A dilute aqueous solution of sulfuric acid at 25°C is used to absorb ammonia in a continuous reactor, thereby producing ammonium sulfate, a fertilizer:
If the ammonia enters the absorber at 75°C, the sulfuric acid enters at 25°C, and the product solution emerges at 25°C, how much heat must be withdrawn from the unit per mol of
- produced? (All needed physical property data may be found in Appendix B.)
- Estimate the final temperature if the reactor of Part (a) is adiabatic and the product of the solution contains 1.00 mole% ammonium sulfate. Take the heat capacity of the solution to be that of pure liquid water [4.184kJ/(kg·°C)].
- In a real (imperfectly insulated) reactor, would the final solution temperature be less than, equal to, or greater than the value calculated in Part (b), or is there no way to tell without more information? Briefly explain your answer.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 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
Differential Equations: Computing and Modeling (5th Edition), Edwards, Penney & Calvis
Modern Database Management
Computer Science: An Overview (12th Edition)
Thinking Like an Engineer: An Active Learning Approach (4th Edition)
- 30. The following reaction takes place. A,B(s) = 2A(ac) + B(ag) + heat. If 1.80 moles of A,B is added into a 1.00 L container, it is found that 30.0% of the reactant dissociates to reach equilibrium. Find the solubility product constant, Ksp, for this reaction. Note: Your answer must include an ICE table. (aq),arrow_forwardPlease answer this with work shown! Thank you!arrow_forwardCalculate the maximum mass of pure iron that can be produced by the concentration of 350 t of coke. Please don't round when doing matharrow_forward
- 1 H,(9) + 2 NO(g) · N,O(g) + H,O(g) k1 2 H2(g) + N,0(g) → N,(9) + H,O(g) k2 Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: 2H, (g) + 2NO(g) 2H,0(g) + N, Write the experimentally- observable rate law for the overall chemical reaction. rate = k H,NO2 Note: your answer should not contain the concentrations of intermediates. any Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k1 and k-2 for = K,] 21 the reverse of the two elementary reactions in the mechanism.arrow_forwardA 51.0-LL reactor at 1600 KK is charged with 50.0 gg of NiO(s)NiO(s) and 1.40 atmatm of CO(g)CO(g). After equilibrium is reached, what is the partial pressure of CO2(g)CO2(g) in the reactor?arrow_forwardAgBr(s) = Ag*(aq) + Br(aq) Ksp = 5.30 x 10-13 Ag (aq) + 2NH3(aq) [Ag(NH3)₂1 (aq) K+ = 1.70x107 123 When NH3(aq) is added to AgBr(s), a combination of these two reactions occurs: AgBr(s) + 2NH3(aq) == [Ag(NH3)2]* (aq) + Br (aq) What mass of AgBr(s) (187.8 g/mol) can react with 1.00 L of 3.22 M NH3? Provide answer in grams to 3 significant figures.arrow_forward
- 3. One process for removing CO₂ from the atmosphere is to convert CO₂ to carbonate (CO3²) and then precipitate it as calcite (CaCO3). The following equilibria are relevant to this process: CO₂ (g) + 2 OH (aq) → CO32 (aq) + H₂O (1) CaCO3 (s) + 2OH- Ca(OH)2 (aq) + CO3-2 (aq) Write the K, expression for these equilibria and for the overall reaction of CO2 with Ca(OH)2.arrow_forwardSilver chloride is classified as an insoluble compound because it dissolves only to a small extent in water. Consider the balanced equation and equilibrium constant that shows the partial dissolving of silver chloride in water: AgCl(s) = Ag*(aq) + CI"(ag) Keg = 1.70 x 10-10 a) The reaction AgCl(s) = Ag*(aq) + Cl (ag) is classified as a (homogeneous or heterogeneous) equilibrium because it involves more than one physical state, solid and aqueous. b) Based on the equilibrium constant value and the equilibrium constant expression, the concentration of each ion in a saturated solution of silver chloride is : Concentration of Ag = x 10 Concentration of CI" = x 10 Marrow_forwardConsider a general reaction enzyme A(aq) = B(aq) The AGo of the reaction is-8.290 kJ · mol. Calculate the equilibrium constant for the reaction at 25 °C. %3D What is AG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.50 M? kJ mol-! AG = %3D |help terms of use contact us careers privacy policy about s MacBook Proarrow_forward
- One of the major factors influencing seasonal ozone loss in the Antarctic winter is the dimerization of CIO in the stratosphere. The equilibrium constant (K) for the reaction 2 CIO(g) → (CIO)2 (g) at different temperatures is shown below. (Data obtained from Nature 332, 796 (1988)). • T(K) 233 248 258 268 273 280 288 295 303 4.13 5.00 1.45 5.37 3.20 K 9.62 4.28 1.67 7.02 ×108 ×107 ×107 ×106 ×106 ×10$ x105 ×105 ×104 a) Determine the standard enthalpy and standard entropy of this reaction. b) Calculate the standard enthalpy of formation and the standard molar entropy of (CIO)2 given that AH°(CIO) = 101.8 kJ/mol and AS° (cio) = 226.6 J/molkarrow_forwardTwo reactants are placed into a flask. A single displacement reaction occurs, with the general reaction scheme of: 2 AB + 2X2 → 2 AX2 + B2 What are the potential identities of A, B, and X?arrow_forwardGiven the solubility of ferrihydrite (Fe(OH)3) and goethite (FeOOH), with dissolution reactions shown below: [1] Fe(OH)3 3 H+ à Fe3+ + 3 H2O Ksp = 8.4 x 10^4 ∆ Gr0 = -28 KJ/mol Solubility of Fe(OH3) = 7.468 [2] FeOOH + 3 H+ à Fe3+ + 2 H2O Ksp = 8.8 x 10^-2 ∆ Gr0 = 6 KJ/mol Solubility of FeOOH = 0.353 QUESTION: [A] How much Fe3+ from ferrihydrite would dissolve at pH 2 ? [B] How much Fe3+ from ferrihydrite would dissolve at pH 7 ? [C] How much Fe3+ from goethite would dissolve at pH 2 ? [D] How much Fe3+ from goethite would dissolve at pH 7 ?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning