The standard enthalpy of formation (ΔH°f) for one mole of ICl₃(g) is -88 kJ, as determined by Hess' law.
We want to determine the standard enthalpy of formation (ΔH°f) for one mole of ICl₃(g). The equation for which we are looking the enthalpy of reaction is:
0.5 I₂(s) + 1.5 Cl₂(g) ⟶ ICl₃(g)
We will use Hess' law, which states that the total enthalpy change during the complete course of a chemical reaction is independent of the number of steps taken. Let's consider the following thermochemical equations.
I₂(g) + 3 Cl₂(g) ⟶ 2 ICl₃(g) ΔH°298 = −214 kJ
I₂(s) ⟶ I₂(g) ΔH°298 = 38 kJ
We will add the reactions and their enthalpies. The resulting reaction is:
I₂(s) + 3 Cl₂(g) ⟶ 2 ICl₃(g) ΔH°298 = −-176 kJ
Finally, since we want to calculate the standard enthalpy per mole of ICl₃, we will divide the previous equation by 2.
0.5 I₂(s) + 1.5 Cl₂(g) ⟶ ICl₃(g) ΔH°298 = −88 kJ
The standard enthalpy of formation (ΔH°f) for one mole of ICl₃(g) is -88 kJ, as determined by Hess' law.
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