Chemistry & Chemical Reactivity 9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
1 Basic Concepts Of Chemistry 2 Atoms Molecules And Ions 3 Chemical Reactions 4 Stoichiometry: Quantitative Information About Chemical Reactions 5 Principles Of Chemical Reactivity: Energy And Chemical Reactions 6 The Structure Of Atoms 7 The Structure Of Atoms And Periodic Trends 8 Bonding And Molecular Structure 9 Bonding And Molecular Structure: Orbital Hybridization And Molecular Orbitals 10 Gases And Their Properties 11 Intermolecular Forces And Liquids 12 The Solid State 13 Solutions And Their Behavior 14 Chemical Kinetics: The Rates Of Chemical Reactions 15 Principles Of Chemical Reactivity: Equilibria 16 Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases 17 Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria 18 Principles Of Chemical Reactivity: Entropy And Free Energy 19 Principles Of Chemical Reactivity: Electron Transfer Reactions 20 Environmental Chemistry-earth's Environment, Energy, And Sustainability 21 The Chemistry Of The Main Group Elements 22 The Chemistry Of The Transistion Elements 23 Carbon: Not Just Another Element 24 Biochemistry 25 Nuclear Chemistry L Let's Review Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
5.1 Energy: Some Basic Principles 5.2 Specific Heat Capacity: Heating And Cooling 5.3 Energy And Changes Of State 5.4 The First Law Of Thermodynamics 5.5 Enthalpy Changes For Chemical Reactions 5.6 Calorimetry 5.7 Enthalpy Calculations 5.8 Product- Or Reactant-favored Reactions And Thermodynamics Chapter Questions Section: Chapter Questions
Problem 1PS: Define the terms system and surroundings. What does it mean to say that a system and its... Problem 2PS: What determines the directionality of energy transfer as heat? Problem 3PS: Identify whether the following processes are exothermic or endothermic. Is the sign on qsys positive... Problem 4PS: Identify whether the following processes are exothermic or endothermic. Is the sign on qsys positive... Problem 5PS: The molar heat capacity of mercury is 28.1 J/mol K What is the specific heat capacity of this metal... Problem 6PS: The specific heat capacity of benzene (C6H6) is 1.74 J/g K. What is its molar heat capacity (in... Problem 7PS: The specific heat capacity of copper metal is 0.385 J/g K. How much energy is required to heat 168... Problem 8PS: How much energy as heat is required to raise the temperature of 50.00 mL of water from 25.52 C to... Problem 9PS: The initial temperature of a 344-g sample of iron is 18.2 C. If the sample absorbs 2.25 kJ of energy... Problem 10PS: After absorbing 1.850 kJ of energy as heat, the temperature of a 0.500-kg block of copper is 37 C.... Problem 11PS: A 45.5-g sample of copper at 99.8 C is dropped into a beaker containing 152 g of water at 18.5 C.... Problem 12PS: One beaker contains 156 g of water at 22 C, and a second beaker contains 85.2 g of water at 95 C.... Problem 13PS: A 182-g sample of gold at some temperature was added to 22.1 g of water. The initial water... Problem 14PS: When 108 g of water at a temperature of 22.5 C is mixed with 65.1 g of water at an unknown... Problem 15PS: A 13.8-g piece of zinc is heated to 98.8 C in boiling water and then dropped into a beaker... Problem 16PS: A 237-g piece of molybdenum, initially at 100.0 C, is dropped into 244 g of water at 10.0 C. When... Problem 17PS: How much energy is evolved as heat when 1.0 L of water at 0 C solidifies to ice? (The heat of fusion... Problem 18PS: The energy required to melt 1.00 g of ice at 0 C is 333 J. If one ice cube has a mass of 62.0 g and... Problem 19PS: How much energy is required to vaporize 125 g of benzene, C6H6, at its boiling point, 80.1 C? (The... Problem 20PS: Chloromethane, CH3CI, arises from microbial fermentation and is found throughout the environment. It... Problem 21PS: The freezing point of mercury is 38.8 C. What quantity of energy, in joules, is released to the... Problem 22PS: What quantity of energy, in joules, is required to raise the temperature of 454 g of tin from room... Problem 23PS: Ethanol, C2HsOH, boils at 78.29 C. How much energy, in joules, is required to raise the temperature... Problem 24PS: A 25.0-mL sample of benzene at 19.9 C was cooled to its melting point, 5.5 C, and then frozen How... Problem 25PS: As a gas cools, it is compressed from 2.50 L to 1.25 L under a constant pressure of 1.01 105 Pa.... Problem 26PS: A balloon expands from 0.75 L to 1.20 L as it is heated under a constant pressure of 1.01 105 Pa.... Problem 27PS: A balloon does 324 J of work on the surroundings as it expands under a constant pressure of 7.33 ... Problem 28PS: As the gas trapped in a cylinder with a movable piston cools, 1.34 kJ of work is done on the gas by... Problem 29PS: When 745 J of energy in the form of heat is transferred from the environment to a gas, the expansion... Problem 30PS: The internal energy of a gas decreases by 1.65 kJ when it transfers 1.87 kJ of energy in the form of... Problem 31PS: A volume of 1.50 L of argon gas is confined in a cylinder with a movable piston under a constant... Problem 32PS: Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 104... Problem 33PS: Nitrogen monoxide, a gas recently found to be involved in a wide range of biological processes,... Problem 34PS: Calcium carbide, CaC2, is manufactured by the reaction of CaO with carbon at a high temperature.... Problem 35PS: Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air... Problem 36PS: Acetic acid. CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide. CH3OH ()... Problem 37PS: You mix 125 mL of 0.250 M CsOH with 50.0 mL of 0.625 M HF in a coffee-cup calorimeter, and the... Problem 38PS: You mix 125 mL of 0.250 M CsOH with 50.0 mL of 0.625 M HF in a coffee-cup calorimeter, and the... Problem 39PS: A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5 C and then... Problem 40PS: A piece of chromium metal with a mass of 24.26 g is heated in boiling water to 98.3 C and then... Problem 41PS: Adding 5.44 g of NH4NO3(s) to 150.0 g of water in a coffee-cup calorimeter (with stirring to... Problem 42PS: You should use care when dissolving H2SO4 in water because the process is highly exothermic. To... Problem 43PS: Sulfur (2.56 g) was burned in a constant-volume calorimeter with excess O2(g). The temperature... Problem 44PS: Suppose you burned 0.300 g of C(s) in an excess of O2(g) in a constant-volume calorimeter to give... Problem 45PS: Suppose you burned 1.500 g of benzoic acid, C6H5CO2H, in a constant-volume calorimeter and found... Problem 46PS: A 0.692-g sample of glucose, C6H12O6, was burned in a constant-volume calorimeter. The temperature... Problem 47PS: An ice calorimeter can be used to determine the specific heat capacity of a metal. A piece of hot... Problem 48PS: A 9.36-g piece of platinum was heated to 98.6 C in a boiling water bath and then dropped onto ice.... Problem 49PS: The enthalpy changes for the following reactions can be measured: CH4(g) + 2 O2(g) CO2(g) + 2... Problem 50PS: The enthalpy changes of the following reactions can be measured: C2H4(g) + 3 O2(g) 2 CO2(g) + 2... Problem 51PS: Enthalpy changes for the following reactions can be determined experimentally: N2(g) + 3 H2(g) 2... Problem 52PS: You wish to know the enthalpy change for the formation of liquid PCl3 from the elements. P4(s) + 6... Problem 53PS: Write a balanced chemical equation for the formation of CH3OH() from the elements in their standard... Problem 54PS: Write a balanced chemical equation for the formation of CaCO3(s) from the elements in their standard... Problem 55PS: (a) Write a balanced chemical equation for the formation of 1 mol of Cr2O3(s) from Cr and O2 in... Problem 56PS: (a) Write a balanced chemical equation for the formation of 1 mol of MgO(s) from the elements in... Problem 57PS: Use standard enthalpies of formation in Appendix L to calculate enthalpy changes for the following:... Problem 58PS: Use standard enthalpies of formation in Appendix L to calculate enthalpy changes for the following:... Problem 59PS: The first step in the production of nitric acid from ammonia involves the oxidation of NH3. 4 NH3(g)... Problem 60PS: The Romans used calcium oxide, CaO, to produce a strong mortar to build stone structures. Calcium... Problem 61PS: The standard enthalpy of formation of solid barium oxide, BaO, is 553.5 kJ/mol, and the standard... Problem 62PS: An important step in the production of sulfuric acid is the oxidation of SO2 to SO3. SO2(g) + O2(g)... Problem 63PS: The enthalpy change for the oxidation of naphthalene, C10Hg, is measured by calorimetry. C10H8(s) +... Problem 64PS: The enthalpy change for the oxidation of styrene. C8H8, is measured by calorimetry. C8H8() + 10... Problem 65GQ Problem 66GQ Problem 67GQ: For each of the following, define a system and its surroundings, and give the direction of energy... Problem 68GQ Problem 69GQ: Use Appendix L to find the standard enthalpies of formation of oxygen atoms, oxygen molecules (O2),... Problem 70GQ: You have a large balloon containing 1.0 mol of gaseous water vapor at 80 C. How will each step... Problem 71GQ: Determine whether energy as heat is evolved or required, and whether work was done on the system or... Problem 72GQ: Determine whether energy as heat is evolved or required, and whether work was done on the system or... Problem 73GQ: Use standard enthalpies of formation to calculate the enthalpy change that occurs when 1.00 g of... Problem 74GQ: Which evolves more energy on cooling from 50 C to 10 C: 50.0 g of water or 100. g of ethanol... Problem 75GQ: You determine that 187 J of energy as heat is required to raise the temperature of 93.45 g of silver... Problem 76GQ: Calculate the quantity of energy required to convert 60.1 g of H2O(s) at 0.0 C to H2O(g) at 100.0 C.... Problem 77GQ: You add 100.0 g of water at 60.0 C to 100.0 g of ice at 0.00 C. Some of the ice melts and cools the... Problem 78GQ: Three 45-g ice cubes at 0 C are dropped into 5.00 102 mL of tea to make iced tea. The tea was... Problem 79GQ: Suppose that only two 45-g ice cubes had been added to your glass containing 5.00 102 mL of tea... Problem 80GQ: You take a diet cola from the refrigerator and pour 240 mL of it into a glass. The temperature of... Problem 81GQ: The standard molar enthalpy of formation of diborane, B2H6(g), cannot be determined directly because... Problem 82GQ: Chloromethane, CH3Cl, a compound found throughout the environment, is formed in the reaction of... Problem 83GQ Problem 84GQ: Camping stoves are fueled by propane (C3H8), butane [C4H10(g), fH = 127.1 kJ/mol]. gasoline. or... Problem 85GQ Problem 86GQ Problem 87GQ: (a) Calculate the enthalpy change, rH, for the formation of 1.00 mol of strontium carbonate (the... Problem 88GQ: You drink 350 mL of diet soda that is at a temperature of 5 C. (a) How much energy will your body... Problem 89GQ: Chloroform, CHCl3, is formed from methane and chlorine in the following reaction. CH4(g) + 3 Cl2(g) ... Problem 90GQ: Water gas, a mixture of carbon monoxide and hydrogen, is produced by treating carbon (in the form of... Problem 91GQ: Using standard enthalpies of formation, verify that 2680 kJ of energy is released in combustion of... Problem 93IL: A piece of lead with a mass of 27.3 g was heated to 98.90 C and then dropped into 15.0 g of water at... Problem 94IL: A 192-g piece of copper is heated to 100.0 C in a boiling water bath and then dropped into a beaker... Problem 95IL: Insoluble AgCl(s) precipitates when solutions of AgNO3(aq) and NaCl(aq) are mixed. AgNO3(aq) +... Problem 96IL: Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2(aq) and NaBr(aq) are mixed. Pb(NO3)2(aq)... Problem 97IL: The value of U for the decomposition of 7.647 g of ammonium nitrate can be measured in a bomb... Problem 98IL: A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The... Problem 99IL: The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase... Problem 100IL: On a cold day, you can warm your hands with a heat pad, a device that uses the oxidation of iron to... Problem 101SCQ: Without doing calculations, decide whether each of the following is exo- or endothermic. (a) the... Problem 102SCQ Problem 103SCQ: You want to determine the value for the enthalpy of formation of CaSO4(s), but the reaction cannot... Problem 104SCQ: Prepare a graph of specific heat capacities for metals versus their atomic weights. Combine the data... Problem 105SCQ Problem 106SCQ: You are attending summer school and living in a very old dormitory. The day is oppressively hot.... Problem 107SCQ Problem 108SCQ Problem 109SCQ Problem 110SCQ: Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take... Problem 111SCQ: Isomers are molecules with the same elemental composition but a different atomic arrangement. Three... Problem 112SCQ Problem 113SCQ Problem 114SCQ: A piece of gold (10.0 g, CAu = 0.129 J/g K) is heated to 100.0 C. A piece of copper (also 10.0 g,... Problem 115SCQ: Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy... Problem 116SCQ: Calculate rH for the reaction 2 C(s) + 3 H2(g) + O2(g) C2H5OH() given the information below. C(s)... Problem 117SCQ: You have the six pieces of metal listed below, plus a beaker of water containing 3.00 102 g of... Problem 119SCQ: Sublimation of 1.0 g of dry ice. CO2(s), forms 0.36 L of CO2(g) (at 78 C and 1.01 105 Pa). The... Problem 120SCQ: In the reaction of two moles of gaseous hydrogen and one mole of gaseous oxygen to form two moles of... Problem 36PS: Acetic acid. CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide. CH3OH ()...
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Concept explainers
Arrange the following amines in order of increasing basicity. For example, an answer of 1234 would indicate that you think 1 is least basic and 4 is most basic
Transcribed Image Text: H3C CH3
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Definition Definition Organic compounds with a nitrogen atom having a lone pair of electrons on it. Amines are derived from ammonia (NH 3 ), wherein hydrogen atoms are substituted by an aryl or alkyl group.
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