The bond dissociation energies for `Cl_(2)`, `I_(2)` and `IC l` are `242.3`, `151.0` and `211.3 kJ//"mole"` respectively. The enthalpy of sublimation of iodine is `62.8 kJ //"mole"`. What is the standard enthalpy of formation of `ICI(g)` nearly equal toA. `-211.3 kJ//"mole"`B. `-14.6 kJ//"mole"`C. `16.8 kJ//"mole"`D. `33.5 kJ//"mole"`

The bond dissociation energies for `Cl_(2)`, `I_(2)` and `IC l` are `2

1.	The bond dissociation energies for `Cl_(2)`, `I_(2)` and `IC l` are `242.3`, `151.0` and `211.3 kJ//"mole"` respectively. The enthalpy of sublimation of iodine is `62.8 kJ //"mole"`. What is the standard enthalpy of formation of `ICI(g)` nearly equal toA. `-211.3 kJ//"mole"`B. `-14.6 kJ//"mole"`C. `16.8 kJ//"mole"`D. `33.5 kJ//"mole"`
Answer» Correct Answer - C We aim at `(1)/(2)I_(2)(s)+(1)/(2)Cl_(2)(g)toICl(g)` We are given `(i) Cl_(2)(g)to2Cl(g)`, `DeltaH=242.3 kJ` `(ii) I_(2)(g)to2I(g)`, `DeltaH=151 kJ` `(iii) Icl(g)toI(g)+Cl(g)`, `DeltaH=211.3 kJ` `(iv) I_(2)(s)toI_(2)(g)`, `DeltaH=62.8kJ` `(1)/(2)(ii)+(1)/(2)(i)-(iii)+(1)/(2)(iv)` gives the required equation `DeltaH=(1)/(2)(151)+(1)(2)(242.3)-211.3+(1)(2)(62.8)` `=16.75 kJ`

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