Use the standard reaction enthalpies given below to determine δh°rxn for the following reaction: 4 so3(g) → 4 s(s) + 6 o2(g) δh°rxn = ? given: so2(g) → s(s) + o2(g) δh°rxn = +296.8 kj 2 so2(g) + o2(g) → 2 so3(g) δh°rxn = -197.8 kj

The addition of the enthalpies obtained gives the enthalpy of the target reaction which is;

ΔH°rxn = 1582.8 kJ

In this scenario, we need to manipulate the equations given;

The equations given are;

The target equation is;

The first equation needs to be multiplied by 4;

so that the 4S(s) product in the target equation can be accounted for.

The second equation needs to be multiplied by 2 and multiplied by -1, so as to reverse the reactants and products.

Therefore, the reactions given become;

Ultimately, the addition of both equations yields the target equation;

Therefore, the addition of the enthalpies obtained gives the enthalpy of the target reaction.

ΔH°rxn = 1582.8 kJ

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Enthalpy is defined as the sum of internal energy. The enthalpy of a system changes continuously and is measured by its heat content. The addition of enthalpies of the given reaction is = 1582.8 kJ.

The equations and their enthalpies are given as:

To find, change in enthalpy of the equation:

Now, the equation will be multiplied by 4S to correct the reaction stoichiometrically. The second equation will be multiplied by 2 and -1.

Thus, the equation becomes:

The addition of both equation will result in:

Therefore, the enthalpy change for the given equation is 1582.8 kJ.

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