Sulfur trioxide (SO3) dissolves in and reacts with water to form an aqueous solution of sulfuric acid (H2SO4). The vapor in equilibrium with the solution contains both SO3 and H2O. If enough SO3 is added, all of the water reacts and the solution becomes pure H2SO4. If still more SO3 is added, it dissolves to form a solution of SO3 in H3SO4, called oleum or fuming sulfuric acid. The vapor in equilibrium with oleum is pure SO3. Twenty percent oleum by de?nition contains 20 kg of dissolved SO3 and 80 kg of H2SO4 per hundred kilograms of solution. Alliteratively, the oleum composition can be expressed as % SO3 by mass, with the constituents of the oleum considered to be SO3 and H2O.
(a) Prove that a 15.0% oleum contains 84.4% SO3.
(b) Suppose a gas stream at 40°C and 1.2 atm containing 90 mole% SO3 and 10% N2 contacts a liquid stream of 98 wt% H2SO4 (aq), producing 15% oleum. Tabulated equilibrium data indicate that the partial pressure of SO3 in equilibrium with this oleum is 1.15 mm Hg. Calculate (i) the mole fraction of SO3 in the outlet gas if this gas is in equilibrium with the liquid product at 40°C and 1 atm, and (ii) the ratio (m3 gas feed)/(kg liquid feed).
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Chapter 6 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
Additional Science Textbook Solutions
Elements of Chemical Reaction Engineering (5th Edition) (Prentice Hall International Series in the Physical and Chemical Engineering Sciences)
Process Dynamics and Control, 4e
Objects First with Java: A Practical Introduction Using BlueJ (6th Edition)
ANALYSIS+DESIGN OF LINEAR CIRCUITS(LL)
Introductory Circuit Analysis (13th Edition)
- According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?arrow_forwardA 0.250-M sodium sulfate solution is added to a 0.200-M barium nitrate solution and 0.700 g barium sulfate precipitates. Write the balanced equation for this reaction. Calculate the minimum volume of barium nitrate solution that was used. Calculate the minimum volume of sodium sulfate needed to precipitate 0.700 g barium sulfate. Assume 100% yield.arrow_forwardThe hydrocarbon naphthalene was frequently used in mothballs until recently, when it was discovered that human inhalation of naphthalene vapors can lead to hemolytic anemia. Naphthalene is 93.71% carbon by mass, and a 0.256-mole sample of naphthalene has a mass of 32.8 g. What is the molecular formula of naphthalene? This compound works as a pesticide in mothballs by. sublimation of the .solid so that it fumigates enclosed spaces with its vapors according to the equation Naphthalene(s)naphthalene(g)K=4.29106(at298K) If 3.00 g solid naphthalene is placed into an enclosed space with a volume of 5.00 L at 25C, what percentage of the naphthalene will have sublimed once equilibrium bas been established?arrow_forward
- You are designing a process to remove carbonate ions from an aqueous system by precipitation. If the effectiveness of the process is the only concern (meaning there are no environmental or other issues involved), which of the following metal ions would be the best choice: Ca2+,Fe2+,Pb2+,orAg2+ ? Explain your answer. Salt Ksp CaCO3 4.8109 FeCO3 3.51011 PbCO3 1.51013 Ag2CO3 8.21012arrow_forwardThe ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forward
- Which of the following is the correct equilibrium law for the following reactions N2(g) + 3H2(g) 2NH3(g) Select one: O a. K, = O b. K, = [NH,] [N ][H,]° [TH,] O c. K, = O d. K, = [NE, Which of the following is the expression for the solubility product of Baz(AsO2)2? earch F4 F5 F6 FZ F8 F9 F10 F11 %24 4 6 8 R T. Y 10O F G H J K V Barrow_forward500 mL of 0.0100 M CaCl2 is mixed with 500 mL of 0.0100 M Na2SO4. How many grams of CaSO4 will precipitate when the equilibrium is reached? The solubility product constant of CaSO4 is Ksp = 2.50 × 10–5. MM(CaSO4) = 136.14 g mol–1. A. 0.68 g B. 2.04 g C. 1.36 g D. No precipitate will form E. 5.45 garrow_forwardTo 200 ml of a solution containing 0.002 mol of aluminium chloride and 0.001 mol of calcium chloride is slowly added solid sodium phosphate (assuming no change in volume). How many grams of sodium phosphate must be added to precipitate as much of one ion as possible, while the other ion just doesn't precipitate? What percentage of the ion that will precipitate first is left in the solution at that moment?arrow_forward
- (a) If the molar solubility of Nd₂(CO3)3 at 25 °C is 1.00e-07 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 8.90e-06 g of Y₂(CO3)3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility- product constant for Y₂(CO3)3. Ksp = (c) The Ksp of Ag₂C₂04 at 25 °C is 5.40e-12. What is the molar solubility of Ag2C₂04? solubility mol/Larrow_forwardCompare the solubility of barium sulfate in each of the following aqueous solutions: Clear All 0.10 М Ba(СHзсо0) More soluble than in pure water. 0.10 M (NH4)2S04 Similar solubility as in pure water. 0.10 М КСH3CO0 Less soluble than in pure water. 0.10 Μ ΗΝΟ;arrow_forwardGiven: 2N2(g)+ O2(g) = 2N20(g); Ke(1) = 5.8 x 10-36 and N2(g) + O2(g) = 2NO(g); K(2) = 4.1 x 10-31 What is the equilibrium constant for the reaction? 2N20(g) + O2(g) = 4NO(g)arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133109655/9781133109655_smallCoverImage.jpg)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780534420123/9780534420123_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079113/9781305079113_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079243/9781305079243_smallCoverImage.gif)