As the chemical equation is not qiven correctly, we can look through some other example of how to use Hess Law.
For example to calculate the enthalpy for this reaction:
2C(s) + H2(g) ---> C2H2(g)
Given the following thermochemical equations:
C2H2(g) + 5⁄2O2(g) ---> 2CO2(g) + H2O(ℓ)ΔH° = −1299.5 kJ
C(s) + O2(g) ---> CO2(g)ΔH° = −393.5 kJ
H2(g) + 1⁄2O2(g) ---> H2O(ℓ)ΔH° = −285.8 kJ
Solution:
1) Determine what we must do to the three given equations to get our target equation:
a) first eq: flip it so as to put C2H2 on the product side
b) second eq: multiply it by two to get 2C
c) third eq: do nothing. We need one H2 on the reactant side and that's what we have.
2) Rewrite all three equations with changes applied:
2CO2(g) + H2O(ℓ) ---> C2H2(g) + 5⁄2O2(g) ΔH° = +1299.5 kJ
2C(s) + 2O2(g) ---> 2CO2(g) ΔH° = −787 kJ
H2(g) + 1⁄2O2(g) ---> H2O(ℓ)ΔH° = −285.8 kJ
Notice that the ΔH values changed as well.
3) Examine what cancels:
2CO2 ⇒ first & second equation
H2O ⇒ first & third equation
5⁄2O2 ⇒ first & sum of second and third equation
4) Add up ΔH values for our answer:
+1299.5 kJ + (−787 kJ) + (−285.8 kJ) = +226.7 kJ
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