CHEMISTRY: MOLECULAR...(LL) W/ALEKS9th EditionSILBERBERG Publisher: MCG CUSTOMISBN: 9781265141875
CHEMISTRY: MOLECULAR...(LL) W/ALEKS
Solutions for CHEMISTRY: MOLECULAR...(LL) W/ALEKS
Problem 3.3P:
Why might the expression “1 mol of chlorine” be confusing? What change would remove any uncertainty?...Problem 3.12P:
Calculate each of the following quantities:
Mass (g) of 0.346 mol of Zn
Number of F atoms in 2.62...Problem 3.13P:
Calculate each of the following quantities:
Amount (mol) of Mn atoms in 62.0 mg of Mn
Amount (mol)...Problem 3.20P:
Calculate each of the following:
Mass % of H in ammonium bicarbonate
Mass % of O in sodium...Problem 3.21P:
Calculate each of the following:
Mass % of I in strontium periodate
Mass % of Mn in potassium...Problem 3.22P:
Calculate each of the following:
Mass fraction of C in cesium acetate
Mass fraction of O in uranyl...Problem 3.23P:
Calculate each of the following:
Mass fraction of Cl in calcium chlorate
Mass fraction of N in...Problem 3.24P:
Oxygen is required for the metabolic combustion of foods. Calculate the number of atoms in 38.0 g of...Problem 3.25P:
Cisplatin (right), or Platinol, is used in the treatment of certain cancers. ( Calculate (a) the...Problem 3.26P:
Allyl sulfide (below) gives garlic its characteristic odor. Calculate (a) the mass (g) of 2.63 mol...Problem 3.27P:
Iron reacts slowly with oxygen and water to form a compound commonly called rust (Fe2O3·4H2O). For...Problem 3.30P:
The mineral galena is composed of lead(II) sulfide and has an average density of 7.46 g/cm3. (a) How...Problem 3.33P:
List three ways compositional data may be given in a problem that involves finding an empirical...Problem 3.40P:
What is the molecular formula of each compound?
Empirical formula CH2 (ℳ = 42.08 g/mol)
Empirical...Problem 3.43P:
Find the empirical formula of each of the following compounds: (a) 0.039 mol of iron atoms combined...Problem 3.44P:
An oxide of nitrogen contains 30.45 mass % N. (a) What is the empirical formula of the oxide? (b) If...Problem 3.46P:
A sample of 0.600 mol of a metal M reacts completely with excess fluorine to form 46.8 g of MF2.
How...Problem 3.75P:
Elemental phosphorus occurs as tetratomic molecules, P4. What mass (g) of chlorine gas is needed to...Problem 3.77P:
Solid iodine trichloride is prepared in two steps: first, a reaction between solid iodine and...Problem 3.95P:
When 20.5 g of methane and 45.0 g of chlorine gas undergo a reaction that has a 75.0% yield, what...Problem 3.101P:
Sodium borohydride (NaBH4) is used industrially in many organic syntheses. One way to prepare it is...Problem 3.103P:
The first sulfur-nitrogen compound was prepared in 1835 and has been used to synthesize many others....Problem 3.107P:
Serotonin () transmits nerve impulses between neurons. It contains 68.2% C, 6.86% H, 15.9% N, and...Problem 3.108P:
In 1961, scientists agreed that the atomic mass unit (amu) would be defined as the mass of an atom...Problem 3.110P:
Isobutylene is a hydrocarbon used in the manufacture of synthetic rubber. When 0.847 g of...Problem 3.111P:
The multistep smelting of ferric oxide to form elemental iron occurs at high temperatures in a blast...Problem 3.121P:
For the reaction between solid tetraphosphorus trisulfide and oxygen gas to form solid...Problem 3.129P:
Ferrocene, synthesized in 1951, was the first organic iron compound with Fe─C bonds. An...Problem 3.132P:
Citric acid (below) is concentrated in citrus fruits and plays a central metabolic role in nearly...Problem 3.134P:
Nitrogen monoxide reacts with elemental oxygen to form nitrogen dioxide. The first scene below...Problem 3.137P:
Manganese is a key component of extremely hard steel. The element occurs naturally in many oxides. A...Problem 3.138P:
The human body excretes nitrogen in the form of urea, NH2CONH2. The key step in its biochemical...Problem 3.139P:
Aspirin (acetylsalicylic acid, C9H8O4) is made by reacting salicylic acid (C7H6O3) with acetic...Problem 3.143P:
When powdered zinc is heated with sulfur, a violent reaction occurs, and zinc sulfide forms:
Some...Browse All Chapters of This Textbook
Chapter 1 - Keys To Studying Chemistry: Definitions, Units, And Problem SolvingChapter 1.1 - Some Fundamental DefinitionsChapter 1.3 - Measurement And Chemical Problem SolvingChapter 1.4 - Uncertainty In Measurement: Significant FiguresChapter 2 - The Components Of MatterChapter 2.1 - Elements, Compounds, And Mixtures: An Atomic OverviewChapter 2.2 - The Observations That Led To An Atomic View Of MatterChapter 2.3 - Dalton’s Atomic TheoryChapter 2.5 - The Atomic Theory TodayChapter 2.6 - Elements: A First Look At The Periodic Table
Chapter 2.7 - Compounds: Introduction To BondingChapter 2.8 - compounds: Formulas, Names, And MassesChapter 3 - Stoichiometry Of Formulas And EquationsChapter 3.1 - The MoleChapter 3.2 - Determining The Formula Of An Unknown CompoundChapter 3.3 - Writing And Balancing Chemical EquationsChapter 3.4 - Calculating Quantities Of Reactant And ProductChapter 4 - Three Major Classes Of Chemical ReactionsChapter 4.1 - Solution Concentration And The Role Of Water As A SolventChapter 4.2 - Precipitation ReactionsChapter 4.3 - Acid-base ReactionsChapter 4.4 - Oxidation-reduction (redox) ReactionsChapter 4.5 - Elements In Redox ReactionsChapter 5 - Gases And The Kinetic-molecular TheoryChapter 5.2 - Gas Pressure And Its MeasurementChapter 5.3 - The Gas Laws And Their Experimental FoundationsChapter 5.4 - Rearrangements Of The Ideal Gas LawChapter 5.5 - The Kinetic-molecular Theory: A Model For Gas BehaviorChapter 6 - Thermochemistry: Energy Flow And Chemical ChangeChapter 6.1 - Forms Of Energy And Their InterconversionChapter 6.2 - Enthalpy: Changes At Constant PressureChapter 6.3 - Calorimetry: Measuring The Heat Of A Chemical Or Physical ChangeChapter 6.4 - Stoichiometry Of Thermochemical EquationsChapter 6.5 - hess’s Law: Finding Δh Of Any ReactionChapter 6.6 - Standard Enthalpies Of Reaction (δhrxn∘)Chapter 7 - Quantum Theory And Atomic StructureChapter 7.1 - The Nature Of LightChapter 7.2 - Atomic SpectraChapter 7.3 - The Wave-particle Duality Of Matter And EnergyChapter 7.4 - The Quantum-mechanical Model Of The AtomChapter 8 - Electron Configuration And Chemical PeriodicityChapter 8.2 - The Quantum-mechanical Model And The Periodic TableChapter 8.3 - Trends In Three Atomic PropertiesChapter 8.4 - Atomic Properties And Chemical ReactivityChapter 9 - Models Of Chemical BondingChapter 9.2 - The Ionic Bonding ModelChapter 9.3 - The Covalent Bonding ModelChapter 9.4 - Bond Energy And Chemical ChangeChapter 9.5 - Between The Extremes: Electronegativity And Bond PolarityChapter 10 - The Shapes Of MoleculesChapter 10.1 - Depicting Molecules And Ions With Lewis StructuresChapter 10.2 - Valence-shell Electron-pair Repulsion (vsepr) TheoryChapter 10.3 - Molecular Shape And Molecular PolarityChapter 11 - Theories Of Covalent BondingChapter 11.1 - Valence Bond (vb) Theory And Orbital HybridizationChapter 11.2 - Modes Of Orbital Overlap And The Types Of Covalent BondsChapter 11.3 - Molecular Orbital (mo) Theory And Electron DelocalizationChapter 12 - Intermolecular Forces: Liquids, Solids, And Phase ChangesChapter 12.2 - Quantitative Aspects Of Phase ChangesChapter 12.3 - Types Of Intermolecular ForcesChapter 12.6 - The Solid State: Structure, Properties, And BondingChapter 13 - The Properties Of Mixtures: Solutions And ColloidsChapter 13.1 - Types Of Solutions: Intermolecular Forces And SolubilityChapter 13.3 - Why Substances Dissolve: Breaking Down The Solution ProcessChapter 13.4 - Solubility As An Equilibrium ProcessChapter 13.5 - Concentration TermsChapter 13.6 - Colligative Properties Of SolutionsChapter 13.7 - The Structure And Properties Of ColloidsChapter 14 - Periodic Patterns In The Main-group ElementsChapter 15 - Organic Compounds And The Atomic Properties Of CarbonChapter 15.2 - The Structures And Classes Of HydrocarbonsChapter 15.3 - Some Important Classes Of Organic ReactionsChapter 15.4 - Properties And Reactivities Of Common Functional GroupsChapter 15.6 - The Monomer-polymer Theme Ii: Biological MacromoleculesChapter 16 - Kinetics: Rates And Mechanisms Of Chemical ReactionsChapter 16.2 - Expressing The Reaction RateChapter 16.3 - The Rate Law And Its ComponentsChapter 16.4 - Integrated Rate Laws: Concentration Changes Over TimeChapter 16.5 - Theories Of Chemical KineticsChapter 16.6 - Reaction Mechanisms: The Steps From Reactant To ProductChapter 16.7 - Catalysis: Speeding Up A ReactionChapter 17 - Equilibrium: The Extent Of Chemical ReactionsChapter 17.2 - The Reaction Quotient And The Equilibrium ConstantChapter 17.3 - Expressing Equilibria With Pressure Terms: Relation Between Kc And KpChapter 17.4 - Comparing Q And K To Determine Reaction DirectionChapter 17.5 - How To Solve Equilibrium ProblemsChapter 17.6 - Reaction Conditions And Equilibrium: Le Chatelier's PrincipleChapter 18 - Acid-base EquilibriaChapter 18.2 - Proton Transfer And The Bronsted Lowry Acid-base DefinitionChapter 18.3 - Autoionization Of Water And The Ph ScaleChapter 18.4 - Strong Acids And Bases And Ph CalculationsChapter 18.5 - Weak Acids And Their Equilibria CalculationsChapter 18.7 - Weak Bases And Their Relation To Weak AcidsChapter 18.8 - Acid-base Properties Of Salt SolutionsChapter 18.10 - Electron-pair Donation And The Lewis Acid-base DefinitionChapter 19 - Ionic Equilibria In Aqueous SystemsChapter 19.1 - Equilibria Of Acid-base BuffersChapter 19.2 - Acid-base Titration CurvesChapter 19.3 - Equilibria Of Slightly Soluble Ionic CompoundsChapter 19.4 - Equilibria Involving Complex IonsChapter 20 - Thermodynamics: Entropy, Free Energy, And Reaction DirectionChapter 20.1 - The Second Law Of Thermodynamics: Predicting Spontaneous ChangeChapter 20.2 - Calculating The Change In Entropy Of A ReactionChapter 20.3 - Entropy, Free Energy, And WorkChapter 20.4 - Free Energy, Equilibrium, And Reaction DirectionChapter 21 - Electrochemistry: Chemical Change And Electrical WorkChapter 21.1 - Redox Reactions And Electrochemical CellsChapter 21.2 - Voltaic Cells: Using Spontaneous Reactions To Generate Electrical EnergyChapter 21.3 - Cell Potential: Output Of A Voltaic CellChapter 21.4 - Free Energy And Electrical WorkChapter 21.7 - Electrolytic Cells: Using Electrical Energy To Drive Nonspontaneous ReactionsChapter 22 - The Elements In Nature And IndustryChapter 23 - Transition Elements And Their Coordination CompoundsChapter 23.1 - Properties Of The Transition ElementsChapter 23.2 - The Inner Transition ElementsChapter 23.3 - Coordination CompoundsChapter 23.4 - Theoretical Basis For The Bonding And Properties Of Complex IonsChapter 24 - Nuclear Reactions And Their ApplicationsChapter 24.1 - Radioactive Decay And Nuclear StabilityChapter 24.2 - The Kinetics Of Radioactive DecayChapter 24.3 - Nuclear Transmutation: Induced Changes In NucleiChapter 24.6 - The Interconversion Of Mass And Energy
Sample Solutions for this Textbook
We offer sample solutions for CHEMISTRY: MOLECULAR...(LL) W/ALEKS homework problems. See examples below:
The change is depicted as follows: Each sphere represents one particle or atom. Atoms from A react...Elements are the simplest form of matter composed of only one type of atom. Hence elements can be...The atomic mass of Al is 26.98 amu and the mass of 1 mol of Al is 26.98 g. The atomic mass of Al is...A water molecule has a bent structure with oxygen atom present as central atom and hydrogen atoms...The gaseous state of matter has a large intermolecular distance between particles with the weakest...The work done by the system and heat released by the system is negative because the final energy of...Ultraviolet and microwave radiations are among the seven electromagnetic radiations. Hence they are...The periodic table is based on the atomic numbers of the elements. The atomic number of tin is 50...On moving across the period in the periodic table, the size of the atoms decreases. Thus the...
Oxygen (1s22s22p4) belongs to the 16th group in the periodic table. It has six valence electrons and...The molecule that has trigonal planar geometry is BF3. The atomic number of boron is 5 so its...The energy of attraction between particles is the potential energy and energy of motion is kinetic...Seawater or salt water contains water, some amino acids, sodium chloride, and some other dissolved...The electronic configuration of hydrogen and lithium are, H = 1S1Li = 1S2,2S1 In generally the full...The compounds that are organic are The compounds that are inorganic areThe reaction rate of the chemical reaction: Reaction rate = -Δ[R]Δt. During the chemical reaction,...According to Le-Chatelier principle, whenever a system is disturbed the system will try to nullify...According to Arrhenius definition, water plays the vital role in the classification acid and bases....Buffer solution: An aqueous solution consisting mixture of weak base and its conjugate acid or weak...Spontaneous process proceeds without outside intervention, whether a chemical or physical change is...The term oxidation is defined as loss of electrons from a compound and it is said to be oxidized....The abundance of hydrogen in universe is far more than earth’s atmosphere. Hydrogen exists as H2 in...It is always one less than the period number. The periodic table consists of sublevel blocks...Change in energy during a chemical reaction is relatively small. In the case of nuclear reaction...
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