The standard heat of formation values of $S F_{6} (g)$ , $S (g)$ and $F (g)$ are: $- 1100, 275$ and $80 K J m o l^{- 1}$ respectively. Then the average S - F bond energy in $S F_{6}$ is:

$301 K J m o l^{- 1}$

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$- 183 K J m o l^{- 1}$

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$309 K J m o l^{- 1}$

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$280 K J m o l^{- 1}$

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Solution

The correct option is C
$309 K J m o l^{- 1}$

$S (g) + 6 F (g) \to S F_{6} (g); Δ H_{r} = - 1100 K J m o l^{- 1}$

$S (S) \to S (g); Δ H = + 275 K J m o l^{- 1}$

$\frac{1}{2} F_{2} (g) \to Δ H = 80 K J m o l^{- 1}$

Therefore heat of formation = Bond energy of reactant - Bond energy of product - $1100 = [275 + 6 \times 80] - [6 \times S - F]$

Thus bond energy of $S - F = 309 K j m o l^{- 1}$

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The standard heat of formation values of $S F_{6} (g)$ , $S (g)$ and $F (g)$ are: $- 1100, 275$ and $80 K J m o l^{- 1}$ respectively. Then the average S - F bond energy in $S F_{6}$ is:

The standard heat of formation values of $S F_{6} (g), S (g)$ and $F (g)$ are $- 1100, 275$ and $80$ J mol $^{- 1}$ respecitvely. The $S - F$ bond energy in $S F_{6}$ is :

The standard heat of formation values of $S F_{6} (g)$ , $S (g)$ and $F (g)$ are: $- 1100, 275$ and $80 K J m o l^{- 1}$ respectively. Then the average S - F bond energy in $S F_{6}$ is: