OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:5th EditionSTANITSKI Publisher: Cengage LearningISBN: 9781285460369
OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
Solutions for OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
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Chapter 1 - The Nature Of ChemistryChapter 1.4 - Identifying Matter: Physical PropertiesChapter 1.5 - Measurements, Units, And CalculationsChapter 1.6 - Chemical Changes And Chemical PropertiesChapter 1.8 - Classifying Matter: Elements And CompoundsChapter 1.9 - Nanoscale Theories And ModelsChapter 1.11 - Communicating Chemistry: SymbolismChapter 1.13 - The Periodic TableChapter 1.14 - The Biological Periodic TableChapter 2 - Chemical Compounds
Chapter 2.1 - Atomic Structure: Subatomic ParticlesChapter 2.2 - The Nuclear AtomChapter 2.3 - Isotopes And Average Atomic MassChapter 2.4 - Ions And Ionic CompoundsChapter 2.5 - Naming Ions And Ionic CompoundsChapter 2.6 - Ionic Compounds: Bonding And PropertiesChapter 2.7 - Molecular CompoundsChapter 2.8 - Naming Binary Molecular CompoundsChapter 2.9 - Organic Molecular CompoundsChapter 2.11 - Molar MassChapter 2.12 - Composition And Chemical FormulasChapter 3 - Chemical ReactionsChapter 3.1 - Chemical EquationsChapter 3.2 - Balancing Chemical EquationsChapter 3.3 - Precipitation ReactionsChapter 3.4 - Acid-base ReactionsChapter 3.5 - Oxidatino-reduction And Electron TransferChapter 3.6 - The Mole And Chemical ReactionsChapter 3.7 - Limiting ReactantsChapter 3.8 - Evaluating Chemical Synthesis: Percent YieldChapter 3.9 - Composition And Empirical FormulasChapter 3.10 - Solution Concentration: MolarityChapter 3.11 - Stoichiometry In Aqueous SolutionsChapter 3.12 - Titrations In Aqueous SolutionsChapter 4 - Energy And Chemical ReactionsChapter 4.1 - The Nature Of EnergyChapter 4.2 - Conservation Of EnergyChapter 4.3 - Keeping Track Of Energy TransfersChapter 4.4 - Heat CapacityChapter 4.5 - Energy And EnthalpyChapter 4.6 - Reaction Enthalpies For Chemical ReactionsChapter 4.7 - Where Does The Energy Come From?Chapter 4.8 - Measuring Reaction Enthalpies: CalorimetryChapter 4.9 - Hess's LawChapter 4.10 - Standard Formation EnthalpiesChapter 4.11 - Fuels For Society And Our BodiesChapter 5 - Electron Configurations And The Periodic TableChapter 5.1 - Electromagnetic Radiation And MatterChapter 5.2 - Planck's Quantum TheoryChapter 5.3 - The Bohr Model Of The Hydrogen AtomChapter 5.4 - Beyond The Bohr Model: The Quantum Mechanical Model Of The AtomChapter 5.5 - Quantum Numbers, Energy Levels, And Atomic OrbitalsChapter 5.7 - Atom Electron ConfigurationChapter 5.8 - Ion Electron ConfigurationChapter 5.9 - Periodic Trends: Atomic RadiiChapter 5.10 - Periodic Trends: Ionic RadiiChapter 5.11 - Periodic Trends: Ionization EnergiesChapter 5.13 - Energy, Ions, And Ionic CompoundsChapter 6 - Covalent BondingChapter 6.2 - Single Covalent Bonds And Lewis StructuresChapter 6.3 - Single Covalent Bonds In HydrocarbonsChapter 6.4 - Multiple Covalent BondsChapter 6.5 - Multiple Covalent Bonds In HydrocarbonsChapter 6.6 - Bond Properties: Bond Length; Bond EnergyChapter 6.7 - Bond Properties: Polarity; ElectronegativityChapter 6.8 - Formal ChargeChapter 6.9 - Lewis Structues And ResonanceChapter 6.10 - Exceptions To The Octet RuleChapter 6.11 - Aromatic CompoundsChapter 6.12 - Molecular Orbital TheoryChapter 7 - Molecular StructuresChapter 7.2 - Predicting Molecular Shapes: VseprChapter 7.4 - Hybridization: Molecules With Multiple BondsChapter 7.5 - Molecular PolarityChapter 7.6 - Noncovalent Interactions And Forces Between MoleculesChapter 7.7 - Biomoleules: Dna And The Importance Of Molecular StructureChapter 8 - Properties Of GasesChapter 8.1 - Gas PressureChapter 8.2 - Kinetic-molecular TheoryChapter 8.3 - The Behavior Of Ideal Gases: Gas LawChapter 8.4 - Gas Density, Molar Mass, And The Ideal Gas LawChapter 8.5 - Quantities Of Gases In Chemical ReactionsChapter 8.6 - Gas Mixtures And Partial PressuresChapter 8.7 - Kinetic-molecular Theory And The Velocities Of Gas MoleculesChapter 8.8 - The Behavior Of Real (non-ideal) GasesChapter 8.11 - Greenhouse Gases And Global WarmingChapter 8.12 - Chemistry Of Air Quality And Air PollutionChapter 9 - Liquids, Solids, And MaterialsChapter 9.1 - Liquids, Solids, And Intermolecular ForcesChapter 9.2 - Vaporization And CondensationChapter 9.3 - Vapor PressureChapter 9.4 - Solids And Changes Of PhaseChapter 9.5 - Water: Its Important And Unusual PropertiesChapter 9.6 - Crystalline SolidsChapter 9.9 - Metals, Semiconductors, And InsulatorsChapter 9.11 - Cement, Ceramics, And GlassChapter 10 - Fuels, Organic Chemicals, And PolymersChapter 10.1 - PetroleumChapter 10.2 - U. S/ Energy Sources And ConsumptionChapter 10.4 - Alcohols And Their Oxidation ProductsChapter 10.5 - Carboxylic Acids And EstersChapter 10.6 - Synthetic Organic PolymersChapter 10.7 - Biopolymers: Polysaccharides And ProteinsChapter 11 - Chemical Kinetics: Rates Of ReactionsChapter 11.1 - Reaction RateChapter 11.2 - Effect Of Concentration On Reaction RateChapter 11.3 - Rate Law And Order Of ReactionsChapter 11.4 - A Nanoscale View: Elementary ReactionsChapter 11.5 - Temperature And Reaction Rate: The Arrhenius EquationChapter 11.6 - Rate Laws For Elementary ReactionsChapter 11.7 - Reaction MechanismsChapter 11.8 - Catalysts And Reaction RateChapter 11.9 - Enzymes: Biological CatalystsChapter 12 - Chemical EquilibriumChapter 12.1 - Characteristics Of Chemical EquilibriumChapter 12.2 - The Equilibrium ConstantChapter 12.3 - Determining Equilibrium ConstantsChapter 12.4 - The Meaning Of The Equilibrium ConstantsChapter 12.5 - Using Equilibrium ConstantsChapter 12.6 - Shifting A Chemical Equilibrium: Le Chatelier's PrincipleChapter 12.7 - Equilibrium At The NanoscaleChapter 12.8 - Controlling Chemical Reactions: The Haber-bosch ProcessChapter 13 - The Chemistry Of Solutes And SolutionsChapter 13.1 - Solubility And Intermolecular ForcesChapter 13.2 - Solubility And EquilibriumChapter 13.4 - Temperature And SolubilityChapter 13.5 - Pressure And Dissolving Gases In Liquids: Henry's LawChapter 13.6 - Expressing Solution CompositionChapter 13.7 - Colligative Properties Of SolutionsChapter 13.9 - SurfactantsChapter 13.10 - Water: Natural, Clean, And OtherwiseChapter 14 - Acids And BasesChapter 14.1 - Bronsted-lowry Acids And BasesChapter 14.2 - Carboxylic Acids And AminesChapter 14.3 - The Autoionization Of WaterChapter 14.4 - The Ph ScaleChapter 14.5 - Ionization Constants Of Acids And BasesChapter 14.6 - Molecular Structure And Acid StrengthChapter 14.7 - Problem Solving Using Ka And KbChapter 14.8 - Acid-base Reactions Of SaltsChapter 14.9 - Lewis Acids And BasesChapter 14.10 - Additional Applied Acid-base ChemistryChapter 15 - Additional Aqueous EquilibriaChapter 15.1 - Buffer SolutionsChapter 15.2 - Acid-base TitrationsChapter 15.4 - Solubility Equilibria And The Solubility Product Constant, KspChapter 15.5 - Factors Affecting SolubilityChapter 15.6 - Precipitation: Will It Occur?Chapter 16 - Thermodynamics: Directionality Of Chemical ReactionsChapter 16.1 - Reactant-favored And Product-favored ProcessesChapter 16.2 - Chemical Reactions And Dispersal Of EnergyChapter 16.3 - Measuring Dispersal Of Energy: EntropyChapter 16.4 - Calculating Entropy ChangesChapter 16.5 - Entropy And The Second Law Of ThermodynamicsChapter 16.6 - Gibbs Free EnergyChapter 16.7 - Gibbs Free Energy Changes And Equilibrium ConstantsChapter 16.8 - Gibbs Free Energy, Maximum Work, And Energy ResourcesChapter 16.9 - Gibbs Free Energy And Biological SystemsChapter 16.11 - Thermodynamic And Kinetic StabilityChapter 17 - Electrochemistry And Its ApplicationsChapter 17.1 - Redox ReactionsChapter 17.2 - Half-reactions And Redox ReactionsChapter 17.3 - Voltaic CellsChapter 17.4 - Voltaic Cells And Cell PotentialChapter 17.5 - Using Standard Half-cell PotentialsChapter 17.6 - E⁰cell, Gibbs Free Energy, And K⁰Chapter 17.7 - Effect Of Concentration On Cell Potential: The Nernst EquationChapter 17.8 - Common BatteriesChapter 17.10 - Electrolysis-causing Reactant-favored Redox Reactions To OccurChapter 17.11 - Counting ElectronsChapter 17.12 - Corrosion: Undesirable Product-favored Redox ReactionsChapter 18 - Nuclear ChemistryChapter 18.2 - Nuclear ReactionsChapter 18.3 - Stability Of Atomic NucleiChapter 18.4 - Rates Of Disintegration ReactionsChapter 18.5 - Artificial TransmutationsChapter 18.6 - Nuclear FissionChapter 18.7 - Nuclear FusionChapter 18.8 - Nuclear Radiation: Effects And UnitsChapter 18.9 - Applications Of RadioactivityChapter 19 - The Chemistry Of The Main-group ElementsChapter 19.1 - Formation Of The ElementsChapter 19.2 - Terrestrial ElementsChapter 19.3 - Extraction By Physical Methods: Nitrogen, Oxygen, And SulfurChapter 19.4 - Extraction By Electrolysis: Sodium, Chlorine, Magnesium, And AluminiumChapter 19.5 - Extraction By Chemical Oxidation-reduction: Phosphorus, Bromine, And IodineChapter 19.6 - A Periodic Perspective: The Main-group ElementsChapter 20 - Chemistry Of Selected Transition Elements And Coordination CompoundsChapter 20.1 - Properties Of The Transition (d-block) ElementsChapter 20.2 - Iron And Steel: PyrometallurgyChapter 20.3 - Copper: A Coinage MetalChapter 20.4 - Silver And Gold: The Other Coinage MetalsChapter 20.5 - ChromiumChapter 20.6 - Coordinate Covalent Bonds: Complex Ions And Coordination CompoundsChapter 20.7 - Crystal-field Theory: Color And Magnetism In Coordination Compounds
Sample Solutions for this Textbook
We offer sample solutions for OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY: homework problems. See examples below:
Nanoscale indicates something that is one billion times smaller than something else. Nanoscale...Chapter 1, Problem 21QRTThe given calculation is 2221.05- 3256.53.20 The calculation is division. The numerator consists of...The given three different proportions of chromium in 100 g of oxide are 52.0 %, 68.4% and 76.5%. The...Given, The diameter of Earth as 8,000 mi. The surface of the earth is calculated by 4πr2. = 4 ×...The mass of each atom to the mass of sample is given as 1.0000 g AgCl = mAg + mCl1.6381 g AgI = mAg...The mass of each atom to the mass of sample is given as 35.48 g rust = mFe + mO22.65 g aluminum...Given, Debt is $28.8 × 106. The value of gold is $21.25/troy oz (1 troy oz = 31.103 g). The gold...Aspirin: The molecular formula of aspirin is C9H8O4. Mass of the given compound is 12.0 g. Molar...
Chapter 2, Problem ISP(i)Ammonium dichromate contains the ammonium cation, NH4+ and the dichromate anion Cr2O72-. The...Given the number of moles of methanol is 1. Number of moles of carbon = 1 mole. Number of moles of...Given the number of moles of glucose is 1. Number of moles of carbon = 6 moles. Number of moles of...The given substance is methanol CH3OH. Mass of carbon = 12.0107 g/mol. Mass of hydrogen = 1.0079...The molecular formula of aspirin is C9H8O4. The molecular formula of sodium carbonate is NaHCO3. The...The given compound is PbS, lead (II) sulfide (galena). Mass of lead is 207.2 g/mol. Mass of sulfur...The molecular formula of caffeine is C8H10N4O2. Mass of nitrogen per mole of C8H10N4O2: 2 × 14.0067...Sample containing 1 mol Cl2 has more atoms than a sample containing 1 mol Cl, since the molecule of...Chapter 2, Problem 131QRTThe given BrCl is a binary compound. Then the name of the compound is bromine monochloride.Given the amount of Fe2O3 is 10.3 g. Molar mass of Fe2O3 is: (2×55.854 g/mol Fe) + (2×15.9994 g/mol...Given, The molar mass of one compound is 110.2 g/mol. Molar mass of potassium is 39.0983 g and...The three compounds have different formulas. The first of these has a larger number of Ey atoms in...Using the relationship between Ex and Ez in the given formula, then it is possible to determine the...The given reactant is shown below, BaCl2(aq) and Na2C2O4(aq) The product of the reaction is shown...Chapter 3, Problem ISPChapter 3, Problem IISPThe given compound is shown below, Potassium monohydrogen phosphate (K2HPO4) All 1A (Li+, Na+, K+,...Chapter 3, Problem 30QRTThe given compound is shown below, NaNO2 NaNO2 dissociates in water (dissociation). Therefore NaNO2...The given compound is shown below, NaCH3COO NaCH3COO is formed from the neutralization of CH3COOH...Given, Fe(OH)3(s) + 3HNO3 The product of the reaction is shown below, Fe(OH)3(s) + HNO3(aq)→...The given statement is shown below, CCl2F2 reacts with sodium oxalate gives carbon, carbon dioxide,...Chapter 3, Problem 92QRTThe reaction is shown below, C6H8O6(aq) + Br2(aq) → 2 HBr(aq) + C6H6O6(aq) 1.00 g Chewable vitamin C...The given equation is shown below, NaOH(aq) + H3PO4(aq) → NaH2PO4(aq) + H2O(l) Oxidation number of...Generally organic molecule undergoes combustion reaction which produces carbon dioxide and water...The balanced equation for the reaction is given below, 3 C2H5OH(aq) + 2 K2Cr2O7(aq) + 8 H2SO4(aq)...Given, 0.1235-g of H2X (diacid) is neutralized with 15.55 mL of 0.1087-M NaOH. Then, 0.3469-g sample...Given, Three Group 2A elements magnesium, calcium, and strontium are allowed to react with liquid...Given, TrialABCDE0.10 M Xn+7 mL6 mL5 mL4 mL3 mL0.20 M Ym-3 mL4 mL5 mL6 mL7 mLExcess Xn+...Given, 100.0 g cobalt and 200.0 g carbon monoxide gives 89.7 % yield of dicobalt octacarbonyl...First law of thermodynamics – Law of conservation of energy and Hess’s Law are the two laws stated...Chapter 4, Problem 61QRTThe reactions of molecular hydrogen with bromine and iodine are as follows, H2+Br2→ 2HBrH2+I2→ 2HI...Mixing of two given solutions with change in temperature, the heat transferred is determined as...Given: Al2O3(s) The balanced expression for formation of one mole Al2O3(s) with ΔfH∘ value taken...CaO(s) and CO2(g) are products. CaCO3(s) is reactant. The standard reaction enthalpy is determined...Combustion reaction of sulfur is S(s)+O2(g)→SO2(g). The ΔfH∘ value of above reaction is - 1206.92...The equations for combustion of one mole of CH3OH and C8H18 are as follows,...The given equations for combustion are as follows,...Given: NH4NO3(s)→N2O(g)+2H2O(g) Using the above given reaction enthalpy is calculated by subtracting...Given Step 1: SO2(s)+2H2O(g)+Br2(g)→H2SO4(l)+2HBr(g) Using the above given reaction enthalpy is...The dimensions of tank car are 20 feet (6.1m) long, 8 feet (2.4 m) high and 8 feet (2.4 m) wide. Now...First, the octane in milliliters is determined. Volume ⇒1 gal×4 quart1 gal×1.00×10-3 m31.056710...The Table 4.3 is as follows, The food items in above table are ranked from low caloric value to high...Frequency: It is the number of complete waves passing through a point in a given period of time. The...Given, compounds containing barium emits at the wave length 493 nm. The color of the wave length 493...The electronic configuration of boron atom is given by 1s2 2s2 2p1 The arrangement of electrons in...Chapter 5, Problem 44QRTChapter 5, Problem 79QRTA modern periodic table is given by Figure 1 Sulphur belongs to p-block element of periodic table....Electron affinity is the energy required to add an electron to the neutral atom. A + e- → A- The...Chapter 5, Problem 130QRTThese O2- , F− , Na+,and Mg2+ electrons are all isoelectronic, with a grouped electron...Enthalpy of formation of Calcium chloride is calculated as, Ca(g)+ +Cl(g)- →CaCl(s) ΔH rex =lattice...Enthalpy of formation of Silver chloride is calculated as, Ag(g)+ +Cl(g)- →AgCl(s) ΔH rex =lattice...An ionic bond and a covalent bond differ in the location of the electrons. Ionic bondCovalent Bond...Oxygen is in Group 6A and Chlorine is in Group 7A and the valence electrons present in the Cl2O...The correct Lewis structure of the Acetaldehyde can be drawn as, Draw a chart: C− C= H OValence...The correct Lewis structure of the KrF4 can be drawn as, Draw a chart: Kr F Valence electrons 8...Chapter 6, Problem 43QRTThe correct Lewis structure of Peroxydisulfate ion (S2O82−) can be drawn as, Achart can be drawn as,...The correct Lewis structure of the Nitrosyl Fluoride can be drawn as, Draw a chart: O N Cl I II I II...Chapter 6, Problem 46QRTThe correct Lewis structure of the POF3 can be drawn as, Draw a chart: O N Cl P O F Valence...The total number of valence electrons present in Peroxide ion is 14 electrons. The molecular orbital...The total number of valence electrons present in CO molecule is 10 electrons. The molecular orbital...Given, C(g)=ΔfHo=716.7kJ/molH(g)=ΔfHo=218 kJ/mol The average C-H bond energy in methane can be...Chapter 7, Problem ISPGiven molecule is BeH2 . The Lewis electron dot structure for given molecule can be determined by...Given molecule is NH2Cl . The Lewis electron dot structure for given molecule can be determined by...Given molecule is BO33− . The Lewis electron dot structure for given molecule can be determined by...Given molecule is CO2. The Lewis electron dot structure for given molecule can be determined by...Given molecule is SO2. The Lewis electron dot structure for SO2 is given below: The electron-region...Given molecule is SO2. The Lewis electron dot structure for SCl2 is given below: . The...Given molecule is CH3CH2CCH. The Lewis electron dot structure for alanine is given below: . Consider...Given molecule is OCS. The Lewis electron dot structure for OCS is given below: . Sigma bond and pi...Chapter 7, Problem 100QRTChapter 7, Problem 104QRTChapter 8, Problem ISPGiven that pressure is 720 mmHg. Convert the unit of pressure from mmHg to atm as follows, P= 720...Given that pressure is 120 mmHg. Convert the unit of pressure from mmHg to atm as follows, P= 120...Given data is shown below, V = 1.05×103 LP = 745 mmHg = 745 mmHg×1 atm760 mmHg= 0.980 atmT = 20°C =...Given data is shown below, M of C = 12.0107 g/molM of H = 1.0079 g/molmCxHy = 0.293 g P = 374 mmHg×1...Given information is shown below, Ptotal = 740 mm HgpN2 = 575 mm HgpAr = 6.9 mm HgpCO2 = 0.2 mm...Given data is shown below, PO2 = 1.46 atmPN2 = 0.908 atmPAr = 2.71 atmVO2 = 3.0 LVN2 = 2.0 LVAr =...Calculate the volume of He: mass = n×Molar mass= (1 mol)(4.003 g/mol) = 4.003 gdensity = massVolume=...Reaction is shown below, H2(g)+ Cl2(g) → 2 HCl(g) Number of moles of H2 and Cl2 can be determined...Given data is shown below, T = 25°C = (25+273)K= 298KT = 35°C = (35+273)K= 308K Molar mass of Cl2 is...Given information is shown below, P= 750 mmHg= 750 mmHg×1 atm760 mmHg = 0.987 atmT = 50°C =...Number of moles of PCl5 before vaporization is calculated as given below, n = MassMolar mass= 2.69...Diameter of the atom is determined as follows, 1 pm = 10−10 cmσ=2r = 2×91 pm = 182 pm×10−10 cm1 pm=...Figure 1 Vapour pressure of a liquid is defined as the pressure of the vapour when liquid and vapour...Given data: The heat capacities of solid ice and liquid water are 2.06 Jg−1 ∘C−1 and 4.184 Jg−1 ∘C−1...Given data: The heat capacities of solid ice and liquid water are 2.06 Jg−1 ∘C−1 and 4.184 Jg−1 ∘C−1...Given data: The specific heat capacity of liquid water is 4.184 Jg−1 ∘C−1. The fusion of enthalpy...The maximum wavelength of the radiation that would be diffracted by a crystal is equal to its unit...Given that, typical cement contains 65% CaO, 20% SiO2,5% Al2O3 ,6% Fe2O3, and 4% MgO. It implies...Given data: The specific heat capacities of gas and liquid are .61 Jg−1 ∘C−1 and 0.97 Jg−1 ∘C−1...Given data: The specific heat capacities of gas and liquid are 2.2 Jg−1 ∘C−1 and 4.7 Jg−1 ∘C−1....The atoms can be assumed to be spherical in shape with radius r. So the volume of one atom can be...The phase diagram of sulfur is given below. Figure 2 From the above phase diagram, it is clear that...Sample 1 has been prepared by grinding one mole of KCl and one mole of RbCl together . Sample 2 has...The heat capacity of liquid water and water vapor are 4.18 Jg−1∘C−1 and 1.84 Jg−1∘C−1 respectively....The give compound, CH3(CH2)8CH2OH is an alcohol with ten carbon atoms. According to the basic...Gasoline (C8H18) reacts with oxygen gas to give the products water and carbon dioxide gas. The...Chapter 10, Problem 97QRTThe amount of fuel that is CH3OH required to travel 20 mile by car is 1 gallon. So, the amount of...The polymer Teflon is formed by the addition reaction of tetrafluoroethylene. Consider the given...The mass of carbon dioxide produced is 5.287 g. The mass of water produced is 2.164 g. The molar...The mass of carbon dioxide produced is 7.720 g. The mass of water produced is 3.612 g. The molar...The given blank is: A triglyceride _______ The triglyceride is formed by the reaction of glycerol...The given blank is: Can be oxidized to an aldehyde _______ Oxidation of alcohol is the process in...The number of moles of hydrocarbon is calculated by the formula shown below. Number of moles...The hydrogenation reaction of 4-octyne gives an alkene, 4-octene, in the first step. The alkyne has...The halogenation reaction of 3-Hexene gives an alkyl halide, 3-chlorohexene. The alkene has a π bond...The given data table is shown below. HydrocarbonFormulaEnthalpy if combustion (kJ/mol)ButaneC4H10...Chapter 11, Problem ISPGiven that the concentration of N2O5 at t= 0.00 h is 0.849 mol/L and the concentration of N2O5 at t=...Average concentrations can be calculated as given below. From 0 to 0.50 h: Average...The rate law can be represented as given below. Rate=k[I]i[II]j Where, k, i and j are unknown. The...Chapter 11, Problem 26QRTThe activation energy can be calculated using following formula, lnk2k1=EaR(1T1−1T2) Given,...The reaction: 2NO(g)+Cl2(g)→2NOCl(g) The accepted mechanism: NO+Cl2⇌k−1k1NOCl2 fastNOCl2+NO→k22NOCl...2NO(g)+O2(g)→2NO2(g) Suppose the rate law of the above reaction is as follows, Rate=k[NO]i[O2]j...Chapter 11, Problem 95QRTThe rate constant of the reaction is 0.68 s−1. So the given reaction is first order because the unit...(a) The accepted mechanism: 12Cl2⇌Cl fastCl+Cl2⇌Cl3 fastCl3+CO→COCl2+Cl slowCl⇌12Cl2 fast The rate...The rate is affected by the concentration of Benzenesulfonyl chloride (BSC), but it is kept constant...Chemical equilibrium is a state of a chemical reaction at which both the reactants and products are...Given reaction, N2(g) + O2(g) ⇌ 2 NO(g) KC = 1.7 × 10-3 at 2300 K[N2] = [O2] = 0.25 M and [NO] =...Given information, N2(g) + O2(g) ⇌ 2 NO(g) KC = 1.7 × 10-3 at 2300 KN2 = 0.25 mol ; O2 = 0.25 mol...Given information, H2(g) + I2(g) ⇌ 2 HI(g) KC = 50.0 at 745 KH2 = 0.025 mol ; I2 = 0.025 mol and HI...Given information, C (graphite) + CO2(g) ⇌ 2 CO(g) KC = 3.7 × 10-23 at 25oCCO = 3.5 mol and CO2 =...The equilibrium constant expressions in terms of the unknown variable x for 1 reaction is, H2O(l) ⇌...The equilibrium constant expressions in terms of the unknown variable x for 1 reaction is, 2O3(g) ⇌...Using ICE table to calculate x value. The concentration of E2 is = 1.00 mol1.0 L =1.0 M E2(g) ⇌...Balanced reaction is, Ni(s) + 4CO(g) ⇌ Ni(CO)4(g) Mole of CO in 2.05 g CO is, = 2.05 g CO ×1 mol...Given information, Volume of flask is 10.00 L. Equilibrium constant value for the reaction, 2 HI(g)...Given information, Volume of flask is 10.00 L. Equilibrium constant value for the reaction, CO(g) +...Given information, Formation of carbonylbromide from Carbon monoxide and Bromine, CO(g) + Br2(g) ⇌...Given information, Temperature is 20.0 oC or 293.2 K, volume of flask is 5.00 L, amount of SCl2 and...Given reaction, Step 1: NO(g) + Br2(g) ⇌ NOBr2(g)Step 2 : NOBr2(g) + NO(g) → 2 NOBr(g) Write the...The Mass fraction: Mass fraction of A = Mass of A Mass of A + Mass of B + Mass of C+ .... Given data...From the two given molecule namely motor oil and gasoline; motor oil is non-polar. Gasoline is also...Given mass is 14.2 g; Volume is 250 mL; Molar mass KCl is 74.55 g/mol. Calculate the number of...Given mass is 6.18 g; Volume is 250 mL; Molar mass MgNH4PO4 is 137.31 g/mol. Calculate the number of...Chapter 13, Problem 56QRTThe Mass fraction: Mass fraction of A = Mass of A Mass of A + Mass of B + Mass of C+ .... Given...The Mass fraction: Mass fraction of A = Mass of A Mass of A + Mass of B + Mass of C+ .... Given...Chapter 13, Problem 67QRTChange in boiling point is calculated as shown below, Given information as follows, Tb(solution)=...Using Freezing point of the solution: ΔTf =Tf °(solution)-Tf (solvent)= -15.0∘C +(-0.0∘C)= -15.0∘C ....Given data as follows: Mole of NaCl= 0.100 mole; molality of NaCl solution = 0.100 mol/kg; ‘i’ is =...Lye(NaOH): The weight percent: weight % A = (Mass fraction)×100%. Given value of the mass fraction...Table salt: The Mass fraction: Mass fraction of A = Mass of A Mass of A + Mass of B + Mass of C+...Given information as: The compound contains 73.94% of Carbon and 8.27% of Hydrogen and the remaining...Given information is given as, 0.63% of SnF2 is present. As known, 1% = 10,000 ppm. So, 0.63% of...Chapter 14, Problem ISPGiven formula is HI. This is a Brønsted-Lowry acid, as this has one more H+ ion. When this is added...Given formula is CN−. This is a Brønsted-Lowry base, as this does not have H+ ions. When this is...Given reaction is, HS−(aq)+H2O(l)→H2S(aq)+OH−(aq) In the above equation, water present in the...Solution D: Concentration of H3O+ is given as 2×10−3 M. Using the equation for ionization constant...Solution W: Concentration of H3O+ is given as 5×10−6 M. Using the equation for ionization constant...(a) pH=1.00 The relationship between pH and pOH is given below. pH+pOH=14 Therefore,...(a) [H3O+]=6.1×10-7M The pH of the solution can be calculated as given below....HNO2 is a weak acid as its Ka value is 7.1×10−4. Its pH will be between 2 and 6.The equilibrium reaction is given below. HNO2(aq)+H2O(l)⇌NO2−(aq)+H3O+(aq) The acid ionization...The equation for the equilibrium can be written as given below....The solution contains NH4+ and [B(OH)4]− ions. Ka for NH4+ is 5.6×10−10 and Kb for [B(OH)4]− is...Given that, the pH values of sodium salts NaM, NaQ and NaZ are 7.0, 8.0 and 9.0 respectively. The...The buffer solution always consists of conjugate acid and conjugate base. As per the given data the...As per the given data the number of moles of silver ion is 0.0010 mol in 0.500 L of solution. The...The value of pH of the buffer solution before NaOH is added to the buffer solution is calculated...The value of pH of the buffer solution before NaOH is added to the buffer solution is calculated...The standard value of Ka for CH3CH2COOH is 1.4×10−5. The pKa for CH3CH2COOH is calculated by using...Let the strong acid be hydrochloric acid and weak base be ammonia. The concentration and volume of...The given molarity of benzoic acid is 0.100 M. The given molarity of titrant, NaOH is 0.100 M. The...Given, The titration of 50 mL of 0.150 M HCl solution with 0.150 M NaOH solution. Volume of the...Given, Volume of acid in liters: =50 mL ×1 L 1000 mL=0.05000L Original mole H3O+added: =0.05000L...The dissociation reaction of ZnCO3 is shown below. ZnCO3(s)⇌Zn2+(aq)+CO32−(aq) The Ksp for ZnCO3 is...Given, The concentration of Mg2+ is 0.050 M. Salts gets dissociation in to their ions, Mg(OH)2salt...As per the given data, the volume of the solution is 100 mL. The unit conversion of volume from mL...The standard values of Ksp for BaSO4 is 1.1×10−10. The dissociation reaction for BaSO4 is shown as...Chapter 16, Problem 1QRTThe reaction is shown below. C2H4(g)+H2(g)→C2H6(g) The value of ΔrS° is calculated by the formula...The given reaction is shown below. Fe2O3(s)+2Al(g)→2Fe(s)+Al2O3(s) The standard enthalpy change for...The given reaction is shown below. C6H12O6(s)+6O2(g)→6CO2(g)+6H2O(l) The standard enthalpy change...The given reaction is shown below. CO(g)+2H2(g)→CH3OH(l) The formula to calculate ΔrG° is shown...The given reaction is shown below. CO(g)+2H2(g)⇄CH3OH(l) The formula to calculate ΔrG° is shown...The given reaction is shown below. 2H2(g)+O2(g)⇄2H2O(g) The formula to calculate ΔrG° is shown...The given reaction is shown below. H2(g)+I2(g)⇌2HI(g) The formula to calculate ΔrG° is shown below....The given reaction is shown below. 2C6H6(l)+15O2(g)→12CO2(g)+6H2O(g) The value of ΔrG° is calculated...The given reaction is shown below. Al2O3(s)→2Al(s)+32O2(g) The value of ΔrG° is calculated by the...The unbalance equation of decomposition of copper (II) oxide is shown below. CuO(s)→Cu(s)+O2(g) A...The value of standard Gibbs free energy of the formation H2(g) is 0 kJ mol−1. The value of standard...Reaction of carbon with steam results in the formation of various gases along with carbon dioxide as...The half-cell reactions which take place at cathode and anode in nickel-zinc battery are shown...The given reaction is shown below. Fe(s)+Br(l)→FeBr2(s) The oxidation number of any element in its...The reaction for the conversion of MnO4− to Mn2+ ion is shown below. MnO4−(aq)→Mn2+(aq) The number...The given reaction is shown below. Fe(s)+Br2(l)→FeBr2(s) The oxidation number of any element in its...The given reaction is shown below. Fe(s)+Br2(l)→FeBr2(s) The oxidation number of any element in its...The given unbalanced redox reaction is shown below. CO(g)+ O3(g)→ CO2(g) The carbon atoms in the...The given unbalanced redox reaction is shown below. FeO(s)+ O3(g)→ Fe2O3(s) The iron atom and oxygen...The given compound is CH3SO2F. In CH3SO2F, the sulfur is the center atom. The sulfur atom is...The given first unbalanced redox reaction is shown below. NO3−(aq)+ H+(aq)+Hg(l)→...The E° value of Cr2+|Cr is −0.89 V. The E° value of Zn2+|Zn is −0.763 V. The E° value of Zn2+ is...The main products produced by the complete combustion of octane are carbon dioxide and water. The...When uranium-238 undergoes reaction with a neutron, the mass number increases by 1 and there is no...Alpha emission results in the formation of nucleus that has mass number less by 4 and atomic number...Given nuclear equation is, ? → N1022e + e+10 In a nuclear equation the sum of subscript on both...Given equations in the problem statement is, 5H11 + 5n01 → B5105H11 + 6n01 → B511 For B510: The...Given equations in the problem statement is, 15H11 + 15n01 → P153015H11 + 16n01 → P1531 For P1530:...Given nuclear equation in the problem statement is, U92235 + n01 → ? + S3893r + 3n01 In a balanced...Given nuclear equation is, 214Bi → + 214Po Atomic number of bismuth is 83 and atomic number of...Given nuclear equation is, + neutron → 2 neutrons + 137Tc + 97Zr Neutron can be represented as n01....Given nuclear equation is, U92238 + N714 → + 5n01 The unknown particle can be assigned as XZA....Given reaction is that element 117 is synthesized by collision of berkelium-249 and calcium-48...Mass of carbon present in 1.14 g of CaCO3 can be calculated using the conversion factors as shown...Nuclear fusion of hydrogen (protons) to form helium nucleus is known as hydrogen burning. Inside the...Magnesium chloride undergoes electrolysis to form magnesium metal and chlorine gas. This can be...In Downs process, the reaction that takes place is given as, 2Na+(aq) + 2e- → 2Na(s) 2Cl-(aq) →...Entry 1: Name is given as nitrogen. The formula of nitrogen is N2. Oxidation state of nitrogen in...Entry 1: Name is given as phosphorus. The formula of phosphorus is P. Oxidation state of phosphorus...In Downs process, the reaction that takes place is given as, 2Na+(aq) + 2e- → 2Na(s) 2Cl-(aq) →...Oxidation state of nitrogen in N2H4: Hydrogen has an oxidation state of +1. Sum of oxidation state...Given reaction in the problem statement is, Cl2(g) + H2O(l) ⇌ H+(aq) + Cl-(aq) + HOCl(aq) Oxidation...Given equation is, MnO2(s) + Br-(aq) → Mn2+(aq) + Br2(l) The oxidation state of manganese has...Clausius-Clapeyron equation can be given as, ln P = −ΔvapHRT + C −−−−−−−−−−−−−−−−−−−(1) Where,...Phosphorus belongs to Group VA in periodic table. It is a non-metal. Non-metals burns with oxygen to...Most abundant transition metal is Iron. It is also the second most abundant element that is metal....Chapter 20, Problem 16QRTGiven reaction is shown below. Fe(s)+NO3−(aq)→Fe3+(aq)+NO2(g) Balancing first half reaction: The...Given reaction is shown below. Cu(s)+NO3−(aq)→Cu2+(aq)+NO2(g) Balancing first half reaction: The...Given compound is V2O5. The transition metal that is present in the given compound is vanadium. In...Given reaction is, 2Al(s) + Cr2O3(s) → 2Cr(s) + Al2O3(s) ΔrG° can be calculated as shown below, ΔrG°...Ligands present in complex Na3[IrCl6]: In this complex, the counter ion is three Na+ ions. Complex...Given complex ion is [Cr(H2O)6]2+. The central metal ion is Cr2+. Cr2+ ion is said to contain four...Octahedral complex contains six ligands inside the coordination sphere. Central metal atom is given...Given complex has formula of [Pt(en)Cl2]. The complex [Pt(en)Cl2] do not dissociate into ions in...Given complex has formula of [Pt(en)Cl2]. The complex [Pt(en)Cl2] do not dissociate into ions in...
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