The ΔG° for the reaction in kJ/mol is -17.09.
Calculation,
The reaction is given below.
[tex]ICl(g)+Cl_{2} (g)[/tex] → [tex]ICl_{3} (s)[/tex]
The ΔG° for [tex]ICl(g)[/tex] = -5.5 kJ/mol
The ΔG° for [tex]ICl_{3} (s)[/tex] = -22.59 kJ/mol
The ΔG° for [tex]Cl_{2} (g)[/tex] = 0 kJ/mol ( change in gibb's free energy of standard state )
ΔG° for the reaction = ΔG° (product) - ΔG° (reactant)
ΔG° for the reaction = -22.59 kJ/mol - ( -5.5 kJ/mol + 0 kJ/mol )
ΔG° for the reaction = -17.09 kJ/mol
The value of change standard gibb's free energy for the standard state ( most stable form of elements) is zero.
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