Final answer:
The ∆G of the reaction ICI(g) + Cl₂(g) → ICl₃(s) is calculated using the standard free energies of formation for the reactants and products, resulting in a ∆G of -17.09 kJ/mol.
Step-by-step explanation:
To find the ∆G of the reaction ICI(g) + Cl₂(g) → ICl₃(s), we need to use the standard free energies of formation (∆G°f) for the reactants and products. The formula for calculating ∆G of a reaction is:
∆G = ∆G°f(products) - ∆G°f(reactants)
According to the question, the ∆G°f for ICI(g) is -5.5 kJ/mol and for ICl₃(s) is -22.59 kJ/mol. Since we have one mole of ICI and ICl₃ each, we can simply plug these values into the formula:
∆G = (-22.59 kJ/mol) - (-5.5 kJ/mol)
∆G = -22.59 kJ/mol + 5.5 kJ/mol
∆G = -17.09 kJ/mol
Therefore, the ∆G of the reaction is -17.09 kJ/mol, indicating that the reaction is spontaneous under standard conditions.