The oxidation of SO2 is the key step in H2SO4 production:

Problem 1P A change in reaction conditions increases the rate of a certain forward reaction more than that of the reverse reaction. What is the effect on the equilibrium constant and the concentrations of reactants and products at equilibrium?

Problem 2P When a chemical company employs a new reaction to manufacture a product, the chemists consider its rate (kinetics) and yield (equilibrium). How do each of these affect the usefulness of a manufacturing process?

Problem 3P If there is no change in concentrations, why is the equilibrium state considered dynamic?

Problem 8P Explain the difference between a heterogeneous and a homogeneous equilibrium. Give an example of each.

Problem 9P Does Q for the formation of 1 mol of NO from its elements differ from Q for the decomposition of 1 mol of NO to its elements? Explain and give the relationship between the two Q’s.

Problem 6P In a study of the thermal decomposition of lithium peroxide, 2Li2O2(s)? 2Li2O(s) + O2(g) a chemist finds that, as long as some Li2O2 is present at the end of the experiment, the amount of O2 obtained in a given container at a given T is the same. Explain.

Problem 10P Does Q for the formation of 1 mol of NH3 from H2 and N2 differ from Q for the formation of NH3 from H2 and 1 mol of N2? Explain and give the relationship between the two Q’s.

Problem 7P In a study of the formation of HI from its elements, H2(g) + I2(g)?2HI(g) equal amounts of H2 and I2 were placed in a container, which was then sealed and heated. (a) On one set of axes, sketch concentration vs. time curves for H2 and HI, and explain how Q changes as a function of time. ________________ (b) Is the value of Q different if [I2] is plotted instead of [H2]?

Problem 12P Balance each reaction and write its reaction quotient,Qc: (a) C2H6(g)+ O2(g)? CO2(g) + H2O(g) ________________ (b) CH4(g) + F2(g) ? CF4(g) + HF(g) ________________ (c) SO3(g) ? SO2(g) + O2(g)

At a particular temperature, \(K_{\mathrm{c}}=6.5 \times 10^{2}\) for Calculate ????c for each of the following reactions: Equation Transcription: ????c = 6.5102 Text Transcription: ????_c = 6.5 times 10^2

Problem 11P Balance each reaction and write its reaction quotient,Qc: (a) NO(g)+ O2(g) ? N2O3(g) ________________ (b) SF6(g)+ SO3(g) ? SO2F2(g) ________________ (c) SClF5(g) + H 2(g) ? S2F10(g) + HCl(g)

Problem 17P Write Qc for each of the following: (a) Hydrogen chloride gas reacts with oxygen gas to produce chlorine gas and water vapor. ________________ (b) Solid diarsenic trioxide reacts with fluorine gas to produce liquid arsenic pentafluoride and oxygen gas. ________________ (c) Gaseous sulfur tetrafluoride reacts with liquid water to produce gaseous sulfur dioxide and hydrogen fluoride gas. ________________ (d) Solid molybdenum(VI) oxide reacts with gaseous xenon di-fluoride to form liquid molybdenum(VI) fluoride, xenon gas, and oxygen gas.

At a particular temperature, \(K_{\mathrm{c}}=1.6 \times 10^{-2}\) for Calculate ????c for each of the following reactions: Equation Transcription: ????c = 1.610-2 Text Transcription: ????_c = 1.6 times 10^-2

Problem 16P Balance each of the following examples of heterogeneous equilibria and write its reaction quotient,Qc: (a) H2O(l)+ SO3(g) ?H2SO4(aq) ________________ (b) KNO3(s) ? KNO2(s)+ O2(g) ________________ (c) S8(s) + F2(g) ? SF6(g)

Problem 15P Balance each of the following examples of heterogeneous equilibria and write its reaction quotient,Qc: (a) Na2O2(s) + CO2(g) ? Na2CO3(s) + O2(g) ________________ (b) H2O(l) ? H2O(g) ________________ (c) NH4Cl(s) ? NH3(g)+ HCl(g)

Problem 20P When are Kc and Kp equal, and when are they not?

Problem 19P Guldberg and Waage proposed the definition of the equilibrium constant as a certain ratio of concentrations. What relationship allows us to use a particular ratio of partial pressures (for a gaseous reaction) to express an equilibrium constant? Explain.

Problem 21P A certain reaction at equilibrium has more moles of gaseous products than of gaseous reactants. (a) Is Kc larger or smaller than Kp? ________________ (b) Write a statement about the relative sizes of Kc and Kp for any gaseous equilibrium.

Problem 18P The interhalogen ClF3 is prepared in a two-step fluorination of chlorine gas: Cl2(g) + F2(g) ? ClF(g) ClF(g) + F2(g) ? C1F3(g) (a) Balance each step and write the overall equation. ________________ (b) Show that the overall Qc equals the product of the Qc’s for the individual steps.

Problem 24P Calculate Kc for each of the following equilibria: (a) CO(g) + Cl2(g) ? COCl2(g); Kp = 3.9 × 10?2 at 1000. K ________________ (b) S2(g) + C(s) ? CS2(g); Kp = 28.5 at 500. K

Problem 23P Determine ?ngas for each of the following reactions: (a) MgCO3(s) ? MgO(s) + CO2(g) ________________ (b) 2H2(g) + O2(g) ? 2H2O(l) ________________ (c) HNO3(l)+ ClF(g) ? ClONO2(g) + HF(g)

Problem 22P Determine ?ngas for each of the following reactions: (a) 2KClO3(s) ? 2KCl(s) + 3O2(g) ________________ (b) 2PbO(s) + O2(g) ? 2PbO2(s) ________________ (c) I2(s) + 3XeF2(s) ? 2IF3(s) + 3Xe(g)

Problem 26P When the numerical value of Q is less than K, in which direction does the reaction proceed to reach equilibrium? Explain.

Problem 25P Calculate Kc for each of the following equilibria: (a) H2(g) + I2(g) ? 2HI(g);Kp= 49 at 730. K ________________ (b) 2SO2(g) + O2(g) ? 2SO3(g);Kp=2.5×1010 at 500. K

The following molecular scenes depict the aqueous reaction \(2 \mathrm{D} \rightleftharpoons \mathrm{E}\), with \(\mathrm{D}\) red and \(\mathrm{E}\) blue. Each sphere represents \(0.0100 \mathrm{~mol}\), but the volume in scene \(A\) is \(1.00 \mathrm{~L}\), whereas in scenes \(B\) and \(\mathrm{C}\), it is \(0.500 \mathrm{~L}\). (a) If the reaction in scene \(\mathrm{A}\) is at equilibrium, calculate \(K_{\mathrm{c}}\). (b) Are the reactions in scenes \(B\) and \(C\) at equilibrium? Which, if either, is not, and in which direction will it proceed?

For a problem involving the catalyzed reaction of methane and steam, the following reaction table was prepared: Explain the entries in the “\(Change\)” and “\(Equilibrium\)” rows. Equation Transcription: Text Transcription: Change Equilibrium

Problem 32P (a) What is the basis of the approximation that avoids using the quadratic formula to find an equilibrium concentration? ________________ (b) When should this approximation not be made?

Problem 29P At 100°C, Kp = 60.6 for the reaction 2NOBr(g) ? 2NO(g) + Br2(g) In a given experiment, 0.10 atm of each component is placed in a container. Is the system at equilibrium? If not, in which direction will the reaction proceed?

Problem 33P In an experiment to study the formation of HI(g), H2(g) + I2(g) ? 2HI(g) H2(g) and I2(g) were placed in a sealed container at a certain temperature. At equilibrium, [H2] = 6.50×10?5M, [I2]=1.06× 10?3 M, and [HI] = 1.87× 10?3M. Calculate Kc for the reaction at this temperature.

Problem 28P At 425°C,Kp = 4.18× 10?9 for the reaction 2HBr(g) ? H2(g) + Br2(g) In one experiment, 0.20 atm of HBr(g), 0.010 atm of H2(g) and 0.010 atm of Br2(g) are introduced into a container. Is the reaction at equilibrium? If not, in which direction will it proceed?

Problem 30P The water-gas shift reaction plays a central role in the chemical methods for obtaining cleaner fuels from coal: CO(g) + H2O(g) ? CO2(g) + H2(g) At a given temperature,Kp= 2.7. If 0.13 mol of CO, 0.56 mol of H2O, 0.62 mol of CO2, and 0.43 mol of H2 are put in a 2.0-L flask, in which direction does the reaction proceed ?

Problem 36P Hydrogen fluoride, HF, can be made from the reaction H2(g) + F2(g) ? 2HF(g) In one experiment, 0.10 mol of H2(g) and 0.050 mol of F2(g) are added to a 0.50-L flask. Write a reaction table for this process.

Problem 35P Gaseous PCl5 decomposes according to the reaction PCl5(g) ? PCl3(g) + Cl2(g) In one experiment, 0.15 mol of PCl5(g) was introduced into a 2.0-L container. Construct the reaction table for this process.

Problem 34P Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2NH3(g) ? N2(g) + 3H2(g) At equilibrium, [NH3] = 0.0225M, [N2] = 0.114M, and [H2] = 0.342 M. Calculate Kc for the reaction at this temperature.

Problem 38P For the following reaction, Kp = 0.262 at 1000°C: C(s) + 2H2(g) ? CH4(g) At equilibrium, PH2 is 1.22 atm. What is the equilibrium partial pressure of CH4(g)?

Problem 37P For the following reaction,Kp= 6.5×104 at 308 K: 2NO(g) + Cl2(g) ? 2NOCl(g) At equilibrium, PNO = 0.35 atm and PCl2 = 0.10 atm. What is the equilibrium partial pressure of NOCl(g)?

Problem 39P Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp= 0.11 at 250°C: NH4HS(s) ? H2S(g) + NH3(g) If 55.0 g of NH4HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium?

Problem 40P Hydrogen sulfide decomposes according to the following reaction, for which Kc= 9.30× 10?8 at 700°C: 2H2S(g) ? 2H2(g) + S2(g) If 0.45 mol of H2S is placed in a 3.0-L container, what is the equilibrium concentration of H2(g) at 700°C?

Problem 41P Even at high T, the formation of NO is not favored: N2(g) + O2(g) ?2NO(g) Kc= 4.10 × l0?4 at 2000°C What is [NO] when a mixture of 0.20 mol of N2(g) and 0.15 mol of O2(g) reach equilibrium in a 1.0-L container at 2000°C?

Problem 43P In an analysis of interhalogen reactivity, 0.500 mol of ICl was placed in a 5.00-L flask, where it decomposed at a high T: 2ICl(g) ? I2(g) + Cl2(g). Calculate the equilibrium concentrations of I2, Cl2, and ICl (Kc= 0.110 at this temperature).

Problem 44P A toxicologist studying mustard gas, S(CH2CH2Cl)2, a blistering agent, prepares a mixture of 0.675 M SC12 and 0.973M C2H4 and allows it to react at room temperature (20.0°C): SCl2 (g) + 2C2H4( g) ? S (CH2CH2Cl) 2 (g) At equilibrium, [S(CH2CH2C1) 2] = 0.350M. Calculate Kp.

Problem 46P A key step in the extraction of iron from its ore is FeO(s) + CO(g) ? Fe(s) + CO2(g)Kp= 0.403 at 1000°C This step occurs in the 700°C to 1200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 1.00 atm of CO(g) and excess FeO(s) react in a sealed container at 1000°C?

Problem 47P What is the difference between the equilibrium position and the equilibrium constant of a reaction? Which changes as a result of a change in reactant concentration?

Problem 45P The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates: 4NH3(g) + 3O2(g) ? 2N2(g) + 6H2O(g) When 0.0150 mol of NH3(g) and 0.0150 mol of O2(g) are placed in a 1.00-L container at a certain temperature, the N2 concentration at equilibrium is 1.96 × 10-3M. Calculate Kc.

Problem 49P What is implied by the word “constant” in the term equilibrium constant? Give two reaction parameters that can be changed without changing the value of an equilibrium constant.

Scenes \(A, B\), and \(C\) depict this reaction at three temperatures: (a) Which best represents the reaction mixture at the highest temperature? Explain. (b) Which best represents the reaction mixture at the lowest temperature? Explain. Equation Transcription: Text Transcription: A,B C

Problem 53P Consider this equilibrium system: CO(g) + Fe3O4(s) ? CO2(g) + 3FeO(s) How does the equilibrium position shift as a result of each of the following disturbances? (a) CO is added, (b) CO2 is removed by adding solid NaOH. (c) Additional Fe3O4(s) is added to the system. (d) Dry ice is added at constant temperature.

Problem 54P Sodium bicarbonate undergoes thermal decomposition according to the reaction 2NaHCO3(s) ? Na2CO3(s) + CO2(g) + H2O(g) How does the equilibrium position shift as a result of each of the following disturbances? (a) 0.20 atm of argon gas is added. (b) NaHCO3(s) is added, (c) Mg(CIO4)2(s) is added as a drying agent to remove H2O. (d) Dry ice is added at constant T.

Problem 55P Predict the effect of increasing the container volume on the amounts of each reactant and product in the following reactions: (a) F2(g) ? 2F(g) ________________ (b) 2CH4(g) ? C2H2(g) + 3H2(g)

An equilibrium mixture of two solids and a gas, in the reaction \(\mathrm{XY}(s) \rightleftharpoons \mathrm{X}(g)+\mathrm{Y}(s)\), is depicted at right (X is green and Y is black). Does scene A, B, or C best represent the system at equilibrium after two formula units of Y(s) is added? Explain. Equation Transcription: <math xmlns="http://www.w3.org/1998/Math/MathML"><mi>XY</mi><mfenced><mi>s</mi></mfenced><mo>&#x21CC;</mo><mi mathvariant="normal">X</mi><mfenced><mi>g</mi></mfenced><mo>+</mo><mi mathvariant="normal">Y</mi><mfenced><mi>s</mi></mfenced></math> Text Transcription: XY(s) rightleft Harpoon X(g)+Y(s)

Problem 57P How would you adjust the volume of the container in order to maximize product yield in each of the following reactions? (a) Fe3O4(s) + 4H2(g) ? 3Fe(s) + 4H2O(g) ________________ (b) 2C(s)+ O2(g) ? 2CO(g)

Problem 42P Nitrogen dioxide decomposes according to the reaction 2NO2(g) ? 2NO(g) + O2(g) where Kp = 4.48 × 10-13 at a certain temperature. If 0.75 atm of NO2 is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO(g) and O2(g)?

Problem 56P Predict the effect of decreasing the container volume on the amounts of each reactant and product in the following reactions: (a) C3H8(g)+ 5O2(g) ? 3CO2(g) + 4H2O(l) ________________ (b) 4NH3(g) + 3O2(g) ? 2N2(g) + 6H2O(g)

Problem 58P How would you adjust the volume of the container in order to maximize product yield in each of the following reactions? (a)Na2O2(s) ? 2Na(l) + O2(g) ________________ (b) C2H2(g) + 2H2(g) ? C2H6(g)

The oxidation of \(\mathrm{SO}_{2}\) is the key step in H2SO4 production: a) What qualitative combination of ???? and ???? maximizes \(\mathrm{SO}_{3}\) yield? (b) How does addition of \(\mathrm{O}_{2}\) affect ????? ????? (c) Why is catalysis used for this reaction? Equation Transcription: SO2 H2SO4 SO3 O2 Text Transcription: SO_2 H_2SO_4 SO_3 O_2

Problem 64P A study of the water-gas shift reaction (see Problem 17.37) was made in which equilibrium was reached with [CO] = [H2O] = [H2] =0.10 M and [CO2] = 0.40 M. After 0.60 mol of H2 is added to the 2.0-L container and equilibrium is re-established, what are the new concentrations of all the components?

Problem 61P The minerals hematite (Fe2O3) and magnetite (Fe3O4) exist in equilibrium with atmospheric oxygen: 4Fe3O4(s) + O2(g) ? 6Fe2O3(s)Kp = 2.5 X1087 at 298 K (a) Determine PO2, at equilibrium, (b) Given that PO2 in air is 0.21 atm, in which direction will the reaction proceed to reach equilibrium? (c) Calculate Kc at 298 K.

Problem 59P Predict the effect of increasing the temperature on the amounts of products in the following reactions: (a) CO(g) + 2H2(g) ? CH3OH(g) ?H°rxn = ?90.7 kJ ________________ (b) C(s) + H2O(g) ? CO(g) + H2(g) ?H°rxn = 131 kJ ________________ (c) 2NO2(g) 2NO(g) + O2(g) (endothermic) ________________ (d) 2C(s) + O2(g) ? 2CO(g) (exothermic)

Problem 60P Predict the effect of decreasing the temperature on the amounts of reactants in the following reactions: (a) C2H2(g) + H2O(g) ? CH3CHO(g) ?H°rxn = ?151 kJ ________________ (b) CH3CH2OH(l) + O2(g) ? CH3CO2H(l) + H2O(g) ?H°rxn = ?451 k J] ________________ (c) 2C2H4(g) + O2(g) ? 2CH3CHO(g) (exothermic) ________________ (d) N2O4(g) ? 2NO2(g) (endothermic)

For the reaction \(\mathrm{M}_{2}+\mathrm{N}_{2} \rightleftharpoons 2 \mathrm{MN}\), scene A represents the mixture at equilibrium, with M black and N orange. If each molecule represents 0.10 mol and the volume is 1.0 L, how many moles of each substance will be present in scene B when that mixture reaches equilibrium? Equation Transcription: <math xmlns="http://www.w3.org/1998/Math/MathML"><msub><mi mathvariant="normal">M</mi><mn>2</mn></msub><mo>&#xA0;</mo><mo>+</mo><mo>&#xA0;</mo><msub><mi mathvariant="normal">N</mi><mn>2</mn></msub><mo>&#xA0;</mo><mo>&#x21CC;</mo><mo>&#xA0;</mo><mn>2</mn><mi>MN</mi></math> Text Transcription: M_2+N_2 rightleft harpoon 2MN

An industrial chemist introduces \(2.0 atm\) of \(\mathrm{H}_{2}\) and \(2.0 atm\) of \(\mathrm{CO}_{2}\) into a 1.00-L container at \(25.0^{\circ} \mathrm{C}\) and then raises the temperature to \(700^{\circ} \mathrm{C}\), at which \(K_{c}=0.534\): How many grams of H2 are present at equilibrium? Equation Transcription: H2 CO2 25.0°C 700.°C ????c = 0.534 Text Transcription: 2.0 atm H_2 CO_2 25.0°C 700.°C ????_c = 0.534

As an EPA scientist studying catalytic converters and urban smog, you want to find \(K_{\mathrm{c}}\) for the following reaction: Use the following data to find the unknown ????c: Equation Transcription: ????c Text Transcription: K_c

When \(0.100 mol\) of \(\mathrm{CaCO}_{3}(s)\) and 0.100 mol of CaO(s) are placed in an evacuated sealed \(10.0-L\) container and heated to \(385 \mathrm{~K}, P_{\mathrm{CO}_{2}}=0.220\) atm after equilibrium is established: An additional \(0.300 atm\) of \(\mathrm{CO}_{2}(\mathrm{~g})\) is then pumped into the container. What is the total mass (in g) of \(\mathrm{CaCO}_{3}(s)\) after equilibrium is re-established? Equation Transcription: CaCO3(s) CO2(g) Text Transcription: 0.100 mol CaCO_3(s) 0.100 mol 10.0-L 385 K._P-Co_2=0.220 0.300 atm CO_2(g)

An engineer examining the oxidation of \(\mathrm{SO}_{2}\) in the manufacture of sulfuric acid determines that \(K_{\mathrm{c}}=1.7 \times 10^{8} \text { at } 600 . \mathrm{K}\): (a) At equilibrium, \(P_{\mathrm{SO}_{3}}=300\) atm and \(P_{\mathrm{O}_{2}}=100 . \mathrm{atm}\). Calculate \(P_{\mathrm{SO}_{2}}\). (b) The engineer places a mixture of 0.0040 mol of \(\mathrm{SO}_{2}(\mathrm{g})\) and 0.0028 mol of \(\mathrm{O}_{2}(\mathrm{g})\) in a 1.0-L container and raises the temperature to 1000 K. At equilibrium, 0.0020 mol of \(\mathrm{SO}_{3}(\mathrm{g})\) is present. Calculate \(K_{\mathrm{c}}\) and \(P_{\mathrm{SO}_{2}}\) for this reaction at 1000. K. Equation Transcription: SO2 ????c = 1.7108 at 600. K <math xmlns="http://www.w3.org/1998/Math/MathML"><msub><mi>P</mi><msub><mi>SO</mi><mn>3</mn></msub></msub><mo mathvariant="italic">&#xA0;</mo><mo>=</mo><mo>&#xA0;</mo><mn>300</mn><mo mathvariant="italic">.</mo></math> <math xmlns="http://www.w3.org/1998/Math/MathML"><msub><mi>P</mi><msub><mi mathvariant="normal">O</mi><mn>2</mn></msub></msub></math> = 100 <math xmlns="http://www.w3.org/1998/Math/MathML"><msub><mi>P</mi><msub><mi>SO</mi><mn>2</mn></msub></msub></math> SO2(g) O2(g) ????c Text Transcription: SO_2 K_c=1.7 times 10^8 at 600. K P_SO_3 = 300 P_0_2=100 P_SO_2 SO_2(g) O_2(g) K_c

The “filmstrip” represents five molecular-level scenes of a gaseous mixture as it reaches equilibrium over time: \(\mathrm{X}\) is purple and \(\mathrm{Y}\) is orange: \(\mathrm{X}_{2}(\mathrm{~g})+\mathrm{Y}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{XY}(\mathrm{g})\). (a) Write the reaction quotient, \(Q\), for this reaction. (b) If each particle represents \(0.1 \mathrm{~mol}\) of particles, calculate \(Q\) for each scene. (c) If \(K>1\), is time progressing to the right or to the left? Explain. (d) Calculate \(K\) at this temperature. (e) If \(\Delta H_{\mathrm{rxn}}^{\circ}<0\), which scene, if any, best represents the mixture at a higher temperature? Explain. (f) Which scene, if any, best represents the mixture at a higher pressure (lower volume)? Explain.

Use each reaction quotient to write the balanced equation: a. \(Q=\frac{\left[\mathrm{CO}_{2}\right]^{2}\left[\mathrm{H}_{2} \mathrm{O}\right]^{2}}{\left[\mathrm{C}_{2} \mathrm{H}_{4}\right]\left[\mathrm{O}_{2}\right]^{3}}\) b. \(Q=\frac{\left[\mathrm{NH}_{3}\right]^{4}\left[\mathrm{O}_{2}\right]^{7}}{\left[\mathrm{NO}_{2}\right]^{4}\left[\mathrm{H}_{2} \mathrm{O}\right]^{6}}\) Equation Transcription: Text Transcription: Q = [CO_2]^2[H_2O]^2/[C_2H_4][O_2]^3 Q = [NH_3]^4[O_2]^7[NO_2]^4[H_2O]^6

Problem 75P When ammonia is made industrially, the mixture of N2, H2, and NH3 that emerges from the reaction chamber is far from equilibrium. Why does the plant supervisor use reaction conditions that produce less than the maximum yield of ammonia?

Consider the following reaction: \(3 \mathrm{Fe}(\mathrm{s})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{s})+4 \mathrm{H}_{2}(\mathrm{g})\) (a) \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) is a compound of iron in which Fe occurs in two oxidation states. What are the oxidation states of Fe in \(\mathrm{Fe}_{3} \mathrm{O}_{4}\)? (b) At \(900^{\circ} \mathrm{C}\), Kc for the reaction is 5.1. If 0.050 mol of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) and 0.100 mol of \(F e(s)\) are placed in a 1.0-L container at \(900^{\circ} \mathrm{C}\), how many grams of \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) are present at equilibrium? Note: The synthesis of ammonia is a major process throughout the industrialized world. Problems 17.75 to 17.79 refer to various aspects of this all-important reaction: \(\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{g}) \quad \Delta H^{\circ} r_{\mathrm{rxn}}=-91.8 \mathrm{kJ}\) Equation Transcription: 900°C Kc Text Transcription: 3Fe(s) + 4H_2O(g) ? Fe_3O_4(s) + 4H_2(g) Fe_3O_4 900°C K_c H_2O(g) Fe(s) 900°C N_2(g) + 3H_2(g) ? 2NH_3(g) Delta H°_rxn = -91.8 kJ

One mechanism for the synthesis of ammonia proposes that \(N_{2}\) and \(H_{2}\) molecules catalytically dissociate atoms: \(\begin{array}{ll} N_{2}(g) \rightleftharpoons 2 N(g) & \log K_{p}=-43.10 \\ H_{2}(g) \rightleftharpoons 2 H(g) & \log K_{p}=-17.30 \end{array} \) (a) Find the partial pressure of N in \(N_{2}\) at 1000. K and 200. Atm. (b) Find the partial pressure of H in \(H_{2}\) at 1000.K and 600. Atm. (c) How many N atoms and H atoms are present per liter? (d) Based on these answers, which of the following is a more reasonable step to continue the mechanism after the catalytic dissociation? Explain. \(\begin{array}{l} N(g)+H(g) \rightarrow N H(g) \\N_{2}(g+H(g) \rightarrow N H(g)+N(g) \end{array} \) Equation Transcription: Text Transcription: N_2 H_2 N_2(g) ? 2N(g) log K_p = -43.10 H_2(g) ? 2H(g) log K_p = -17.30 N(g) + H(g) rightarrow NH(g) N_2(g + H(g) rightarrow NH(g) + N(g)

An equilibrium mixture of car exhaust gases consisting of 10.0 volumes of \(\mathrm{CO}_{2}\), 1.00 volume of unreacted \(\mathrm{O}_{2}\), and 50.0 volumes of unreacted \(N_{2}\) leaves the engine at 4.0 atm and 800. K. (a) Given this equilibrium, what is the partial pressure of CO? \(2 \mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)+O_{2}(g) \quad K_{p}=1.4 \times 10^{-28} \text { at } 800 . \mathrm{K}\) (b) Assuming the mixture has enough time to reach equilibrium, what is the concentration in picograms per liter (pg/L) of CO in the exhaust gas? (The actual concentration of CO in car exhaust is much higher because the gases do not reach equilibrium in the short transit time through the engine and exhaust system.). Equation Transcription: at 800. K Text Transcription: CO_2 O_2 N_2 2CO_2(g) ? 2CO(g) + O2(g) K_p=1.4x10^-28 at 800. K

You are a member of a research team of chemists discussing the plans to operate an ammonia processing plant: \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{g})\) (a) The plant operates at close to 700 K, at which \(K_{p}\) is \(1.00 \times 10^{-14}\), and employs the stoichiometric 1/3 ratio of \(\mathrm{N}_{2} / \mathrm{H}_{2}\) At equilibrium, the partial pressure of \(\mathrm{NH}_{3}\) is 50. atm. Calculate the partial pressures of each reactant and \(P_{\text {total. }}\). (b) One member of the team makes the following suggestion: since the partial pressure of \(\mathrm{H}_{2}\) is cubed in the reaction quotient, the plant could produce the same amount of \(\mathrm{NH}_{3}\) if the reactants were in a 1/6 ratio of \(\mathrm{N}_{2} / \mathrm{H}_{2}\) and could do so at a lower pressure, which would cut operating costs. Calculate the partial pressure of each reactant and \(P_{\text {total. }}\) under these conditions, assuming an unchanged partial pressure of 50. atm for \(\mathrm{NH}_{3}\) Is the team member’s argument valid? Equation Transcription: 1.00x10-14 Ptotal. Text Transcription: N_2(g) + 3H_2(g) ? 2NH_3(g) Kp 1.00x10^-14 N_2/ H_2 NH_3 Ptotal. H_2

Isopentyl alcohol reacts with pure acetic acid to form isopentyl acetate, the essence of banana oil: \(\mathrm{C}_{5} \mathrm{H}_{11} \mathrm{OH}+\mathrm{CH}_{3} \mathrm{COOH} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOC}_{5} \mathrm{H}_{11}+\mathrm{H}_{2} \mathrm{O}\) A student adds a drying agent to remove \(\mathrm{H}_{2} \mathrm{O}\) and thus increase the yield of banana oil. Is this approach reasonable? Explain. Equation Transcription: C5H11OH + CH3COOH ? CH3COOC5H11 + H2O H2O Text Transcription: C_5H_11OH + CH_3COOH ? CH_3COOC_5H_11 + H_2O H_2O

The two most abundant atmospheric gases react to a tiny extent at 298 K in the presence of a catalyst: \(\mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g}) \quad K_{p}=4.35 \times 10^{-31}\) (a) What are the equilibrium pressures of the three components when the atmospheric partial pressures of \(\mathrm{O}_{2}\) (0.210 atm) and of \(\mathrm{N}_{2}\) (0.780 atm) are put into an evacuated 1.00-L flask at 298 K with catalyst? (b) What is \(P_{\text {total}}\) in the container? (c) Find \(\mathrm{K}_{c}\) for this reaction at 298 K. Equation Transcription: N2 + O2 ? 2NO Kp = 4.35x10-31 O2 N2 Ptotal Kc Text Transcription: N_2(g) + O_2(g) ? 2NO(g) K_p = 4.35x10^-31 O_2 N_2 P_total K_c

For the equilibrium \(2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \quad K_{0}=9.10 \times 10^{-8} \text { at } 700^{\circ} \mathrm{C}\) the initial concentrations of the three gases are \(0.300 \mathrm{MH}_{2} \mathrm{S}\), \(0.300 \mathrm{MH}_{2}\) and \(0.150 \mathrm{MS}_{2}\). Determine the equilibrium concentrations of the gases. Equation Transcription: 2H2S? 2H2 + S2 Kc = 9.10x10-8 at 700°C 0.300 M H2S 0.150 M S2 Text Transcription: 2H_2S(g)? 2H_2(g) + S_2(g) K_c = 9.10x10^-8 at 700°C 0.300 M H_2S 0.150 M S_2

The molecular scenes depict the reaction \(Y \rightleftharpoons 2 Z\) at four different times, out of sequence, as it reaches equilibrium. Each sphere (Y is red and Z is green) represents \(0.025 mol\) and the volume is \(0.40 L\). (a) Which scene(s) represent(s) equilibrium? (b) List the scenes in the correct sequence. (c) Calculate Kc. Equation Transcription: Y ? 2Z Text Transcription: Y ? 2Z 0.025 mol 0.40 L

Isomers \(Q\) (blue) and \(R\) (yellow) interconvert. They are depicted in an equilibrium mixture in scene \(A\). Scene \(B\) represents the mixture after addition of more \(Q\). How many molecules of each isomer are present when the mixture in scene \(B\) attains equilibrium again? Equation Transcription: Text Transcription: Q R A B

Using CH4 and steam as a source of H2 for NH3 synthesis requires high temperatures. Rather than burning CH4 separately to heat the mixture, it is more efficient to inject some oxygen into the reaction mixture. All of the H2 is thus released for the synthesis, and the heat of reaction for the combustion of CH4 helps maintain the required temperature. Imagine the reaction occurring in two steps: \(\begin{aligned} 2 \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})+4 \mathrm{H}_{2}(\mathrm{~g}) & \\ K_{p} &=9.34 \times 10^{28} \text { at } 1000 . \mathrm{K} \\ \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+{H}_{2}(\mathrm{~g}) & \\ K_{p} &=1.374 \text { at } 1000 . \mathrm{K} \end{aligned} \) (a) Write the overall equation for the reaction of methane, steam, and oxygen to form carbon dioxide and hydrogen. (b) What is Kp for the overall reaction? (c) What is Kc for the overall reaction? (d) A mixture of 2.0 mol of CH4 , 1.0 mol of O2 , and 2.0 mol of steam with a total pressure of 30. atm reacts at 1000. K at constant volume. Assuming that the reaction is complete and the ideal gas law is a valid approximation, what is the final pressure? Equation Transcription: at 1000. K at 1000. K Text Transcription: 2CH_4(g) + O_2(g) ? 2CO(g) + 4H_2(g) K_p = 9.341028 at 1000. K CO(g) + H_2O(g) ? CO_2(g) + H_2(g) K_p = 1.374 at 1000. K

Problem 85P In a study of synthetic fuels, 0.100 mol of CO and 0.100 mol of water vapor are added to a 20.00-L container at 900°C, and they react to form CO2 and H2. At equilibrium, [CO] is 2.24 × 10?3M (a) Calculate Kc at this temperature. (b) Calculate Ptotal in the flask at equilibrium. (c) How many moles of CO must be added to double this pressure? (d) After Ptotal is doubled and the system reattains equilibrium, what is [CO]eq?

Glauber’s salt, \(\mathrm{Na}_{2} \mathrm{SO}_{4} \cdot 10 \mathrm{H}_{2} \mathrm{O}\), was used by J. R. Glauber in the 17th century as a medicinal agent. At \(25^{\circ} \mathrm{C}, K_{p} 4.08 \times 10^{-25}\) for the loss of water of hydration from Glauber’s salt: \(\mathrm{Na}_{2} \mathrm{SO}_{4} \cdot 10 \mathrm{H}_{2} \mathrm{O}(s) \rightleftharpoons \mathrm{Na}_{2} \mathrm{SO}_{4}(s) \cdot 10 \mathrm{H}_{2} \mathrm{O}(g)\) (a) What is the vapor pressure of water at \(25^{\circ} \mathrm{C}\) in a closed container holding a sample of \(\mathrm{Na}_{2} \mathrm{SO}_{4} \cdot 10 \mathrm{H}_{2} \mathrm{O}(s)\)? (b) How do the following changes affect the ratio (higher, lower,same) of hydrated form to anhydrous form for the system above? (1) Add more \(\mathrm{Na}_{2} \mathrm{SO}_{4}(s)\) (2) Reduce the container volume (3) Add more water vapor (4) Add \(\mathrm{N}_{2}\) gas Equation Transcription: Na2SO410H2O 25°C, Kp 4.08x10-25 Na2SO410H2O(s) ? Na2SO4(s)10H2O 25°C Na2SO4(s) N2 Text Transcription: Na_2SO_4 times 10H_2O 25°C, K_p 4.08x10^-25 Na_2SO_4 times 10H_2O(s) ? Na_2SO_4(s) times 10H_2O(g) 25°C Na_2SO_4(s) N_2