A process of synthesizing NH3 through the reaction:3H (g) + N (g) 2 2NH (g)AG°(NH )16500J(pada 25ºC)molAH reaction = -92.400 J/mol.Ammonia synthesis is difficult to carry out although thermodynamically the processcan take place spontaneously.a) Explain why ammonia is difficult to produce on an industrial scale?b) What is the solution so that ammonia synthesis can run quickly so that it is profitable ifit is produced on an industrial scale?

The catalyst currently used in the Haber process: Finely divided iron along with potassium…

Answered: A process of synthesizing NH3 through…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Determine ΔG°rxn for the following reaction: N2O (g) + NO2 (g) à 3 NO (g)ΔG° = ? Use the following reaction with known ΔG° values. Rxn 1:2 NO (g) + O2 (g) à 2 NO2 (g)ΔG1° = - 71.2 kJ Rxn 2:N2 (g) + O2 (g) à 2 NO (g)ΔG2° = + 175.2kJ Rxn 3:2 N2O (g) à 2 N2 (g) + O2 (g) ΔG3° = - 207.4kJ
A student determines the value of the equilibrium constant to be 5.14×1091 for the following reaction.H2CO(g) + O2(g)CO2(g) + H2O(l)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 2.29 moles of H2CO(g) at standard conditions at 298K. G°rxn = ____________ kJ
Given the following thermodynamic data: CO2(g) + 2NH3(g) → CO(NH2)2(s) + H2O(l) ΔH°298 =-133.3 kJ ΔG°298 =-6.97 kJ ΔH°f (kJ/mol) -393.5 -46.11 -285.8 S° (J/mol K) 213.6 192.3 104.6 69.91 a) Determine ΔH⁰f for CO(NH2)2(s) b) Determine K for the reaction at 298 K c) Determine ΔS⁰ for the reaction in units of J/K d) Determine ΔG if the pressure of CO2 is 0.450 bar and the pressure of NH3 is 0.650 bar e) Determine K for the reaction at 250 K
Use the reaction for the formation of NH3 from its elements N2(g) and H2(g) . This reaction has the following thermodynamic data: ΔfHo (NH3) = - 45.9 kJ/mol and ΔfSo (NH3) = - 99.1 J/mol*K at 298 K a) Write a balanced equation (whole number ratios) for this process and write out the expression for the reaction quotient Q using partial pressures. b) Without doing any calculations, explain how the progression of the reaction will change (more reactants or more products) with respect to 1) increasing temperature, and 2) increasing pressure. c) Calculate the equilibrium constant K at 298 K d) Assuming that : ΔfHo is independent of temperature, calculate K at - 78o C
1. Consider the reaction: A 2 B, where Keg 1.33 x 10-1. (a) What is the AGº' for this reaction? (b) If the reaction above is initially at standard-state conditions, what are the concentrations of A and B once equilibrium is reached?
15. See image below: * 15. Given the enthalpy changes for the following reactions, calculate AH,° for CO(a C(graphite) +1/202 → CO C(gaphite)+ O2g →CO2 CO( + 1/202 → CO12) AH° = -393.5 kJ AH = -283.0 kJ %3D O -110.5 kJ O +6.78 x 10² kJ O -6.78 x 102 kJ O +110.5 kJ
Using ONLY the information given in the problem (no thermodynamic table), calculate the standard free energy change for this reaction. At 298K, K = 6.74 x 106 for the following reaction: %3D C;H,O3 (g) C,H6(g) + 3CO(g)
Most of the coal available in the United States is bituminous or "soft" coal, which contains as much as 5% sulfur by weight. When this coal is burned, the sulfur reacts with oxygen to form sulfur dioxide gas. When the sulfur dioxide gas dissolves in raindrops, it forms sulfuric acid. This is how we get acid rain. Here is the reaction that produces sulfur dioxide gas when soft coal is burned: S,()+80, (g) - 880,(g) Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 153.9 g of solid sulfur and 27.1g of oxygen gas each. The volume and temperature of each vessel is shown in the table below. db Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. initial rate of vessel volume…
Calculate AG° for the reaction shown below using the provided thermodynamic properties information. H2O2 (1) → 2 H2O () + O2 (g) Substance AH°; (kJ/mol) AS° (J/(mol•K)) H2O2 (1) - 187.8 232.9 H20 (1) -285.83 69.91 O2 (g) 205.0 -396.4 kJ/mol -350.5 kJ/mol -33.70 kJ/mol -1105 kJ/mol -417.2 kJ/mol
a) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) = -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l) b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?
9. For the reaction: 2 CH,OH(g) + H2(g) - C2H(g) + 2 H2O(g) a) Calculate AG° for this reaction using free energy values in your text book. b) Calculate AG at standard temperature when the pressure of CH3OH is 4.97 atm, H2 is 3.56 atm, C2H6 is 4.85 atm, and H20 is 2.18 atm. c) Calculate Kp for this reaction
Use the following information to calculate the standard free energy change (AG°) and equilibrium constant (K) for the following system: CaCO3(s) = CaO(s) + CO2(g) T= 900.0 °C AH;° values (kJ/mol): CaO(s) = -634.9, CO2(g) = -393.51, CaCO3(s) =–1220.0 %3D S° values (J/mol K): CaO(s) = 110.0, CO2(g) = 213.8, CACO3(s) = 38.1 %3D %3D %3D

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