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 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....
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Transcribed Image Text: 6. A gas in a piston chamber is kept in a constant-temperature bath at 300 K expands from 25.0 mL to 75.0 mL
against a constant pressure of 2 atm. If there are 0.0100 moles of gas in the chamber, calculate the work done by
the system.
Branch of chemistry that studies how atoms, molecules, and materials interact with each other. Physical chemistry focuses on the behavior of matter, such as solids, liquids, and gases, as they interact with other matter. The study of physical chemistry is crucial to thermodynamics, quantum mechanics, and photochemistry.
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