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13 Dec 2019

. One reaction involved in the conversion of iron ore to themetal is

FeO(s) + CO(g) --> Fe(s) + CO2(g)

Calculate the enthalpy change for this reaction using thefollowing reactions of iron oxides with CO.

(a) 3 Fe2O3(s) + CO(g) --> 2Fe3O4(s) + CO2(g) ?H

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Keith Leannon
Keith LeannonLv2
17 Dec 2019

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Related questions

Question 1

Iron is made from a reaction of iron oxide with carbon monoxide in the following reaction:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)

Using Hess' Law, calculate the enthalpy of reaction given:

C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ/mol

2 Fe(s) + 3/2 O2(g) → Fe2O3(s) ΔH = -824.2 kJ/mol

C(s) + 1/2 O2(g) → CO(g) ΔH = -110.5 kJ/mol

Question 2

Use Hess' Law to calculate enthalpy of reaction for the following equation:

2 N2(g) + 5 O2(g) → 2 N2O5(g)

Given:

2 H2(g) + O2(g) → 2 H2O(l) ΔH = -571.6 kJ/mol

N2O5(g) + H2O(l) → 2 HNO3(l) ΔH = -76.6 kJ/mol

1/2 N2(g) + 3/2 O2(g) + 1/2 H2(g) → HNO3(l) ΔH = -174.1 kJ/mol

Question 3

Using standard enthalpies of formation, determine the ΔHreaction for the following equations:

2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)

The carbon monoxide reduces the iron ore (in the chemical equation below, hematite) to iron, becoming carbon dioxide in the process: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

Reactant or product ΔG∘f(kJ/mol)
Fe2O3(s) -742.2
CO(g) -137.2
Fe(s) 0
CO2(g) -394.4

A) Use standard free energies of formation to determine ΔG∘rxn for this reaction at 25 ∘C.

B) Is the reaction spontaneous at standard conditions?

1)

Given the following data,

2 Fe(s) + 3/2 O2(g) => Fe2O3(s) ΔGo = -746

CO(g) + ½ O2 => CO2(g) ΔGo = -253

Find ΔGo for Fe2O3(s) + 3 CO(g) => 2 Fe(s) + 3 CO2(g)

2)

At 782 K, ΔGo equals -61 kJ for the reaction, 2 I(g) <=> I2(g)

Calculate the value of ln K for the reaction at this temperature to one decimal place.

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