Physical Chemistry 2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Ball, David W. (david Warren), BAER, Tomas
1 Gases And The Zeroth Law Of Thermodynamics 2 The First Law Of Thermodynamics 3 The Second And Third Laws Of Thermodynamics 4 Gibbs Energy And Chemical Potential 5 Introduction To Chemical Equilibrium 6 Equilibria In Single-component Systems 7 Equilibria In Multiple-component Systems 8 Electrochemistry And Ionic Solutions 9 Pre-quantum Mechanics 10 Introduction To Quantum Mechanics 11 Quantum Mechanics: Model Systems And The Hydrogen Atom 12 Atoms And Molecules 13 Introduction To Symmetry In Quantum Mechanics 14 Rotational And Vibrational Spectroscopy 15 Introduction To Electronic Spectroscopy And Structure 16 Introduction To Magnetic Spectroscopy 17 Statistical Thermodynamics: Introduction 18 More Statistical Thermodynamics 19 The Kinetic Theory Of Gases 20 Kinetics 21 The Solid State: Crystals 22 Surfaces Chapter2: The First Law Of Thermodynamics
Chapter Questions Section: Chapter Questions
Problem 2.1E: Calculatethe work performed by a person whoexertsa force of 30 NN = newtonstomove abox 30metersif... Problem 2.2E: Explain inyour own words why work done by the system is defined as the negative of pV, not positive... Problem 2.3E: Calculate the work in joules when a piston moves from a volume of 50.00 mL to a volume of 450.00 mL... Problem 2.4E: Calculatethe work on the system whena piston is compressed by a pressure of 1780torr from 3.55 L... Problem 2.5E: Calculatethe work in joules needed to expanda balloon from5mL to 3.350 L against standard... Problem 2.6E: Consider exercise 2.5. Would the workbe more or less if it were performedagainstdifferent external... Problem 2.7E: Apistonhaving0.033 mol ofgas at 35.0Cexpands from0.77 Lto 2.00L.Calculate the work performed if... Problem 2.8E: A bottle of soda has a head space containing 25.0 mL of CO2 gas at 4.2 atm pressure when the soda is... Problem 2.9E Problem 2.10E: Calculate the specific heat of a material if 288J of energy were required to heat 50.5g of the... Problem 2.11E: There is 3930 J of energy added to a 79.8-g sample of H2 gas. By how much doesthe temperature... Problem 2.12E: If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A... Problem 2.13E: Liquid hydrogen fluoride, liquid water,and liquid ammonia all have relatively high specific heats... Problem 2.14E: A 5-mmdiameter hailstone has a terminal velocity of10.0m/s. Assuming its mass is6.031025 kg and all... Problem 2.15E: A7.50-gpiece of iron at 100.0C is dropped into 25.0g of water at 22.0C. Assuming that the heat lost... Problem 2.16E: With reference to Joules apparatus inFigure2.6, assuminga massof 100.Kg ofwater about100L,a weight... Problem 2.17E Problem 2.18E: True or false: Althoughwork done bya free expansion is zero for an ideal gas, it is nonzero for a... Problem 2.19E: What arethe differencesbetween an open, a closed, and an isolated system?Describe an example of... Problem 2.20E: The statement Energycan beneithercreatednor destroyedis sometimes used as an equivalent statement of... Problem 2.21E Problem 2.22E: What is the change in internal energy when a gas contracts from 377mL to 119mLundera pressure of... Problem 2.23E: Calculate the work for the isothermal, reversible compressionof 0.245 moleof an idealgas going from... Problem 2.24E: Calculate the work donewhen 1.000 mole of an ideal gas expands reversiblyfrom 1.0L to 10L at 298.0K.... Problem 2.25E: Apistonhaving0.033 mol of gas at 35.0C expands from 0.77L to 2.00 L and the systemsimultaneously... Problem 2.26E Problem 2.27E: Indicate which state function is equal to heat, q, for each process described. a. The ignition of a... Problem 2.28E: The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving... Problem 2.29E: Is temperature astate function?Defend your answer. Problem 2.30E: A piston reversibly and adiabatically contracts 3.88 moles of ideal gas to one-tenth of its original... Problem 2.31E: Calculate U when 1.00 mol of H2 goes from 1.00 atm, 10.0 L, and 295 K to 0.793 atm, 15.0 L, and 350... Problem 2.32E: Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special... Problem 2.33E: Under what conditions will U be exactly zero for a process whose initial conditions are not thesame... Problem 2.34E: Aballoon filled with 0.505 mole of gascontracts reversibly from 1.0L to 0.10 L ata constant... Problem 2.35E: A piston having 7.23 g of steam at 110 C increases its temperature by 35 C. At the same time, it... Problem 2.36E: It takes 2260 J to vaporize a gram of liquid water to steam at its normal boiling point of 100C.... Problem 2.37E: True or false: Any process for which H is negative is exothermic. Explain your answer. Problem 2.38E Problem 2.39E: A refrigerator contains approximately 17cubic feet, or about 480 liters, of air. Assuming it acts as... Problem 2.40E: In a constant-volume calorimeter, 35.0g of H2cools from 75.3C to25.0C. Calculate w, q, U, and H for... Problem 2.41E: A 2.50-mol sample of gas is compressed isothermally from 20.0 L to 5.00 L under a constant external... Problem 2.42E: A 244-g amount of coffee in an open plastic cup cools from 80.0C to 20.0C. Assuming no loss of mass... Problem 2.43E Problem 2.44E: Starting with equation 2.27 andthe original definitionof enthalpy, derive the fact that Cp-=Cv-+R Problem 2.45E: Derive the fact that HpT is also zero for an ideal gas. Problem 2.46E: Define isobaric,isochoric, isenthalpic,and isothermal. Can achangein a gaseous system be isobaric,... Problem 2.47E: Starting from the cyclicrule involvingthe Joule- Thomson coefficient, derive equation 2.35 Problem 2.48E: The ideal gas law is theequation of state for an ideal gas. Why cantit be used to determine TpH? Problem 2.49E Problem 2.50E: Estimatethe final temperature of a mole of gas at 200.00 atmand 19.0C as it is forced through a... Problem 2.51E: With regard to exercise 2.50, how accurate do you think your answer is, and why? Problem 2.52E: Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions... Problem 2.53E: Use the data in Table 2.2 to determine PH T for N2 at 50C and 20atm. Make any reasonable assumptions... Problem 2.54E: Someone proposes thatthe Joule-Thomson coefficient can also be defined as UJT = UPTcv Is this... Problem 2.55E: Why is equation2.37 written interms of CV and Cp and not c-v and c-p ? Problem 2.56E: What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units... Problem 2.57E: In a constant-pressure calorimeter that is, one that expands or contracts if the volume of the... Problem 2.58E: What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work... Problem 2.59E Problem 2.60E: Show that =5/3 for a monatomic ideal gas. Problem 2.61E Problem 2.62E Problem 2.63E: A 1.00 mol sample of H2 is carefully warmed from 22 K to 40 K at constant volume. a What is the... Problem 2.64E: Asampleof a monatomic ideal gas doubles itsvolume reversibly and adiabatically. By what percentage... Problem 2.65E: A sample of an ideal diatomic gas is compressed adiabatically and reversibly to double its initial... Problem 2.66E: In orbit about Earth, a weather balloonjettisons a weight andascends to a higher altitude. If the... Problem 2.67E Problem 2.68E Problem 2.69E: If pumping up an automobile tire is assumed to be adiabatic and reversible, what is the new... Problem 2.70E Problem 2.71E: Take the volume change into account and calculate H and U for exactly 1 g of ice melting into 1 g of... Problem 2.72E: How much work is performed by 1 mole of water freezing to 1 mole of ice at 0C at standard pressure?... Problem 2.73E: Why are steam burns so much worse than water burns even if the H2O is at the same temperature for... Problem 2.74E: How many grams of water at 0C will be melted by the condensation of 1 g of steam at 100C? Problem 2.75E: Draw a diagram like Figure 2.11 that illustrates the change in enthalpy for the chemical reaction C... Problem 2.76E: Determine the rxnH(25C) of the following reaction: H2(g)+I2(s)2HI(g) Problem 2.77E: Determine rxnH 25 C for the following reaction: NO g O2 g NO2 g This reaction is a major... Problem 2.78E: The enthalpy of combustion of buckminsterfullerene, C60, is -26,367kJ/mol. C60(s)+60O2(g)60CO2(g)... Problem 2.79E: The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C... Problem 2.80E: Using Hesss law, writeout allof the formation reactions that add up to, and calculate rxnH(25C) for,... Problem 2.81E: Sublimation is the phase change from solid to gas without going through a liquid phase. Solid CO2,... Problem 2.82E: The thermite reaction combines aluminum powder and iron oxide and ignites the mixture to make... Problem 2.83E: Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant... Problem 2.84E: Assume that 1.20 g of benzoicacid, C6H5COOH, is burned in a porcelain dish exposed to the air.If 31,... Problem 2.85E: Natural gas is mostly CH4. When it burns, the chemical reaction is CH4 g 2O2 g CO2 g 2H2O g The H... Problem 2.86E: Assuming constant heatcapacities for products and reactants,determine the H(500C) for... Problem 2.87E: Use the heat capacities of the products and reactants of the thermite reaction and the calculated H... Problem 2.88E: The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500... Problem 2.89E Problem 2.90E Problem 2.91E: The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants... Problem 2.92E Problem 2.93E: Find the enthalpies of the combustion reactions for methane through n-octane. Plot them versus the... Problem 2.20E: The statement Energycan beneithercreatednor destroyedis sometimes used as an equivalent statement of...
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I can determine mathematically how much energy will be produced or absorbed for a given chemical reaction …
using Hess’ law for a net reaction from a series of reactions
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Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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would i put in numbers in the boxes ? are you able to give a real example with numbers , as this is a little bit confusing
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