Considering the Hess's Law, the enthalpy change for the reaction is -906.4 kJ/mol.
<h3>Hess's Law</h3>
Hess's Law indicates that the enthalpy change in a chemical reaction will be the same whether it occurs in a single stage or in several stages. That is, the sum of the ∆H of each stage of the reaction will give us a value equal to the ∆H of the reaction when it occurs in a single stage.
<h3>ΔH in this case</h3>
In this case you want to calculate the enthalpy change of:
4 NH₃ + 5 O₂ → 4 NO + 6 H₂O
which occurs in three stages.
You know the following reactions, with their corresponding enthalpies:
Equation 1: 2 N₂ + 6 H₂ → 4 NH₃ ΔH = –183.6 kJ/mol
Equation 2: 2 N₂ + 2 O₂ → 4 NO ΔH = 361.1 kJ/mol
Equation 3: 2 H₂ + O₂→ 2 H₂O ΔH = -483.7 kJ/mol
Because of the way formation reactions are defined, any chemical reaction can be written as a combination of formation reactions, some going forward and some going back.
In this case, first, to obtain the enthalpy of the desired chemical reaction you need 4 moles of NH₃ on reactant side and it is present in first equation on product side. So you need to invert the reaction, and when an equation is inverted, the sign of delta H also changes.
Now, 4 moles of NO must be a product and is present in the second equation, so let's write this as such.
Finally, you need 6 moles of H₂O on the product side, so you need to multiply by 3 the third equation to obtain the amount of water that you need. Since enthalpy is an extensive property, that is, it depends on the amount of matter present, since the equation is multiply by 3, the variation of enthalpy also.
In summary, you know that three equations with their corresponding enthalpies are:
Equation 1: 2 4 NH₃ → N₂ + 6 H₂ ΔH = 183.6 kJ/mol
Equation 2: 2 N₂ + 2 O₂ → 4 NO ΔH = 361.1 kJ/mol
Equation 3: 6 H₂ + 3 O₂→ 6 H₂O ΔH = -1,451.1 kJ/mol
Adding or canceling the reactants and products as appropriate, and adding the enthalpies algebraically, you obtain:
4 NH₃ + 5 O₂ → 4 NO + 6 H₂O ΔH= -906.4 kJ/mol
Finally, the enthalpy change for the reaction is -906.4 kJ/mol.
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