The bond dissociation energies forCl_(2),I_(2) and ICIare 242.3,151.0 and211.3 kJ //mole respectively . The enthalpyof sublimation of iodine is62.8 kJ // mole.What is the standard enthalpy of formation ofICI(g) nearly equal to ?

The bond dissociation energies forCl_(2),I_(2) and ICIare 242.3,151.0

1.	The bond dissociation energies forCl_(2),I_(2) and ICIare 242.3,151.0 and211.3 kJ //mole respectively . The enthalpyof sublimation of iodine is62.8 kJ // mole.What is the standard enthalpy of formation ofICI(g) nearly equal to ?
Answer» `- 211.3 kJ //`MOLE `- 14.6kJ //`mole 16.8 kJ`//` mole `33.5 kJ//` mole Solution :We aim `:(1)/(2) I_(2)(s) + (1)/(2) Cl_(2) (g) RARR ICI (g) ` We are given`:` (i) `Cl_(2)(g)rarr 2Cl(g), DeltaH=242.3 kJ` (II) `I_(2)(g) rarr 2I(g),DeltaH = 151 kJ` (iii) `ICI (g) rarr (i) + Cl(g), DeltaH =211.3 kJ` (iv) `I_(2)(s) rarrI_(2)(g), DeltaH =62.8 kJ` `(1)/(2) (ii) (1)/(2) (i)- (iii) +(1)/(2) ` gives the required EQUATION with `DeltaH =(1)/(2) (151) +(1)/(2) (292.3) -211.3 + (1)/(2) (62.8) = 16.75kJ`