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Enthalpy

If values of ...

Question

If values of $Δ H_{f}^{o}$ of $I C l (g), C l (g), I (g)$ are respectively $17.57, 121.34, 106.96$ J mol $^{- 1}$ . The value of $I - C l$ (bond energy) in J mol $^{- 1}$ is:

17.57

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210.73

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35.15

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106.96

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Solution

The correct option is A $210.73$
Gas Values of ${Δ H}_{f}$
$I C l$ $17.57$
$C l$ $121.34$
$I$ $106.96$
$I + C l \to I C l$
$(g)$ $(g)$ $(g)$
according to Hess less,
$Δ H = {Δ H}_{f}$ (reactants) $- Δ H_{f}$ (products)
$= (106.96 + 121.34) - (17.57)$
$= 210.73$ J/mol
$\Rightarrow$ Value of $I - C l$ (bond energy) in J/mol $= 210.73$ J/mol

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