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# Answer to Question #161211 in General Chemistry for neyola rebello

Question #161211

Given the following data:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)      ΔH = -26.8 kJ

FeO(s) + CO(g) → Fe(s) + CO2(g)             ΔH = -16.5 kJ

Calculate the ΔH for the reaction below:

Fe2O3(s) + CO(g) → 2 FeO(s) + CO2(g)

1
2021-02-04T07:07:41-0500

### Solution:

Given the chemical reaction:

Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)      ΔH = -26.8 kJ

FeO(s) + CO(g) → Fe(s) + CO2(g)             ΔH = -16.5 kJ

Firstly we should find the standard enthalpies of Fe2O3(s) and FeO(s) in terms of Hesss law:

"\\Delta H_{reaction}=\\Delta H_{product}-\\Delta H_{reactant}"

"\\Delta H(Fe_2O_3) = -822.2 (\\frac{kJ}{mole})"

"\\Delta H(FeO)=-264.8 (\\frac{kJ}{mole})"

Then, we put these values to the main chemical reaction:

"Fe_2O_3+CO\\rightarrow2FeO+CO_2"

Hesss law:

"\\Delta H_{reaction}=\\Delta H_{product}-\\Delta H_{reactant}"

"\\Delta H_{product}=" 2(-264.8 "(\\frac{kJ}{mole})" ) + (-393.5 "(\\frac{kJ}{mole})" )= -923.1 kJ

"\\Delta H_{reactant}=" (-822.2 "(\\frac{kJ}{mole})" ) + (-110.5 "(\\frac{kJ}{mole})" ) = -932.7 kJ

"\\Delta H_{reaction}=" (-923.1 kJ) - ( -932.7 kJ) = 9.6 kJ

"\\Delta H_{reaction}=9.6kJ"

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