If enthalpy of formation of ICl (g), Cl (g) and I (g) is 17.57 , 121.34 and 106.96 J mol-1 respectively. Then bond dissociation energy of I - Cl bond is

Question

If enthalpy of formation of ICl (g), Cl (g) and I (g) is 17.57 , 121.34 and 106.96 J mol-1 respectively. Then bond dissociation energy of I - Cl bond is (A) 35.15 J mol-1 (B) 106.69 J mol-1 (C) 210.73 J mol-1 (D) 420.9 J mol-1

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/d5a4f81531cce55afbf0e6242df23b9b-.png" /> Δ H =Δ Hf( I )°+Δ Hf( Cl )°-Δ Hf( ICl )° =106.96+121.34-17.57=210.73 J mol -1

Q. If enthalpy of formation of $I C l_{(g)}, C l_{(g)}$ and $I_{(g)}$ is $17.57, 121.34$ and $106.96 J m o l^{- 1}$ respectively. Then bond dissociation energy of $I - Cl$ bond is

$35.15 J m o l^{- 1}$

$106.69 J m o l^{- 1}$

$210.73 J m o l^{- 1}$

$420.9 J m o l^{- 1}$

$Δ H = Δ H_{f (I)}^{\circ} + Δ H_{f (Cl)}^{\circ} - Δ H_{f (I Cl)}^{\circ}$ $= 106.96 + 121.34 - 17.57 = 210.73 J m o l^{- 1}$

Q. If enthalpy of formation of ICl(g)​,Cl(g)​ and I(g)​ is 17.57,121.34 and 106.96Jmol−1 respectively. Then bond dissociation energy of I−Cl bond is

35.15Jmol−1

106.69Jmol−1

210.73Jmol−1

420.9Jmol−1