19.2WEGiven, Initial concentration of H2O2, [H2O2]0 = 0.75 MRate constant, k = 1.8 × 10−5 s−1Time, t = 3 h...Concentration of C2H5I after 10 min,[C2H5I]t is calculated below Given, Initial concentration of...In order to find the activation energy we need to find the slope value of line which obtained from...The rate law from the balanced equation of step 1 is as follows, rateforward=k1[NO][Br2]ratereverse...Chapter 19, Problem 19.1VCExplanation: To determine the order of the reaction From the given information, experiments 2 and 5...Explanation: To determine the concentration of NaOBr after 22s The given reaction is...Chapter 19, Problem 19.56QPChapter 19, Problem 19.85QPExplanation: From the given information, A and B both were decomposed by first-order kinetics....Explanation: The rate constant for the given first order nuclear decay is calculated from half-life...Explanation: First of all, calculate the number of radium nuclei in 1.0g 1.0g×1 mol Ra226.03 g...Explanation: The given reaction is Hb(aq)+O2(aq)→kHbO2(aq) The order of the reaction is second order...Explanation: We can easily determine the rate constant of a reaction if half-life value is given by...Chapter 19, Problem 19.131QPExplanation: We can write the balanced reaction from the given information as follows P → P*P* →P2_P...Reason for correct option To find: The original mass of sample of 61Cu The original mass of sample...Reason for correct option To find: The remaining mass of sample of 126I after 24 h The remaining...Reason for correct option To find: The age of the rock The age of the rock is 165 million years The...Determine the value of k Half-life of radioactive decay is the time required for a radioactive...Explanation: Nuclear reactions are differing from ordinary chemical reaction by the following way....Explanation: The binding energy is the energy required for the process He24→2p11+2n01 There are two...Explanation Nuclear reaction can be written in the shorthand notation with the parentheses....Explanation Nuclear reaction can be written in the shorthand notation with the parentheses....Explanation Nuclear reaction can be written in the shorthand notation with the parentheses....Explanation: Nuclear reaction can be written in the shorthand notation with the parentheses....Explanation Nuclear reaction can be written in the shorthand notation with the parentheses....Explanation: For the given 10B , there are5 protons and 5 neutrons. Mass of protons = 1.00728amuMass...Explanation Nuclear reaction can be written in the shorthand notation with the parentheses....Explanation Half-life of radioactive decay is the time required for a radioactive sample to decay to...Explanation Nuclear reaction can be written in the shorthand notation with the parentheses....Explanation: To explain about mineral: These are the substances naturally occurs and which are...Explanation: (a) Sodium metal reacts with water to produce sodium hydroxide and hydrogen gas. Na(s)...Explanation: To determine ΔH∘ values for decomposition of MgCO3(s)→MgO(s)+CO2(g) Substitute the...Explanation: To write the balanced equation for preparation of Al2Cl6 We can produce Al2Cl6 by...Explanation: The reaction between iron ion and permanagate and its balanced equation is represented...Explanation: Record the given data. Reactions: 2Fe2O3(s)→4Fe(s)+ 3O2(g) The temperature of the...Explanation: To write the balanced equation for heating of Al2(CO3)3 By heating of heating of...Chapter 21, Problem 21.74QPChapter 22.1, Problem 1PPAChapter 22, Problem 22.1QPExplanation: Interpret the complex ion [Cr(CN)6]4- . In complex ion [Cr(CN)6]4- , the oxidation...Chapter 22, Problem 22.33QPExplanation: Predict the complex which absorbs the longer wavelength. In the given complex ions, the...Chapter 22, Problem 22.71QPExplanation: Interpret the reason. Orbital Splitting diagram of linear complex: In the linear...Explanation: Find the concentration of lead ion [Pb(EDTA)2-] . [Pb]2++ EDTA4- ⇄...Interpret the given information. The complex ion[Mn(CN)6]5-. In complex ion[Mn(CN)6]5-, the...Interpret the given information. The Cu3+ion is unstable because of the high charge density on the...Explanation: To find: The name of the given organic compounds. The name of the given organic...Explanation: To find: Carbon forms more compound than the other element Catenation of the carbon...Explanation: To find: The name of the given organic compounds Name of the given organic compounds is...Chapter 23, Problem 23.10QPExplanation: To find: The structure of the given organic molecule. Name of the given organic...Explanation: To find: The structure of the given organic molecule. Name of the given organic...Explanation: To find: The structure of the given organic molecule. Name of the given organic...Explanation: To find: The structure of the given organic molecule. Name of the given organic...Explanation: To find:type of the reaction. The given reaction is isomerization reaction, the...Chapter 23, Problem 23.53QPExplanation: To find: The given compound is resonance structure, constitutional isomer, cis/trans...Chapter 24, Problem 24.1QP
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