Important industrial processes, such as converting iron ore to iron and then to steel, involve coupling a non-spontaneous reaction, such as reducing Fe2O3 (iron ore)to metallic iron, with a spontaneous process such as the oxidation of carbon in CO to CO2:
Fe2O3 (s) + 3 CO (g) 2 Fe (s) + 3 CO2 (g)
Reagent |
ΔHºf (kJ/mol) |
ΔSº(J/mol*K) |
Fe2O3 (s) |
-824.2 |
87.4 |
CO (g) |
-110.5 |
197.7 |
Fe(s) |
0 |
27.3 |
CO2 (g) |
-393.5 |
213.8 |
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Important industrial processes, such as converting iron ore to iron and then to steel, involve coupling...
Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) - 2 Fe(s) + 3 CO2(g) AG° = -28.0 kJ P(CO) - 3.1 atm, P(CO2) - 1.7 atm Calculate Arxn at 298 K, and indicate if the reaction is more or less spontaneous under these conditions than under standard conditions? -4.5 kJ, more spontaneous than under standard conditions None of these -4.5 kJ, less spontaneous than under standard conditions -23.5 kJ, more spontaneous than under standard conditions...
025 10.0 points The following reaction occurs during the pro- duction of metallic iron: 2 Fe2O3(s) + 3 C(graphite) → 4 Fe(s) + 3 CO2(g) Calculate AH for this reaction at 25°C and 1 atm. AHf for CO2(g) = -393.51 kJ/mol, and AHf for Fe2O3(s) = -824.2 kJ/mol. 1. +430.7 kJ 2. - 430.7 kJ 3. -467.9 kJ 4. There is insufficient information to answer this question. . 5. +467.9 kJ
19. For the conversion of iron ore to iron metal, given in the equation FeOo) +CO)Fe) +C020) (a) (12 points) Calculate ΔΗ0m from the following equations 3 Fe2。3(a) +COO) → 2 Fe3O4(s) + CO2(s) Δ11 17.0 kJ/mol Fe2O3(s) + 3 COG) -+ 2 Fe(a) + 3 COag) ΔΗ,,-25.0 kJ/mol Fesos)+C)3 FeO)+Co) A +19.0 kJ/mol (b) (2 pointsa) Is this reaction endothermic or exothermic? (e) (6 pointa) What is the heat of formation in kJ/mol for FeOsgiven that Ally for FeO)...
Q2) Hematite, Fe2O3, is an important ore of iron. The free metal is obtained by reacting hematite with excess carbon monoxide, CO2, in a blast furnace. Carbon dioxide is formed in the furnace by partial combustion. The unbalanced reaction is: Fe 0; (3) + CO(g) + Fe (8) + CO2(g) How many grams of iron can be produced from placing 1.50 kg of Fe,0, in a blast furnace?
got stuck here урд 5 For Practice 7.8 Recall from Example 7.8 that mining companies extract iron from iron ore according to the following balanced equation: Fe2O3(s) + 3 CO(g) — >2 Fe(s) + 3 CO2(g) 15979 21.. In a reaction mixture containing 167 g Fe2O3 and 85.8 g CO, CO is the limiting reactant. Calculate the mass of the reactant in excess (which is Fe2O3) that remains after the reaction has gone to completion. Imol Fe2O3 1679 X issing...
→ Fe(s) + CO2(g), AGº is - 5.8 kJ and AH° is -11 kJ. Sº (J mol-? K-'); 4. For the reaction Fe(s) + CO(g) Fe (27.3), CO(197.5), CO (213.7) a) What is AS sur? [37 JK-'] b) Use AG to determine whether the reaction is spontaneous or nonspontaneous under standard conditions. Explain. c) Use AS univ to determine whether the reaction is spontaneous or nonspontaneous under standard conditions. Explain. d) What is Sº for FeO? [61 J mol-'K-']
21A. Calculate the standard free energy change, AGºat 298 K for the reaction 2COXg) + 2NO(g) -2CO(g) + N:(g) The standard free energy of formation for CO is - 137 kJ, for NO it is 87.6 kJ/mol and for CO, it is -394 kJ/mol. B. Calculate the free energy change. AG. at 298 K. given that the partial pressure of CO is 5.0 atm, that of NO is 4.0 atm, that of CO, is 3.0 atm & that of N,...
can you answe both 1 and 2 with all work 1. The Ksp for Ba(103)2 is 6.0 x 10-10 at 25°C. What is the solubility of this salt in water in grams per liter. (10 pts) 2. Iron(III) oxide can be reduced by carbon monoxide. Fe,O3(s) + 3CO(g) 2Fe(s) + 3C02(g) Use the following thermodynamic data at 298 K to determine the AGº and the equilibrium constant (Kc) at 350 K. (12 pts) Substance: Fe 0,(s) CO(g) Fe(s) CO(g) AH”...
2.Calculate the enthalpy of reaction for the following reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol ΔHfo(CO(g)) = -110.5 ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5 kJ/mol
15. (15 points) Iron for the prouction of steel is obtained by a process known as smelting, during which iron(III) oxide is reduced by carbon monoxide to yield pure iron: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g). a. What is the limiting reagent when 32.55 g Fe2O3(s) and 14.78 g CO(g) are combined? For full credit, clearly show your work.(MW Fe2O3 = 159.69 g/mol; MW CO = 28.01 g/mol) b. How many grams of Fe(s) can be...