How does the thermochemical equation S (s) + O2 (g) → SO2 (g), ΔH = –296 kJ, need to be modified to be used as a portion of the data needed to find the change in enthalpy for the chemical reaction 2SO2 (g) + O2 (g) → 2SO3 (g)?

2C(s) + H2(g) ---> C2H2(g)ΔH° = ??? kJ

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

+1299.5 kJ + (−787 kJ) + (−285.8 kJ) = +226.7 kJ

Explanation:

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.

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