consider the reaction. 2 Fe2O3 ----> 4 Fe + 3 O2 ?H rxn= +824.2 kJ The...
Consider the reaction. 2 Fe,O, 4 Fe +30, AHAD +824.2 kJ The formation of 43.0 g of Fe results in the absorption of 635 kJ of heat. the release of 159 kJ of heat. the absorption of 8860 kJ of heat. the release of 635 kJ of heat. the release of 8860 kJ of heat. the absorption of 159 kJ of heat
Given that: 2Al(s)+(3/2)O2(g)--->Al2O3(s) change in H(rxn)= -1601 kJ/mol 2Fe(s)+(3/2)O2(g)--->Fe2O3(s) change in H(rxn)= -821 kJ/mol Calculate the standard enthalpy change for the following reaction: 2Al(s)+Fe2O3(s)--->2Fe(s)+Al2O3(s) _______kJ
Consider the reaction. 2 Fe 2 O 3 ⟶ 4 Fe + 3 O 2 Δ H ∘ r x n = + 824.2 k J The decomposition of 81.0 g of Fe2O3 results in.
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
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) AH = -1652 kJ (a) How much heat is released when 3.54 mol iron are reacted with excess O2? Ok] (b) How much heat is released when 1.48 mol Fe2O3 is produced? CJ) (c) How much heat is released when 2.50 g iron are reacted with excess O2? DJ (d) How much heat is released when 12.6 g Fe and 1.02 g O2 are reacted? CkJ
Based on the balanced reaction 4 Fe + 3 O2 → 2 Fe2O3, a student starts this reaction with these amounts of chemicals: 12 mol Fe, 15 mol O2, and 0 mol Fe2O3. What chemical is the limiting reactant?
You are given the following thermodynamic data. 2 Fe(s) + 3/2 O2(g) → Fe2O3(s) ΔH° = -823 kJ 3 Fe(s) + 2 O2(g) → Fe3O4(s) ΔH° = -1120. kJ Calculate the ΔH° for the following reaction. 3 Fe2O3(s) → 2 Fe3O4(s) + ½ O2(g)
Iron reacts with oxygen to form hematite in the following reaction: 2Fe(s) )Fe2O3(s) Using data from appendix 2 of the book, and assuming that heat capacities are independent of temperature, what is the reaction enthalpy at 653 K? Select one: a. +820.8 kJ b. +824.2 kJ c. -824.2 kJ d.-827.4 kJ e.-815.3 kJ f. -881.5 kJ g. -820.8 kJ h. 3410 kJ
Given the following reactions: Fe2O3(s) + 3 CO(g)2 Fe(s)+ 3 CO2(g) H=-28.0kJ 2 Fe(s) + 4 CO2(g)4 CO(g) + Fe3O4(s) H = +12.5 kJ 3 Fe2O3(s) + CO(g) ? CO2(g) + 2 Fe3O4(s) Find the enthalpy of the reaction of Fe2O3 with CO
The overall reaction in commercial heat packs can be represented as the reaction below. 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s), ΔH = -1652 kJ (a) How much heat is released when 4.23 mol iron is reacted with excess O2? (b) How much heat is released when 1.48 mol Fe2O3 is produced? c) How much heat is released when 1.34 g iron is reacted with excess O2? (d) How much heat is released when 13.10 g Fe and 2.05...