EBK STUDY GUIDE TO ACCOMPANY CHEMISTRY:
7th Edition
ISBN: 9781119360889
Author: HYSLOP
Publisher: VST
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Textbook Question
Chapter 18, Problem 27PE
In which direction will the reaction described in Example 18.10 proceed to reach equilibrium if the partial pressure of
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EBK STUDY GUIDE TO ACCOMPANY CHEMISTRY:
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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- The atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?arrow_forwardAt 1 atm and 25 C, NO2 with an initial concentration of 1.00 M is 3.3103 decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO2(g)2NO(g)+O2(g)arrow_forwardThe equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?arrow_forward
- Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.arrow_forward12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.arrow_forwardDuring an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?arrow_forward
- A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.arrow_forwardGiven these data at a certain temperature, 2H2(g)+O2(g)2H2O(g)Kc=3.21081N2(g)+3H2(g)2NH3(g)Kc=3.5108 calculate Kc for the reaction of ammonia with oxygen to give N2(g) and H2O(g).arrow_forwardKc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?arrow_forward
- The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.arrow_forwardAt 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forwardAt room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?arrow_forward
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