Why is the Fe-Fe3-C phase diagram a metastable phase diagram instead of a true equilibrium phase diagram? (b) Define the following phases that exist in the Fe-Fe3-C phase diagram: (i) austenite, (ii) ferrite, (iii) cementite, (iv) ferrite.
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Why is the Fe-Fe3-C phase diagram a metastable phase diagram instead of a true equilibrium phase diagram? (b) Define the following phases that exist in the Fe-Fe3-C phase diagram: (i) austenite, (ii) ferrite, (iii) cementite, (iv) ferrite.
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- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).Consider the equilibrium 21(8) — 12(8) Calculate the standard change in enthalpy, AH AH = 62.25 kJ/mol for l₂(g) and AH, 106.6 kJ/mol for I(g).4.
- 2 Zn*2 (aq) +Fe*2 (ag) + 6 CN (ag) = Zn2Fe(CN)6 (5) [znz Fe (CN),] A certain equilibrium reaction has K = 2.8 x 10-13 at 25 °C. What is the change in Gibbs Free Energy (kJ/mole) under these conditions?The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0947. A vessel is charged with PCl5 giving an initial pressure of 0.223 atm and yields PCl3 and Cl2. At equilibrium, what is the the partial pressure of each component?Given the equilibrium constants for the following reactions what is the equilibrium constant K. for the reaction 2 Cu (s) + O2 (g) 2 CuO (s)? 4 Cu (s) +O2 (g) 2 Cu20(s) K1 = 6.29 x 104 2 CuO (s) Cu,0(s) + ½ 02 (g) K2 = 17.3
- The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O OGIVEN: Compare the solubility of ferrihydrite (Fe(OH)3) and goethite (FeOOH). Dissolution Reactions: (A) Fe(OH)3 3 H+ à Fe3+ + 3 H2O with Ksp = 8.8 x 10^4 ΔGr = -28 KJ/mol (B) FeOOH + 3 H+ à Fe3+ + 2 H2O with Ksp = 8.8 x 10^-2 ΔGr = 6 KJ/mol ΔGo (KJ/mol): Fe(OH)3 = -692 FeOOH = -489 H+ = 0 Fe3+ = -9 H2O = -237 QUESTION: How much Fe3+ from ferrihydrite would dissolve at pH 2 and 7? How much Fe3+ from goethite would dissolve at pH 2 and 7?Consider the insoluble compound iron(II) sulfide , FeS . The iron(II) ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of FeS (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.For Fe(CN)64- , Kf = 7.7×1036 . Be sure to specify states such as (aq) or (s). + + K =
- In a blast furnace, carbon monoxide (CO) is used to reduce ferric oxide (Fe2O3) to metallic iron, with carbon dioxide as a by-product. The equilibrium constant Kc for the redox reaction is 19.9 at 1000 K. If the equilibrium pressure of CO2 is 2.4 atm, how much pressure is exerted by CO? Fe₂O3 (s)+3CO(g) ⇌ 2Fe(s)+3CO2 (g)What effect will adding CO2(g) have on this: CO2(g) + C(solid graphite) <=> 2 CO(g). The equilibrium constant will increase. The reaction will shift to the right in the direction of products. The reaction will shift to the left in the direction of reactants.Consider the reaction: H2(8) + I½(8) ==2 HI(g) The following data show the equilibrium constant for this reac- tion measured at several different temperatures. Use the data to find AHan and ASn for the reaction. Temperature K, 150 K 1.4 x 10- 175 K 4.6 x 10 200 K 3.6 x 10-2 225 K 1.1 250 K 15.5