Chemistry9th EditionSteven S. Zumdahl Publisher: Cengage LearningISBN: 9781133611097
Chemistry
Solutions for Chemistry
Problem 1RQ:
Use Daltons atomic theory to account for each of the following. a. the law of conservation of mass...Problem 3RQ:
What discoveries were made by J. J. Thomson, Henri Becquerel, and Lord Rutherford? How did Daltons...Problem 4RQ:
Consider Ernest Rutherfords -particle bombardment experiment illustrated in Fig. 2.12. How did the...Problem 5RQ:
Do the proton and the neutron have exactly the same mass? How do the masses of the proton and...Problem 6RQ:
What is the distinction between atomic number and mass number? Between mass number and atomic mass?Problem 7RQ:
Distinguish between the terms family and period in connection with the periodic table. For which of...Problem 8RQ:
The compounds AlCl3, CrCl3, and ICl3 have similar formulas, yet each follows a different set of...Problem 10RQ:
How would you name HBrO4, KIO3, NaBrO2, and HIO? Refer to Table 2.5 and the acid nomenclature...Problem 1ALQ:
Which of the following is true about an individual atom? Explain. a. An individual atom should be...Problem 2ALQ:
How would you go about finding the number of chalk molecules it takes to write your name on the...Problem 3ALQ:
These questions concern the work of J. J. Thomson. a. From Thomsons work, which particles do you...Problem 5ALQ:
You have a chemical in a sealed glass container filled with air. The setup is sitting on a balance...Problem 6ALQ:
The formula of water is If-O. Which of the following is indicated by this formula? Explain your...Problem 7ALQ:
You may have noticed that when water boils, you can see bubbles that rise to die surface of the...Problem 8ALQ:
One of the best indications of a useful theory is that it raises more questions for further...Problem 11ALQ:
Label each of the following as an atomic element, a molecular element, or a compound.Problem 15ALQ:
Which of tire following explain how an ion is formed'? Explain your answer. a. adding or subtracting...Problem 16Q:
What refinements had to be made in Daltons atomic theory to account for Gay-Lussacs results on the...Problem 17Q:
When hydrogen is burned in oxygen to form water, the composition of water formed does not depend on...Problem 18Q:
The two most reactive families of elements are the halogens and the alkali metals. How do they...Problem 19Q:
Explain the law of conservation of mass, the law of definite proportion, and the law of multiple...Problem 20Q:
Section 2.3 describes the postulates of Daltons atomic theory. With some modifications, these...Problem 21Q:
The contributions of J. J. Thomson and Ernest Rutherford led the way to todays understanding of the...Problem 23Q:
The number of protons in an atom determines the identity of the atom. What does the number and...Problem 24Q:
If the volume of a proton were similar to the volume of an electron, how will the densities of these...Problem 26Q:
List some characteristic properties that distinguish die metallic elements from the nonmetallic...Problem 27Q:
Consider the elements of Group 4A (the carbon family): C, Si, Ge, Sn, and Pb. What is the trend in...Problem 28Q:
Distinguish between the following terms. a. molecule versus ion b. covalent bonding versus ionic...Problem 29Q:
Label the type of bonding for each of the following.Problem 30Q:
The vitamin niacin (nicotinic acid. C6H5NO2) can be isolated from a variety of natural sources such...Problem 33E:
When mixtures of gaseous H2 and gaseous Cl2 react, a product forms that has the same properties...Problem 34E:
Observations of the reaction between nitrogen gas and hydrogen gas show us that 1 volume of nitrogen...Problem 35E:
A sample of chloroform is found to contain 12.0 g of carbon, 106.4 g of chlorine, and 1.01 g of...Problem 36E:
A sample of H2SO4 contains 2.02 g of hydrogen, 32.07 g of sulfur, and 64.00 g of oxygen. How many...Problem 37E:
Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of hydrogen...Problem 38E:
Consider 100.0-g samples of two different compounds consisting only of carbon and oxygen. One...Problem 39E:
The three most stable oxides of carbon ire carbon monoxide (CO), carbon dioxide (CO2), and carbon...Problem 40E:
Two elements. R and Q, combine to form two binary compounds. In the first compound, 14.0 g of R...Problem 41E:
In Section 1.1 of the text, the concept of a chemical reaction was introduced with the example of...Problem 42E:
In a combustion reaction, 46.0 g of ethanol reacts with 96.0 g of oxygen to produce water and carbon...Problem 43E:
Early tables of atomic weights (masses) were generated by measuring the mass of a substance that...Problem 44E:
Indium oxide contains 4.784 g of indium for every 1.000 g of oxygen. In 1869, when Mendeleev first...Problem 46E:
If you wanted to make an accurate scale model of the hydrogen atom and decided that the nucleus...Problem 47E:
In an experiment it was found that the total charge on an oil drop was 5.93 1018 C. How many...Problem 48E:
A chemist in a galaxy tar, far away performed the Millikan oil drop experiment and got the following...Problem 49E:
What are the symbols of the following metals: sodium, radium, iron, gold, manganese, lead?Problem 50E:
What are the symbols of the following nonmetals: fluorine, chlorine, bromine, sulfur, oxygen,...Problem 52E:
Give the names of the nonmetals that correspond to the following symbols: As, I, Xe, He, C, Si.Problem 53E:
a. Classify the following elements as metals or nonmetals: Mg Si Rn Ti Ge Rn Au B Am Bi At Br b. The...Problem 54E:
a. List the noble gas elements. Which of the noble gases has only radioactive isotopes? (This...Problem 55E:
For each of the following sets of elements, label each as either noble gases, halogens, alkali...Problem 58E:
Write the atomic symbol (ZAX) for each of the isotopes described below. a. number of protons = 27,...Problem 60E:
For carbon-14 and carbon-12, how many protons and neutrons are in each nucleus? Assuming neutral...Problem 61E:
How many protons and neutrons are in the nucleus of each of the following atoms? In a neutral atom...Problem 63E:
For each of the following ions, indicate the number of protons and electrons the ion contains. a....Problem 64E:
How many protons, neutrons, and electrons are in each of the following atoms or ions? a. 1224Mg b....Problem 66E:
What is the symbol of an ion with 16 protons, 18 neutrons, and 18 electrons? What is the symbol for...Problem 67E:
Complete the following table: Symbol Number of Protons in Nucleus Number of Neutrons in Nucleus...Problem 68E:
Complete the following table: Symbol Number of Protons in Nucleus Number of Neutrons in Nucleus...Problem 69E:
Would you expect each of the following atoms to gain or lose electrons when forming ions? What ion...Problem 71E:
Name the compounds in parts ad and write the formulas for the compounds in parts eh. a. NaBr b. Rb2O...Problem 72E:
Name the compounds in parts a-d and write the formulas for the compounds in parts eh. a. Hg2O b....Problem 84E:
Write the formula for each of the following compounds a. chromium(VI) oxide b. disulfur dichloride...Problem 86E:
Write the formula for each of the following compounds: a. ammonium hydrogen phosphate b. mercury (I)...Problem 88E:
Each of the following compounds is incorrectly named is wrong with each name, and what is the...Problem 89AE:
Chlorine has two natural isotopes: 1737Cl and 1735Cl. Hydrogen reacts with chlorine to form the...Problem 90AE:
What are the symbols for the following nonmetal elements that are most often present in compounds...Problem 91AE:
Four Fe2+ ions are key components of hemoglobin, the protein that transports oxygen in the blood....Problem 92AE:
Which of the following statements is(are) true? For the false statements, correct them. a. All...Problem 93AE:
The isotope of an unknown element, X, has a mass number of 79. The most stable ion of the isotope...Problem 96AE:
Identify each of the following elements: a. a member of the same family as oxygen whose most stable...Problem 103CWP:
Complete the following table. Atom/Ion Protons Neutrons Electrons S50120n M1225g2+ F2656e2+ S3479e...Problem 104CWP:
Which of the following is{are) correct? a. 40Ca2 contains 20 protons and 18 electrons. b. Rutherford...Problem 110CP:
Reaction of 2.0 L of hydrogen gas with 1.0 L of oxygen gas yields 2.0 L of water vapor. All gases...Problem 111CP:
A combustion reaction involves the reaction of a substance with oxygen gas. The complete combustion...Problem 112CP:
A chemistry instructor makes the following claim: Consider that if the nucleus were the size of a...Problem 113CP:
The early alchemists used to do an experiment in which water was boiled for several days in a sealed...Problem 114CP:
Consider the chemical reaction as depicted below. Label as much as you can using the terms atom,...Problem 115CP:
Each of the following statements is true, but Dalton might have had trouble explaining some of them...Problem 116CP:
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as...Problem 117CP:
A single molecule has a mass of 7.31 1023 g. Provide an example of a real molecule that can have...Browse All Chapters of This Textbook
Chapter 1 - Chemical FoundationsChapter 2 - Atoms, Molecules, And IonsChapter 3 - StoichiometryChapter 4 - Types Of Chemical Reactions And Solution StoichiometryChapter 5 - GasesChapter 6 - ThermochemistryChapter 7 - Atomic Structure And PeriodicityChapter 8 - Bonding: General ConceptsChapter 9 - Covalent Bonding: OrbitalsChapter 10 - Liquids And Solids
Chapter 11 - Properties Of SolutionsChapter 12 - Chemical KineticsChapter 13 - Chemical EquilibriumChapter 14 - Acids And BasesChapter 15 - Acid-base EquilibriaChapter 16 - Solubility And Complex Ion EquilibriaChapter 17 - Spontaneity, Entropy, And Free EnergyChapter 18 - ElectrochemistryChapter 19 - The Nucleus: A Chemist's ViewChapter 20 - The Representative ElementsChapter 21 - Transition Metals And Coordination ChemistryChapter 22 - Organic And Biological Molecules
Book Details
1. Chemical Foundations.
2. Atoms, Molecules, and Ions.
3. Stoichiometry.
4. Types of Chemical Reactions and Solution Stoichiometry.
5. Gases
6. Thermochemistry.
7. Atomic Structure and Periodicity.
8. Bonding: General Concepts.
9. Covalent Bonding: Orbitals.
10. Liquids and Solids.
11. Properties of Solutions.
12. Chemical Kinetics.
13. Chemical Equilibrium.
14. Acids and Bases.
15. Acid-Base Equilibria.
16. Solubility and Complex Ion Equilibria.
17. Spontaneity, Entropy, and Free Energy.
18. Electrochemistry.
19. The Nucleus: A Chemist's View.
20. The Representative Elements.
21. Transition Metals and Coordination Chemistry.
22. Organic and Biological Molecules.
Appendix 1. Mathematical Procedures.
A1.1 Exponential Notation.
A1.2 Logarithms.
A1.3 Graphing Functions.
A1.4 Solving Quadratic Equations.
A1.5 Uncertainties in Measurements.
Appendix 2. The Quantitative Kinetic Molecular Model.
Appendix 3. Spectral Analysis.
Appendix 4. Selected Thermodynamic Data.
Appendix 5. Equilibrium Constants and Reduction Potentials.
A5.1 Values of Ka for Some Common Monoprotic Acids.
A5.2 Stepwise Dissociation Constants for Several Common Polyprotic Acids.
A5.3 Values of Kb for Some Common Weak Bases.
A5.4 Ksp Values at 25_C for Common Ionic Solids.
A5.5 Standard Reduction Potentials at 25_C (298K) for Many Common Half-Reactions.
Appendix 6. SI Units and Conversion Factors.
Glossary.
Answers to Selected Exercises.
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2. Atoms, Molecules, and Ions.
3. Stoichiometry.
4. Types of Chemical Reactions and Solution Stoichiometry.
5. Gases
6. Thermochemistry.
7. Atomic Structure and Periodicity.
8. Bonding: General Concepts.
9. Covalent Bonding: Orbitals.
10. Liquids and Solids.
11. Properties of Solutions.
12. Chemical Kinetics.
13. Chemical Equilibrium.
14. Acids and Bases.
15. Acid-Base Equilibria.
16. Solubility and Complex Ion Equilibria.
17. Spontaneity, Entropy, and Free Energy.
18. Electrochemistry.
19. The Nucleus: A Chemist's View.
20. The Representative Elements.
21. Transition Metals and Coordination Chemistry.
22. Organic and Biological Molecules.
Appendix 1. Mathematical Procedures.
A1.1 Exponential Notation.
A1.2 Logarithms.
A1.3 Graphing Functions.
A1.4 Solving Quadratic Equations.
A1.5 Uncertainties in Measurements.
Appendix 2. The Quantitative Kinetic Molecular Model.
Appendix 3. Spectral Analysis.
Appendix 4. Selected Thermodynamic Data.
Appendix 5. Equilibrium Constants and Reduction Potentials.
A5.1 Values of Ka for Some Common Monoprotic Acids.
A5.2 Stepwise Dissociation Constants for Several Common Polyprotic Acids.
A5.3 Values of Kb for Some Common Weak Bases.
A5.4 Ksp Values at 25_C for Common Ionic Solids.
A5.5 Standard Reduction Potentials at 25_C (298K) for Many Common Half-Reactions.
Appendix 6. SI Units and Conversion Factors.
Glossary.
Answers to Selected Exercises.
Information For
College Faculty
College Student
Library Professional
Institutional Purchaser
Business/Professional Learner
ESL/ELT Educator
Grades PreK-8 Educator
Grades 9-12 Educator
Connect
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Contact Us
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Library Tech Support
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Sample Solutions for this Textbook
We offer sample solutions for Chemistry homework problems. See examples below:
Chapter 1, Problem 1RQChapter 1, Problem 30EChapter 1, Problem 35EChapter 1, Problem 36EChapter 1, Problem 38EChapter 1, Problem 45EChapter 1, Problem 57EChapter 1, Problem 59EChapter 1, Problem 60E
Chapter 1, Problem 63EChapter 1, Problem 64EChapter 1, Problem 73EChapter 1, Problem 113CPChapter 2, Problem 1RQChapter 2, Problem 64EChapter 2, Problem 67EChapter 2, Problem 68EExplanation: Atomic number given is 13. From the periodic table we can identify that the element...Chapter 2, Problem 71EExplanation: To determine: The naming of CuI The name of CuI is copper(I) iodide. In naming of...Explanation: To determine: The naming of HC2H3O2 The naming of HC2H3O2 is acetic acid. Rules for...To determine: The formula of of sulfur difluoride The formula of sulfur difluoride is SF2 Sulfur...Explanation: To determine: The formula of sodium oxide. The formula of sodium oxide is Na2O The...Chapter 2, Problem 86EChapter 2, Problem 88EExplanation: To determine: The formula and the name of the binary compound formed from Ca and N. The...Explanation: To determine: The explanation for the term “counting by weighing”. The stated concept,...Chapter 3, Problem 59EChapter 3, Problem 60EChapter 3, Problem 61EExplanation: Given The mass of P4O6 is 1.00 g . The molar mass of P4O6 is 219.866 g/mol . Formula...Chapter 3, Problem 64EChapter 3, Problem 67EChapter 3, Problem 68EChapter 3, Problem 71EChapter 3, Problem 73EChapter 3, Problem 76EChapter 3, Problem 79EChapter 3, Problem 100EChapter 3, Problem 109EChapter 3, Problem 119EChapter 3, Problem 121EChapter 3, Problem 124EChapter 3, Problem 150AEChapter 3, Problem 152CWPChapter 3, Problem 180IPChapter 4, Problem 1RQChapter 4, Problem 7RQExplanation: NaBr(s)→Na(aq)++Braq- Figure 1 Let us consider the above molecular-level pictures of...Explanation: Record the given data Moles of Sodium phosphate= 0.200 moles Volume of the solution=...Chapter 4, Problem 66EChapter 4, Problem 79EChapter 4, Problem 82EChapter 4, Problem 93AEChapter 4, Problem 121CPChapter 4, Problem 122CPChapter 4, Problem 123CPExplanation Record the given data Mass of the sample mixture = 0.205 g Mass of the precipitate =...Explanation: Given: Record the given data Upstream at which the stream rate flows = 5.00×104 L/s...Chapter 4, Problem 144MPChapter 4, Problem 145MPA barometer consists of Mercury column that is tipped inverted and positioned in a dish containing...Chapter 5, Problem 41EExplanation: The relation between pressures measured in the manometers containing mercury and...Explanation According to ideal gas equation, PV=nRT By rearranging the above equation, PVnT=R Since...Chapter 5, Problem 88EExplanation: To find: the mole fractions of CH4 and O2 in the given mixture if the partial pressure...Explanation To find: the number of moles of dimethyl hydrazine from its given mass. The number of...Explanation To determine: The partial pressure of carbon monoxide Partial pressure of carbon...Explanation To determine: The mixing ratio of benzene Mixing ratio of benzene = 9.47 × 10-3ppmv For...Explanation: The mass percent from the given data is, 26.1% Carbon13.1% Hydrogen61.0% Nitrogen Mass...Chapter 5, Problem 135AEExplanation To find: the empirical formula of the compound Convert the mass percent to gram 58.51%...Chapter 5, Problem 139AEChapter 5, Problem 152CPChapter 5, Problem 153CPExplanation To determine: Mass of hot air when the average molar mass of air 29.0g/mol Mass of hot...Chapter 5, Problem 162IPChapter 6, Problem 1RQChapter 6, Problem 20QChapter 6, Problem 34EChapter 6, Problem 50EChapter 6, Problem 52EChapter 6, Problem 79EChapter 6, Problem 80EExplanation: The balanced equation is: a) N2(g)→N2(l) In (a) the volume of products is decreases...Chapter 6, Problem 108AEChapter 6, Problem 115AEChapter 6, Problem 130CPChapter 6, Problem 131CPChapter 6, Problem 134IPChapter 6, Problem 135IPChapter 6, Problem 137MPChapter 7, Problem 1RQChapter 7, Problem 24QChapter 7, Problem 43EChapter 7, Problem 57EChapter 7, Problem 58EChapter 7, Problem 61EChapter 7, Problem 62EChapter 7, Problem 63EChapter 7, Problem 74EChapter 7, Problem 79EChapter 7, Problem 81EChapter 7, Problem 82EChapter 7, Problem 86EChapter 7, Problem 87EChapter 7, Problem 94EChapter 7, Problem 95EChapter 7, Problem 97EChapter 7, Problem 142AEChapter 7, Problem 171CPChapter 8, Problem 1RQExplanation: Refer to figure 3-4. The electro negativity of carbon (C) , nitrogen (N) , and oxygen...Explanation: Refer to figure 3-4 The electro negativity of Sodium (Na) Potassium (K) and Rubidium...Chapter 8, Problem 46EChapter 8, Problem 47EChapter 8, Problem 49EExplanation: In a periodic table the size of ions depends on the nuclear attraction on the valence...Chapter 8, Problem 54EChapter 8, Problem 62EChapter 8, Problem 81EChapter 8, Problem 84EChapter 8, Problem 89EChapter 8, Problem 101EChapter 8, Problem 102EChapter 8, Problem 129AEChapter 8, Problem 154CPChapter 8, Problem 155CPChapter 9, Problem 1RQChapter 9, Problem 23EChapter 9, Problem 24EChapter 9, Problem 26EChapter 9, Problem 29EChapter 9, Problem 30EChapter 9, Problem 39EChapter 9, Problem 52EChapter 9, Problem 53EChapter 9, Problem 63AEChapter 9, Problem 89CPChapter 10, Problem 1RQChapter 10, Problem 41EExplanation: CCl4 , CBr4, CF4 Identify the compound which has highest boiling point and justify it....Chapter 10, Problem 53EChapter 10, Problem 55EChapter 10, Problem 56EChapter 10, Problem 57EChapter 10, Problem 58EChapter 10, Problem 59EChapter 10, Problem 60EChapter 10, Problem 62EChapter 10, Problem 80EChapter 10, Problem 88EChapter 10, Problem 131CPChapter 10, Problem 146CPChapter 10, Problem 148IPExplanation: To explain molarity Molarity can be defined as moles of solute to litres of solution....Chapter 11, Problem 16SRChapter 11, Problem 31EExplanation: Record the given data Gram equivalent of HCl = 0.25 Molarity of HCl = 0.25 M To...Explanation: KrF2 8+2(7)=22e- KrF2 is dissolves in CCl4 . KrF2 is non-polar molecule that makes it...Chapter 11, Problem 55EChapter 11, Problem 79EExplanation: Record the given data, Molality of MgCl2= 0.050 m Molality of FeCl3= 0.050 m To...Explanation: Record the given data, Molality of MgCl2= 0.050 m Molality of FeCl3= 0.050 m To...Explanation: To find the Acetone and water polarity CH3COCH3 and H2O The electrostatic possible...Explanation: Record the given data, Freezing point of an aqueous solution =- 2.79°C To calculate...Mass of Sodium = 285-315 mg Mass of Potassium = 14.1-17.3 mg Mass of Calcium = 4.9-6.0 mg Mass of...Chapter 11, Problem 109AEChapter 11, Problem 120CPChapter 11, Problem 132IPChapter 12, Problem 1RQChapter 12, Problem 30EChapter 12, Problem 33EChapter 12, Problem 35EChapter 12, Problem 36EChapter 12, Problem 58EChapter 12, Problem 84AEChapter 12, Problem 86AEChapter 12, Problem 87AEChapter 12, Problem 91AEChapter 12, Problem 93AEChapter 12, Problem 105CPChapter 12, Problem 112CPChapter 13, Problem 1RQChapter 13, Problem 5ALQChapter 13, Problem 23EChapter 13, Problem 39EChapter 13, Problem 42EChapter 13, Problem 54EChapter 13, Problem 56EChapter 13, Problem 57EChapter 13, Problem 72AEChapter 13, Problem 73AEChapter 13, Problem 78AEChapter 13, Problem 104CPChapter 13, Problem 106CPChapter 14, Problem 1RQChapter 14, Problem 49EChapter 14, Problem 50EChapter 14, Problem 51EChapter 14, Problem 52EChapter 14, Problem 63EChapter 14, Problem 64EChapter 14, Problem 68EChapter 14, Problem 73EChapter 14, Problem 74EExplanation: To determine: The pH, [H+] and [OH−] of (C2H5)3N . The equilibrium constant expression...Chapter 14, Problem 101EChapter 14, Problem 107EChapter 14, Problem 108EChapter 14, Problem 109EChapter 14, Problem 119EChapter 14, Problem 120EChapter 14, Problem 123EChapter 14, Problem 126EChapter 14, Problem 151AEChapter 15, Problem 1RQChapter 15, Problem 7RQChapter 15, Problem 43EChapter 15, Problem 57EChapter 15, Problem 58EChapter 15, Problem 59EChapter 15, Problem 60EChapter 15, Problem 61EChapter 15, Problem 62EChapter 15, Problem 63EChapter 15, Problem 64EChapter 15, Problem 65EExplanation The value of pH of solution when 0.0 mL NaOH has been added is. 1.0_ . Given: The...Chapter 15, Problem 107CWPChapter 16, Problem 1RQExplanation To determine: The solubility product of CaC2O4 . The concentration of Ca2+ is 4.8×10−5...Chapter 16, Problem 22EChapter 16, Problem 27EChapter 16, Problem 28EChapter 16, Problem 35EChapter 16, Problem 36EChapter 16, Problem 37EChapter 16, Problem 40EChapter 16, Problem 53EChapter 16, Problem 70EChapter 16, Problem 102CPChapter 17, Problem 1RQChapter 17, Problem 53EChapter 17, Problem 54EChapter 17, Problem 63EChapter 17, Problem 64EChapter 17, Problem 68EChapter 17, Problem 70EChapter 17, Problem 72EChapter 17, Problem 74EChapter 17, Problem 78EChapter 17, Problem 86AEChapter 17, Problem 90AEChapter 17, Problem 119MPChapter 18, Problem 1RQChapter 18, Problem 16RORRExplanation: Given: I- (aq) + ClO- (aq) →I3− (aq) + Cl-(aq) To write the equations for two...Explanation: Given: Cu (s) + NO3- (aq) →Cu2+ (aq) + NO(g) To write the equations for two...Chapter 18, Problem 47EChapter 18, Problem 75EChapter 18, Problem 76EChapter 18, Problem 85EChapter 18, Problem 86EChapter 18, Problem 95EChapter 18, Problem 115AEChapter 18, Problem 117AEExplanation: Given The given reaction is, Fe(s)+HCl(aq)→HFeCl4(aq)+H2(g) . In this equation, the...Chapter 18, Problem 144CPExplanation The half cell reactions are, Anode: Hg→Hg2++2e− Eanodeο=0.242 V Cathode: 2Ag++2e−→2Ag...Chapter 18, Problem 153CPChapter 18, Problem 159MPExplanation (a) To define: The term thermodynamic stability. The thermodynamic stability is related...Explanation: Alpha particle is emitted. The parent nuclide is 232Th and the nuclide after the...Explanation The most stable isotope is 81Kr and the hottest one is 73Kr The nuclides having longer...Explanation Given The atomic mass of 232Pu is 3.85285×10−22 g . The mass of a neutron is...Explanation The atomic mass of 11H=1.0078 amu The mass of a neutron is 1.0087 amu . Mass of...Explanation Given The value of half life of 87Rb is 4.5×109 years . The decay constant is calculated...Explanation The decay constant is calculated by the formula given below. λ=0.693t1/2 Where t1/2 is...Explanation: The zirconium metal is capable of reducing water to form hydrogen gas at standard...Explanation The number of α and β particles produced are 4_ and 2_ . The mass number of 92238U is...Explanation The nuclear reaction for the synthesis of cobalt- 60 is, 2658Fe+201n→ 2760Co+ −10e . The...Chapter 20, Problem 1RQExplanation The valence electron configuration for halogens is ns2np5 . The common halogen elements...Explanation The value of ΔH° for the given reaction is 180 kJ_ . The stated reaction is,...Explanation: The compound XeO4 and IO4− ion are isoelectronic. The molecule xenon tetroxide (XeO4)...Explanation: The Lewis structure, molecular structure, bond angle and hybridization of central atom...Explanation Given Dimension of room is 10.0 m×10.0 m×10.0 m . Temperature is 25 °C . Pressure is...Explanation: Hydrogen gas is produced by reacting graphite with water. C(s)+H2O(g)→CO(g)+H2(g) The...Explanation: The number of moles of hydrogen gas is 0.249 mol_. Given Mass of alkaline earth metal...Explanation: Mass of radon (Ra) is 25 g_ . Given Mass of pitch-blende is 1.75×108 g . The conversion...Explanation Given Temperature is 900 K . Pressure of In(CH3)3 is 2.00 atm . Volume of In(CH3)3 is...Chapter 20, Problem 108IPChapter 20, Problem 109IPChapter 21, Problem 1RQExplanation: (I) To determine: The geometry and associated bond angles when a metal ion has a...Explanation: Atomic number of Nickel is 28 . Accordingly the electronic configuration is –...Explanation: Atomic number of Nickel is 22 . Accordingly the electronic configuration is –...EXPLANATION (a) To write: The electron configuration of metal ion in (NH4)2[Fe(H2O)2Cl4] . The...Explanation The complex ion is [Ru(NH3)5Cl]2+. This ion contains positive charge. Oxidation state of...Explanation The complex compound is [Co(NH3)6]Cl2 . Oxidation state of Chlorine ion (Cl−) is −1 ....Explanation The complex compound is [Cr(H2O)5Br]Br2 . Oxidation state of Bromine ion (Br−) is −1 ....Explanation The value of ΔH° for the given reaction is −11 kJ_ . For the reaction,...Explanation The reaction that takes place is, 3Fe2O3(s)+CO(g)→2Fe3O4(s)+CO2(g) Refer to Appendix 4....Explanation The given equations are, Co+3+e−→Co+2 Eο=1.82 V (1) Co2++3en→Co(en)32+ K=1.5×1012 (2)...Chapter 21, Problem 99IPChapter 22, Problem 1RQChapter 22, Problem 5RQExplanation: The type of isomerism that could be exhibited by C6H12 and an example that illustrates...Chapter 22, Problem 16EChapter 22, Problem 45EExplanation To determine: The monomer of the given polymer. The monomer is vinyl fluoride. It is an...Explanation The correct name of the compound is 2,3,5,6−Tetramethyl−octane whose structure is shown...Explanation The structure of the given compound 2,3,7,8−tetrachloro−dibenzo−p−dioxin is shown in...Chapter 22, Problem 130AEChapter 22, Problem 136AEExplanation The equilibrium constant for the given reaction is 6.88×10−13_ . The equilibrium...Chapter 22, Problem 148CPExplanation The structure of C5H12 is shown in Figure 1. The structure of C5H12 is, Figure 1 The...Explanation The structure of the polymer of ABS plastic is shown in figure 1. The reaction of Abs...Explanation Given Electronic configuration of M+2 is [Ar]3d10. So, atomic number of M is 30. In...Explanation The empirical formula of the given helicene is C5H3 . Helicene is an aromatic compound...The correct responses are urea and Ammonium cyanate. The first organic compound that is synthesized...Explanation Aldohexose is a six carbon aldehyde sugar with an aldehyde group on one end.
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ISBN: 8220100453809
CHEMISTRY,AP EDITION-W/ACCESS (HS)
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11th Edition
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Chemistry Iae 7ed
7th Edition
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7th Edition
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5th Edition
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4th Edition
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8th Edition
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8th Edition
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