Solutions for Chemistry: A Molecular Approach
Problem 2SAQ:
Q2. Which sample is most likely to undergo the smallest change in temperature upon the absorption of...Problem 4SAQ:
Q4. A 12.5-g sample of granite initially at 82.0 °C is immersed into 25.0 g of water initially at...Problem 5SAQ:
Q5. A cylinder with a moving piston expands from an initial volume of 0.250 L against an external...Problem 6SAQ:
Q6. When a 3.80-g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature...Problem 7SAQ:
Q7. Hydrogen gas reacts with oxygen to form water:
2 H2(g) + O2(g) → 2 H2O(g) ΔH = –483.5...Problem 15SAQ:
Q15. Natural gas burns in air to form carbon dioxide and water, releasing heat.
CH4(g) + O2(g) →...Problem 1E:
1. What is thermochemistry? Why is it important?
Problem 4E:
4. State the law of conservation of energy. How does it relate to energy exchanges between a...Problem 10E:
10. If energy flows out of a chemical system and into the surroundings, what is the sign of...Problem 11E:
11. If the internal energy of the products of a reaction is higher than the internal energy of the...Problem 14E:
14. Explain how the sum of heat and work can be a state function, even though heat and work are...Problem 15E:
15. What is heat capacity? Explain the difference between heat capacity and specific heat capacity.
Problem 16E:
16. Explain how the high specific heat capacity of water can affect the weather in coastal regions.
Problem 17E:
17. If two objects, A and B, of different temperature come into direct contact, what is the...Problem 19E:
19. What is calorimetry? Explain the difference between a coffee-cup calorimeter and a bomb...Problem 20E:
20. What is the change in enthalpy (ΔH) for a chemical reaction? How is ΔH different from ΔE?
Problem 21E:
21. Explain the difference between an exothermic and an endothermic reaction. Give the sign of ΔH...Problem 22E:
22. From a molecular viewpoint, where does the energy emitted in an exothermic chemical reaction...Problem 23E:
23. From a molecular viewpoint, where does the energy absorbed in an endothermic chemical reaction...Problem 24E:
24. Is the change in enthalpy for a reaction an extensive property? Explain the relationship between...Problem 36E:
36. A particular frost-free refrigerator uses about 745 kWh of electrical energy per year. Express...Problem 37E:
37. Which statement is true of the internal energy of a system and its surroundings during an energy...Problem 39E:
39. Identify each energy exchange as primarily heat or work and determine whether the sign of ΔE is...Problem 40E:
40. Identify each energy exchange as primarily heat or work and determine whether the sign of ΔE is...Problem 41E:
41. A system releases 622 kJ of heat and does 105 kJ of work on the surroundings. What is the change...Problem 42E:
42. A system absorbs 196 kJ of heat and the surroundings do 117 kJ of work on the system. What is...Problem 43E:
43. The gas in a piston (defined as the system) warms and absorbs 655 J of heat. The expansion...Problem 47E:
47. How much heat is required to warm 1.50 L of water from 25.0 °C to 100.0 °C? (Assume a density of...Problem 49E:
49. Suppose that 25 g of each substance is initially at 27.0 °C. What is the final temperature of...Problem 50E:
50. An unknown mass of each substance, initially at 23.0 °C, absorbs 1.95 × 103 J of heat. The final...Problem 51E:
51. How much work (in J) is required to expand the volume of a pump from 0.0 L to 2.5 L against an...Problem 53E:
53. The air within a piston equipped with a cylinder absorbs 565 J of heat and expands from an...Problem 54E:
54. A gas is compressed from an initial volume of 5.55 L to a final volume of 1.22 L by an external...Problem 55E:
55. When 1 mol of a fuel burns at constant pressure, it produces 3452 kJ of heat and does 11 kJ of...Problem 56E:
56. The change in internal energy for the combustion of 1.0 mol of octane at a pressure of 1.0 atm...Problem 57E:
57. Determine whether each process is exothermic or endothermic and indicate the sign of ΔH.
a....Problem 58E:
58. Determine whether each process is exothermic or endothermic and indicate the sign of ΔH.
a. dry...Problem 59E:
59. Consider the thermochemical equation for the combustion of acetone (C3H6O), the main ingredient...Problem 60E:
60. What mass of natural gas (CH4) must burn to emit 267 kJ of heat?
CH4(g) + 2 O2(g) → CO2(g) + 2...Problem 63E:
63. The propane fuel (C3H8) used in gas barbeques burns according to the thermochemical...Problem 65E:
65. A silver block, initially at 58.5 °C, is submerged into 100.0 g of water at 24.8 °C, in an...Problem 67E:
67. A 31.1-g wafer of pure gold, initially at 69.3 °C, is submerged into 64.2 g of water at 27.8 °C...Problem 70E:
70. A 2.74-g sample of a substance suspected of being pure gold is warmed to 72.1 °C and submerged...Problem 71E:
71. Exactly 1.5 g of a fuel burns under conditions of constant pressure and then again under...Problem 72E:
72. In order to obtain the largest possible amount of heat from a chemical reaction in which there...Problem 73E:
73. When 0.514 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature...Problem 75E:
75. Zinc metal reacts with hydrochloric acid according to the balanced equation:
Zn(s) + 2 HCl(aq) →...Problem 79E:
79. Calculate ΔHrxn for the reaction:
Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)
Use the following...Problem 80E:
80. Calculate ΔHrxn for the reaction:
CaO(s) + CO2(g) → CaCO3(s)
Use the following reactions and...Problem 81E:
81. Calculate ΔHrxn for the reaction:
5 C(s) + 6 H2(g) → C5H12(l)
Use the following reactions and...Problem 82E:
82. Calculate ΔHrxn for the reaction:
CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g)
Use the following...Problem 83E:
83. Write an equation for the formation of each compound from its elements in their standard states,...Problem 85E:
85. Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4 according to...Problem 89E:
89. During photosynthesis, plants use energy from sunlight to form glucose (C6H12O6) and oxygen from...Problem 91E:
91. Top fuel dragsters and funny cars burn nitromethane as fuel according to the balanced combustion...Problem 92E:
92. The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact...Problem 93E:
93. Determine the mass of CO2 produced by burning enough of each fuel to produce 1.00 × 102 kJ of...Problem 99E:
99. Evaporating sweat cools the body because evaporation is an endothermic process:
H2O(l) →...Problem 101E:
101. Use standard enthalpies of formation to calculate the standard change in enthalpy for the...Problem 102E:
102. Dry ice is solid carbon dioxide. Instead of melting, solid carbon dioxide sublimes according to...Problem 103E:
103. A 25.5-g aluminum block is warmed to 65.4 °C and plunged into an insulated beaker containing...Problem 107E:
107. Derive a relationship between ΔH and ΔE for a process in which the temperature of a fixed...Problem 112E:
112. When 10.00 g of phosphorus is burned in O2(g) to form P4O10(s), enough heat is generated to...Problem 113E:
113. The ?H for the oxidation of sulfur in the gas phase to SO3 is –204 kJ/mol and for the oxidation...Problem 114E:
114. The of TiI3(s) is –328 kJ/mol and the ΔH° for the reaction 2 Ti(s) + 3 I2(g) → 2 TiI3(s) is...Problem 118E:
118. A pure gold ring and a pure silver ring have a total mass of 14.9 g. The two rings are heated...Problem 131E:
131. Which statement is true of the internal energy of the system and its surroundings following a...Problem 133E:
133. Which expression describes the heat evolved in a chemical reaction when the reaction is carried...Problem 135E:
135. A 1-kg cylinder of aluminum and 1-kg jug of water, both at room temperature, are put into a...Browse All Chapters of This Textbook
Chapter 1 - Matter, Measurement, And Problem SolvingChapter 2 - Atoms And ElementsChapter 3 - Molecules, Compounds, And Chemical EquationsChapter 4 - Chemical Quantities And Aqueous ReactionsChapter 5 - GasesChapter 6 - ThermochemistryChapter 7 - The Quantum-mechanical Model Of The AtomChapter 8 - Periodic Properties Of The ElementsChapter 9 - Chemical Bonding I: The Lewis ModelChapter 10 - Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, And Molecular Orbital Theory
Chapter 11 - Liquids, Solids, And Intermolecular ForcesChapter 12 - SolutionsChapter 13 - Chemical KineticsChapter 14 - Chemical EquilibriumChapter 15 - Acids And BasesChapter 16 - Aqueous Ionic EquilibriumChapter 17 - Free Energy And ThermodynamicsChapter 18 - ElectrochemistryChapter 19 - Radioactivity And Nuclear ChemistryChapter 20 - Organic ChemistryChapter 21 - BiochemistryChapter 22 - Chemistry Of The NonmentalsChapter 23 - Metals And MetallurgyChapter 24 - Transition Metals And Coordination Compounds
Book Details
Chemistry: A Molecular Approach, Third Edition is an innovative, pedagogically driven text that explains challenging concepts in a student-oriented manner. Nivaldo Tro creates a rigorous and accessible treatment of general chemistry in the context of relevance and the big picture. Chemistry is presented visually through multi-level images - macroscopic, molecular, and symbolic representations - helping students see the connections between the world they see around them (macroscopic), the atoms and molecules that compose the world (molecular), and the formulas they write down on paper (symbolic). The hallmarks of Dr. Tro's problem-solving approach are reinforced through interactive media that provide students with an office-hour type of environment built around worked examples and expanded coverage on the latest developments in chemistry. Pioneering features allow students to sketch their ideas through new problems, and much more.
Sample Solutions for this Textbook
We offer sample solutions for Chemistry: A Molecular Approach homework problems. See examples below:
Chapter 1, Problem 1SAQChapter 2, Problem 1SAQChapter 3, Problem 1SAQExplanation: Molar mass of MnO2= 55 + 2 × 16 = 55 + 32 = 87 Number of moles of MnO2= 25.087 = 0.287...Given: Initial pressure, P1 = 547 mmHg Initial volume, V1 = 0.500 L Final volume, V2 = 225 mL =...Explanation: Given info: The amount of the heat produced = 155kJ. The amount of the work done =...Chapter 7, Problem 1SAQChapter 8, Problem 1SAQExplanation: Ionic bond is formed between a positive ion and a negative ion. Positive ion results...
Reason for correct option: Lewis structure of CBr4: CBr4 Has 25 valence electrons. The central atom...The molecules of gases are not rigid. They have large space between them, more as compared to...Justify reasons for the correct statement: Octane is a nonpolar solvent. A compound or solute that...Chapter 13, Problem 1SAQJustify reasons for correct statement: The given reaction is as follows: C(s)+2H2(g)⇌CH4(g) Here,...Justification for the correct option: When an acid donates its hydrogen ion, a conjugate base is...In the given buffer of 0.100 M in NH4Cl and 0.100 M in NH3, NH3 is weak base and NH4Cl is a...The phase transition is from solid to gas during the chemical reaction, so entropy increases and...The equation for this reaction as follows: VO2+(aq)+Sn(s)+H+(aq)→VO2+(aq)+Sn2+(aq)+H2O(l) Separate...The original atom is called parent nuclide, and the product of the decay is called the daughter...Justification for the correct statement: Carbon has a valency of 4. So, carbon can form covalent...The lipids are a diverse group of naturally occurring organic compounds and chemical components of...Justify reasons for the correct statement: The AlO2− units substitute for three-fourths of SiO2;...Justify reason for correct statement: Gold occurs in elemental state with some small particles and...When we write the electron configuration of Cu+ ion using the periodic table, we see that argon is...
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