Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Textbook Question
Chapter 18, Problem 23RQ
Second Law of
Explain how the entropy of the surroundings of a reaction is related to the enthalpy of the reaction.
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Chapter 18 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 18 - Molecules of an ideal gas have no intermolecular...Ch. 18 - If a gas is compressed under adiabatic conditions...Ch. 18 - Calculate the difference, in kilojoules, between...Ch. 18 - The reaction CaO(s)+2HCl(g)CaCl2(s)+H2O(g) has...Ch. 18 - Are the following processes spontaneous? (a) Ice...Ch. 18 - The following processes are nor spontaneous as...Ch. 18 - Would you expect the to be positive or negative...Ch. 18 - Predict the sign of the entropy change for (a) the...Ch. 18 - Predict the sing of S for the following reactions:...Ch. 18 - Would you expect the following reactions to be...
Ch. 18 - What change in temperature would make the process...Ch. 18 - Calculate SfforNH3(g). (Hint: Write the equation...Ch. 18 - Calculate the standard entropy change, S,inJK-1...Ch. 18 - Prob. 14PECh. 18 - Use the data in Table 6.2 and Table 18.1 to...Ch. 18 - Calculate for the reaction of iron(III) oxide...Ch. 18 - Calculate Greaction in kilojoules for the...Ch. 18 - Calculate the maximum work that could be obtained...Ch. 18 - Calculate the maximum work that could be obtained...Ch. 18 - The heat of vaporization of ammonia is and the...Ch. 18 - The heat of vaporization of mercury is 60.7...Ch. 18 - Use the data in Table 18.2 to determine whether...Ch. 18 - Use the data in Table 18.2 to determine whether we...Ch. 18 - In Examples 18.3 and 18.4 we computed SandH for...Ch. 18 - Use the data in Table 18.2 to determine for the...Ch. 18 - Calculate for the reaction described in the...Ch. 18 - In which direction will the reaction described in...Ch. 18 - The reaction...Ch. 18 - The reaction...Ch. 18 - Determine the heat of formation of gaseous...Ch. 18 - Determine the heat of formation of gaseous...Ch. 18 - First Law of Thermodynamics
18.1 What is the...Ch. 18 - First Law of Thermodynamics
18.2 State the first...Ch. 18 - First Law of Thermodynamics
18.3 How is a change...Ch. 18 - First Law of Thermodynamics
18.4 What is the...Ch. 18 - First Law of Thermodynamics Which quantities in...Ch. 18 - First Law of Thermodynamics Which thermodynamic...Ch. 18 - Second Law of Thermodynamics
18.7 What are the...Ch. 18 - First Law of Thermodynamics If there is a decrease...Ch. 18 - First Law of Thermodynamics Which of the following...Ch. 18 - Spontaneous Change What is a spontaneous change?...Ch. 18 - Spontaneous Change List five changes that you have...Ch. 18 - Spontaneous Change
18.12 Which of the items that...Ch. 18 - Spontaneous Change At constant pressure, what role...Ch. 18 - Spontaneous Change How do the probabilities of the...Ch. 18 - Entropy An instant cold pack purchased in a...Ch. 18 - Entropy What is entropy?Ch. 18 - Entropy How is the entropy of a substance affected...Ch. 18 - Entropy
18.18 Will the entropy change for each of...Ch. 18 - Entropy On the basis of our definition of entropy,...Ch. 18 - Second Law of Thermodynamics State the second law...Ch. 18 - Second Law of Thermodynamics How can a process...Ch. 18 - Second Law of Thermodynamics Explain the terms...Ch. 18 - Second Law of Thermodynamics Explain how the...Ch. 18 - Second Law of Thermodynamics
18.24 What is the...Ch. 18 - Second Law of Thermodynamics Define Gibbs free...Ch. 18 - Second Law of Thermodynamics
18.26 In terms of the...Ch. 18 - Second Law of Thermodynamics Under what...Ch. 18 - Third Law of Thermodynamics State the third law of...Ch. 18 - Third Law of Thermodynamics Explain why the units...Ch. 18 - Third Law of Thermodynamics Explain why the values...Ch. 18 - Third Law of Thermodynamics Would you expect the...Ch. 18 - Third Law of Thermodynamics Why does entropy...Ch. 18 - Third Law of Thermodynamics Does glass have S = 0...Ch. 18 - Standard Free Energy Change, G What is the...Ch. 18 - Standard Free Energy Change, G Why can G be...Ch. 18 - Maximum Work and G How is free energy related to...Ch. 18 - Maximum Work and
18.37 What is a...Ch. 18 - Maximum Work and G How is the rate at which energy...Ch. 18 - Maximum Work and
18.39 When glucose is oxidized...Ch. 18 - Maximum Work and G Why are real, observable...Ch. 18 - Free Energy and Equilibrium
18.41 In what way is...Ch. 18 - Free Energy and Equilibrium How can boiling points...Ch. 18 - Free Energy and Equilibrium Considering the fact...Ch. 18 - Free Energy and Equilibrium When a warm object is...Ch. 18 - Free Energy and Equilibrium Sketch the shape of...Ch. 18 - Free Energy and Equilibrium Many reactions that...Ch. 18 - Equilibrium Constants and
18.47 Suppose a...Ch. 18 - Equilibrium Constants and G Write the equation...Ch. 18 - Equilibrium Constants and G How is the equilibrium...Ch. 18 - Equilibrium Constants and
18.50 What is the value...Ch. 18 - Equilibrium Constants and
18.51 How does the...Ch. 18 - Bond Energies Define the term atomization enerey.Ch. 18 - Bond Energies Why are the heats of formation of...Ch. 18 - Bond Energies The gaseous C2 molecule has a bond...Ch. 18 - First Law of Thermodynamics
18.55 A certain system...Ch. 18 - First Law of Thermodynamics The value of E for a...Ch. 18 - 18.57 Suppose that you were pumping an automobile...Ch. 18 - 18.58 Consider the reaction between aqueous...Ch. 18 - Calculate H and E for the following reactions at...Ch. 18 - Calculate H and E for the following reactions at...Ch. 18 - The reaction 2N2O(g)2N2(g)+O2(g) has H=-163.14kJ....Ch. 18 - 18.62 A 10.0 L vessel at contains butane, , at a...Ch. 18 - Spontaneous Change Predict the sign of S for the...Ch. 18 - Spontaneous Change
18.64 Predict the sign of for...Ch. 18 - 18.65 Use the data from Table 6.2 to calculate ...Ch. 18 - Use the data from Table 6.2 to calculate H for the...Ch. 18 - Entropy There are two chemical systems, A and B,...Ch. 18 - Entropy
18.68 A chemical system has three panicles...Ch. 18 - Which system has a higher entropy? Explain your...Ch. 18 - Which system has a higher entropy?Ch. 18 - What factors must you consider to determine the...Ch. 18 - 18.72 What factors must you consider to determine...Ch. 18 - 18.73 Predict the algebraic sign of the entropy...Ch. 18 - 18.74 Predict the algebraic sign of the entropy...Ch. 18 - Second Law of Thermodynamics Under what conditions...Ch. 18 - Second Law of Thermodynamics
18.76 Under what...Ch. 18 - Third Law of Thermodynamics Calculate S for the...Ch. 18 - Third Law of Thermodynamics
18.78 Calculate for...Ch. 18 - Calculate Sfo for these compounds in J mol-1K-1....Ch. 18 - Calculate Sfo for these compounds in J mol-1K-1....Ch. 18 - Nitrogen dioxide, NO2, an air pollutant, dissolves...Ch. 18 - Good wine will turn to vinegar if it is left...Ch. 18 - Standard Free Energy Change, G Phosgene, COCl2,...Ch. 18 - Standard Free Energy Change, G Aluminum oxidizes...Ch. 18 - 18.85 Compute in kJ for the following reactions,...Ch. 18 - Prob. 86RQCh. 18 - Given the following,...Ch. 18 - *18.88 Given the following reactions and their ...Ch. 18 - Maximum Work and G Gasohol is a mixture of...Ch. 18 - Maximum Work and
18.90 What is the maximum amount...Ch. 18 - Free Energy and Equilibrium
18.91 Chloroform,...Ch. 18 - For the melting of aluminum,...Ch. 18 - Isooctane, a minor constituent of gasoline, has a...Ch. 18 - Acetone (nail polish remover) has a boiling point...Ch. 18 - 18.95 Determine whether the following reaction...Ch. 18 - Which of the following reactions (equations...Ch. 18 - Equilibrium Constants and G Calculate the value of...Ch. 18 - Equilibrium Constants and
18.98 Calculate the...Ch. 18 - 18.99 The reaction . A 1.00 L reaction vessel at ...Ch. 18 - The reaction...Ch. 18 - A reaction that can convert coal to methane (the...Ch. 18 - 18.102 One of the important reactions in living...Ch. 18 - What is the value of the equilibrium constant for...Ch. 18 - Methanol, a potential replacement for gasoline as...Ch. 18 - Bond Energies
18.105 Use the data in Table 18.4 to...Ch. 18 - 18.106 Approximately how much energy would be...Ch. 18 - 18.107 The standard heat of formation of ethanol...Ch. 18 - The standard heat of formation of ethylene,...Ch. 18 - Carbon disulfide, CS2, has the Lewis structure ,...Ch. 18 - Gaseous hydrogen sulfide, H2S,hasHf=20.15kJmol-1....Ch. 18 - 18.111 For . Use the data in Table 18.3 to...Ch. 18 - 18.112 Use the results of the preceding problem...Ch. 18 - Use the data in Tables 18.3 and 18.4 to estimate...Ch. 18 - What would be the approximate heat of formation of...Ch. 18 - *18.115 Which substance should have the more...Ch. 18 - Would you expect the value of Hf for benzene,...Ch. 18 - 18.117 Look at Table C.2 in Appendix C. Some of...Ch. 18 - Calculate the G for the dissolution of calcium...Ch. 18 - 18.119 If pressure is expressed in atmospheres and...Ch. 18 - 18.120 Calculate the work, in joules, done by a...Ch. 18 - When an ideal gas expands at a constant...Ch. 18 - When a real gas expands at a constant temperature,...Ch. 18 - 18.123 An ideal gas in a cylinder fitted with a...Ch. 18 - A cylinder fitted with a piston contains 5.00 L of...Ch. 18 - The experiment described in Exercise 18.124 is...Ch. 18 - When potassium iodide dissolves in water, the...Ch. 18 - The enthalpy of combustion Hcombustiono, of oxalic...Ch. 18 - Many biochemical reactions have positive values...Ch. 18 - *18.129 The reaction
has . Determine the value of...Ch. 18 - At 1500C,Kc=5.67 for the reaction...Ch. 18 - 18.131 Given the following reactions and their...Ch. 18 - *18.132 At room temperature , the gas ClNO is...Ch. 18 - *18.133 The reaction
has are placed in a 2.00 L...Ch. 18 - Use the data in Table 18.3 to calculate the bond...Ch. 18 - 18.135 The heat of vaporization of carbon...Ch. 18 - At 25C, 0.0560molO2and0.020molN2O were placed in a...Ch. 18 - For the substance SO2F2(g),Hfo=-858kJmol-1. The...Ch. 18 - *18.138 Ethyl alcohol, , has been suggested as an...Ch. 18 - When solutions of sodium hydroxide are used to...Ch. 18 - Prob. 140RQCh. 18 - A certain weak acid has a pKa of 5.83. When 100.0...Ch. 18 - The average CH bond energy calculated using the...Ch. 18 - 18.144 If a catalyst were able to affect the...Ch. 18 - At the beginning of this chapter we noted that the...
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- Define the term entropy, and give an example of a sample of matter that has zero entropy. What are the units of entropy? How do they differ from the units of enthalpy?arrow_forwardA pot of cold water is heated on a stove, and when the water boils, a fresh egg is placed in the water to cook. Describe the events that are occurring in terms of the zeroth law of thermodynamics.arrow_forwardCoal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.arrow_forward
- What are the two ways that a final chemical state of a system can be more probable than its initial state?arrow_forwardThe statement Energycan beneithercreatednor destroyedis sometimes used as an equivalent statement of the first law of thermodynamics. There areinaccuracies to the statement, however. Restate it tomake it less inaccurate.arrow_forwardExplain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.arrow_forward
- When 1.000 g of gaseous butane, C4H10, is burned at 25C and 1.00 atm pressure, H2O(l) and CO2(g) are formed with the evolution of 49.50 kJ of heat. a Calculate the molar enthalpy of formation of butane. (Use enthalpy of formation data for H2O and CO2.) b Gf of butane is 17.2 kJ/mol. What is G for the combustion of 1 mol butane? c From a and b, calculate S for the combustion of 1 mol butane.arrow_forwardFor each process, tell whether the entropy change of the system is positive or negative. (a) A glassblower heats glass (the system) to its softening temperature. (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)arrow_forwardUse data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?arrow_forward
- 9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the combustion of acetaldehyde? CH3CHO(l)+52O2(g)2CO2+2H2O(l)arrow_forwardThe formation of aluminum oxide from its elements is highly exothermic. If 2.70 g Al metal is burned in pure O2 to give A12O3, calculate how much thermal energy is evolved in the process (at constant pressure).arrow_forward
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