Since , From the stoichiometric coefficients , Decomposition of 8 moles of Fe2O3 requires 2224 kJ energy.
So, Decomposition of 12 moles of Fe2O3 will require ;
Energy required= (2224/8) x 12
= 3336 kJ
So option " d " is the correct answer.
8 Fe2O3 (s) 16 FeO (s) + 8 02 (g) If the reaction shown below requires...
Calculate H for this reaction: FeO(s) + CO(g) Fe(s) + CO2(g) Given: Fe2O3(S) + CO(g) 2FeO(s) + CO2(g) H= +38 kJ Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g) H= -28 kJ
Consider the reaction: FeO (s) + Fe (s) + O2(g) → Fe2O3 (s) Given the following table of thermodynamic data at 298 K: Substance ΔHf° (kJ/mol) S° (J/K⋅mol) FeO (s) -271.9 60.75 Fe (s) 0 27.15 O2 (g) 0 205.0 Fe2O3 (s) -822.16 89.96 The value K for the reaction at 25 °C is ________. A.370 B.7.1 x 1085 C.3.8 x 10-14 D.5.9 x 104 E.8.1 x 1019
15. Determine the standard enthalpy of formation of Fe2O3(s), 2Fe(s) + 1.5 02 (g) → Fe2O3(s) given the thermochemical equations below. (4 points) AFH° = +160.9 kJ/mol-rxn Fe(s) + 3 H20(8) - Fe(OH)3(s) + 3/2 H (9) H2(g) + 1/2 O2(g) → H2O(6) Fe2O3(s) + 3 H2O(0) - 2 Fe(OH)3(8) A-H° = -285.8 kJ/mol-rxn A,Hº = +288.6 kJ/mol-rxn
How much energy is evolved during the formation of 197 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ A. 964 kJ B. 1.52 x 103 kJ C. 3.02 x 103 kJ D. 482 kJ E. 8.40 x 103 kJ
How much energy is evolved during the reaction of 53.4 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe,Og(s) + 2 Al(s) + AlzO3(s) + 2 Fe(s) AHnx = -852 kJ 53.4 kJ O 843 kJ 430 kJ 1686 kJ 215 kJ Using the following equation for the combustion of octane, calculate the heat of reaction for 400.0 g of octane. The molar mass of octane is 114.33 g/mole 2 CH + 25 02...
please help with these Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.37 moles of Fe2O3() react at standard conditions. AS system JK 2CO(g) + O2(g) +2CO2(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.54 moles of CO(g) react at standard conditions. AS system JK 2NH3(g) + 3N20(g)— 4N2(g) + 3H2O(g) AH = -879.5 kJ and AS° = 288.1 J/K The...
2 P2S5(s) +16 H2O (l) -> 4 H3PO4 (aq) + 10 H2S (g) H2S production reaction Fe2O3 + 3 H2S -> Fe2S3 +3 H2O H2S neutralizing reaction In the above production reaction, if the pH is 5 ( of the H3PO4 solution) how many moles of H2S would be present? How many moles of Fe2O3 would thus be required to neutralize this many moles of H2S at ph 5?
How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s), ΔH°rxn = -852 kJ
ΔGr for the reaction Fe2O3(s) + 3 H2(g) ⇌ 2 Fe(s) + 3 H2O(g) is 45.0 kJ/mol when there is 1.5 mols Fe2O3, 0.75 mols H2, and 0.15 mols Fe in a 1.0 L flask at 25.0 oC. What is the concentration of H2O in the flask? (Hint: ΔfGo values are available below the periodic table at the end of the exam.) a. 0.15 M b. 0.67 M c. 0.26 M d. 0.75 M e. 0.030M
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...