Consider the reaction:Ca(OH)2 (aq) + 2HCl(aq) → CaCl2 (s) + 2H₂O(1)Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 2.04 moles of Ca(OH)2 (aq) react at standard conditions.AS⁰Substance AH (kJ/mol)Ca(OH)2 (aq)HCl(aq)CaCl₂ (s)H₂O (1)surroundings-1002.8-167.2-795.8-285.8J/K

△S°surrounding = (△H°reaction /T) △H°reaction =2×△Hf°(H2O) +△Hf°(CaCl2) -2×△Hf°(HCl)-△Hf°(Ca(OH)2 )…

Answered: Consider the reaction: Ca(OH)2 (aq) +…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Mn in groundwaterA ground water has the following conditions:{Mn2+ (aq)} = 1.0x10 -5pH = 7.0 (i.e., {H+ } = 1.0x10-7)Saturated with oxygen from the atmosphere: {O 2(aq)} = 2.63x10 -4T = 25 °C(a) Write the balanced equation for oxidation of reduced manganese,Mn2+ (aq), by dissolved oxygen (O 2(aq)) to generate MnO 2(s)(manganese dioxide) or MnOOH(s) (manganite), respectively.(b) Determine whether each of the above two reactions isthermodynamically favorable in the ground water. Which phase ofthe manganese oxide is more stable in the ground water?(c) If groundwater is at 5 oC, does oxidation of Mn 2+ (aq) by dissolvedoxygen to generate MnO 2(s) become more or less favorable?Calculate the saturated {Mn 2+ (aq)} assuming the water pH remainsat 7.0 and the dissolved oxygen concentration is 3.73x10 -4 M. 25C and 1 atm Please be as detailed as possible. I want to be able to replicate. Thank you so much. :)
Consider the excess chemical potential of a gas, Hex = Hig, where Hg is the ideal contribution. Show that it can be calculated at a given number density p and temperature T by use of the relation peZ(T,p') – 1 dp' + Z(T,p) – 1– In Z(T, p) p' Hex kgT In addition, find Hax for a fluid described by a second-order virial expansion, kgTP+ B2p?
2. Consider the following reaction: CO) +=O=COz) s) Find AH (kJ/mol) of the reaction at 298 K and 1 bar (b) ›) Determine the spontaneity of the reaction in a furnace operating at 2000 K where the partial pressures of the compounds are: Compound iP (bar) CO(R) O₂(g) CO2(g) Consider that for this reaction AG2000k = -111 kJ/mol 0.05 2.00 2.50
Consider the following samples of gas.Select the set of graphs below that show the distributions of the speed of the atoms in each sample (please take a photo of the correct graph).
Q6. Nickel at 650∘∘C has 1.50 x 1015 vacancies/cm3. The atomic weight of Ni is 58.69 g/mol and the density at this temperature is 8.6 g/cm3. (10 points) (a) What is the activation energy required to create a vacancy in Ni? (b) Ni is then cooled to 400∘∘C. What will be the number of vacancies per cubic centimeter? Assume that the change in the density in the cooling is negligible.
I only want number 2 answered. The question is based on number one
QUESTION 3 Using AfGO given below at 25°C for the reactants and products to calculate the standard Gibbs energy AGO. Please enter your answer (unit: kJ/mol) with one decimal. for example, 100.345 is written as 100.3, and pay attention to the sign. AfGO (kJ/mol) SO2 (g) + 12 O2(g) SO3(g) -300.1 0 -374.2
Regarding the following reaction, A (s) + 2B (g) →→ C (1) + 3D (g) ArH(298K)=91.4kJ/mol where g, I, s - means gas, liquid and solid, respectively, and assuming all gases are perfect gas, calculate ArU(298K). Instruction: Please enter your answer (unit:kJ/mole) round to 2 decimal place.
1 mol of water solidifies at 95.0 oC and 1 atm.Calculate the (I) entropy of the sample, (II) entropy of the surroundings, (III) total entropy change for the following processes. Are these processes spontaneous? Consult the table below. You will need to use the fact that entropy is a state function to make these calculations.a.1 mol of water solidifies at -5.0 oC and 1atm b. 1 mol of water solidifies at 95.0 oC and 1 atm.
P.9 Assume that a sealed vessel at constant pressure of 1 bar initially contains 2.00 mol of NO₂(g). The system is allowed to equilibrate with respect to the reaction 2 NO₂(g) N₂O4(g). The number of moles of NO₂(g) and N₂O4(g) at equilibrium is 2.00 - 2 and , respectively, where is the extent of reaction. a. Derive an expression for the entropy of mixing as a func- tion of . b. Graphically determine the value of ₹ for which AS mixing has its maximum value. c. Write an expression for Gpure as a function of §. Use Equation 104 to obtain values of Gm for NO2 and N₂O4. d. Plot Gmixture = Gpure + AGmixing as a function of for ₹ T = 298 K and graphically determine the value of & for which Gmixture has its minimum value. Is this value the same as for part (b)?

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