Problem: The ΔHf° for CO2 (g) is -393 kJ/mole and ΔHrxn for the reaction2CO(g) + O2(g) → 2CO2(g) is -560 kJ. The ΔHf° for CO(g) is (in kJ/mole):(a) +113 (b) -673 (c) -113 (d) -209 (e) -226

FREE Expert Solution

We’re being asked to determine the standard enthalpy change of formation (ΔH˚f) for CO(g). Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved


H°rxn =H°f, products - H°f, products


We’re given the ΔH˚rxn for the combustion of 2 moles of CO(g). The chemical equation for that reaction is:


2 CO(g) + O2(g) → 2CO2(g)


This equation is already balanced. 


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Problem Details

The ΔHf° for CO2 (g) is -393 kJ/mole and ΔHrxn for the reaction

2CO(g) + O2(g) → 2CO2(g) is -560 kJ. The ΔHf° for CO(g) is (in kJ/mole):

(a) +113 

(b) -673 

(c) -113 

(d) -209 

(e) -226

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