Calculate the enthalpy change for the reaction: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) ...

Calculate the enthalpy change for the reaction:

4 Fe(s) + 3 O₂(g) → 2 Fe₂O₃(s) ΔH°_rxn = ?

where:

2 Fe(s) + 6 H₂O(ℓ) → 2 Fe(OH)₃(s) + 3 H₂(g) ΔH₁° = +321.8 kJ

2 H₂O(ℓ) → 2 H₂(g) + O₂(g) ΔH₂° = +571.7 kJ

Fe₂O₃(s) + 3 H₂O(ℓ) → 2 Fe(OH)₃(s) ΔH₃° = +288.6 kJ

Expert Solution

∆H°rxn of given equation can be calculated by using equations with known ∆H°rxn.

Answer: ∆H°rxn = -1648.7 kJ.

queen_honey_blossom answered 2 years ago

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) In the preceding reaction, _____ is...

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) In the preceding reaction, _____ is in elemental form and has a standard enthalpy of ______ . This reaction is a ______ reaction (think heat). The standard enthalpy for the reaction is _______ kJ (3 S.F.)

1) Calculate the enthalpy of reaction (ΔHrxn) for the following reaction: Fe2O3(s) + 3 CO(g) →...

1) Calculate the enthalpy of reaction (ΔHrxn) for the following reaction: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) Given: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) ΔH = –1648 kJ 2 CO2(g) → 2 CO(g) + O2(g) ΔH = +565.4 kJ 2) Use standard enthalpies of formation to calculate the standard enthalpy of reaction for the following reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔH∘rxn

Fe2O3(s) + 3 CO(g) —> 2 Fe(s) + 3 CO2(g) delta H = ___ a. Calculate...

Fe2O3(s) + 3 CO(g) —> 2 Fe(s) + 3 CO2(g) delta H = ___ a. Calculate delta H for the reaction above using the following know thermochemical reactions 2Fe(s) + 3/2 O2(g) —> Fe2O3(s) delta h=-824.2 kJ CO(g) + 1/2 O2(g) —> CO2(g) delta h=-282.7. b. Is this reaction endothermic, exothermic, or both? How do you know?

The enthalpy change is -400 kJ for reaction: 2 Al(s)+ 3/2 O2(g) ? Al2O3(s). What is...

The enthalpy change is -400 kJ for reaction: 2 Al(s)+ 3/2 O2(g) ? Al2O3(s). What is the ?H for the following reaction? 2 Al2O3(s) ? 4Al(s) + O2(g) is

9. Given the following reactions 2 Fe (s) + 3 CO2 (g)→ Fe2O3 (s) + 3...

9. Given the following reactions 2 Fe (s) + 3 CO2 (g)→ Fe2O3 (s) + 3 CO (g) ΔHorxn = +28.0 kJ 4 CO (g) + Fe3O4 (s)→ 3 Fe (s) + 4 CO2 (g) ΔHorxn = -12.5 kJ the enthalpy of the reaction (ΔHorxn) of Fe2O3 with CO 3 Fe2O3 (s) + CO (g)→ CO2 (g) + 2 Fe3O4 (s) is_______. 10. Given the following reactions N2 (g) + O2 (g)→ 2 NO (g) ΔHorxn = +180.7 kJ 2...

Consider the following (unbalanced) chemical reaction: Fe2O3(s) + C(s) → Fe(l) + CO2(g)Fe2O3(s) + C(s) →...

Consider the following (unbalanced) chemical reaction: Fe2O3(s) + C(s) → Fe(l) + CO2(g)Fe2O3(s) + C(s) → Fe(l) + CO2(g) a How many grams of carbon are needed to react with 811.21 grams of Fe22O33? b How many grams of iron can be produced from 390.955 g of carbon? c you make 487.857 grams of CO22, how many grams of Fe are produced?

4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) ΔH = -3307.9 kJ 2...

4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) ΔH = -3307.9 kJ 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔH = -1125.2 kJ 4 FeO(s) + O2(g) → 2 Fe2O3(s) ΔH = 578.2 kJ 2 Fe(s) + O2(g) → 2 FeO(s) ΔH = -544 kJ H2(g) + S(s) → H2S(g) ΔH = -20.2 kJ 2 H2(g) + O2(g) → 2 H2O(l) ΔH = 571.7 kJ By combining the above equations calculate the ΔH(formation)...

What is the enthalpy change for the reaction, W (s) + 3 H2O (g) --> WO3...

What is the enthalpy change for the reaction, W (s) + 3 H2O (g) --> WO3 (s) + 3 H2 (g) ? Given: 2 W (s) + 3 O2 (g) --> 2 WO3 (s) ΔH = – 1685.4 kJ H2 (g) + ½ O2 (g) --> H2O (g) ΔH = – 241.82 kJ

Calculate the standard enthalpy of reaction of the following: a. C2H2(g) + O2(g)  2CO(g) +...

Calculate the standard enthalpy of reaction of the following: a. C2H2(g) + O2(g)  2CO(g) + H2O(l) b. NaOH(s) + HCl(g)  NaCl(s) + H2O(l) c. H2SO4(l) + 2 NaOH(s)  Na2SO4(s) + H2O(l)

Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH...

Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ

Question