The average S–F bond energy in $k J m o l^{- 1}$ of $S F_{6}$ is______. (Rounded off to the nearest integer)
[Given : The values of standard enthalpy of formation of $S F_{6} (g), S (g) and F (g) are 1100, 275 and 80 k J m o l^{- 1}$ respectively.]

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Solution

$S F_{6} (g) \to S (g) + 6 F (g)$

$Δ H_{reaction}^{0} = 6 \times E_{S - F} = Δ H_{f}^{0} [S (g)] + 6 \times Δ H_{f}^{0} [F (g)] - Δ H_{f}^{0} [S F_{6} (g)]$
$6 \times E_{S - F} = 275 + 6 \times 80 - (- 1100)$
$6 \times E_{S - F} = 1855$
$E_{S - F} = \frac{1855}{6}$
$E_{S - F} = 309.166 \approx 309$

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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 :

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The average S–F bond energy in kJmol–1 of SF6 is______. (Rounded off to the nearest integer) [Given : The values of standard enthalpy of formation of SF6(g), S(g) and F(g) are 1100, 275 and 80 kJ mol–1 respectively.]

SF6(g)→S(g)+6F(g) ΔH0reaction=6×ES−F=ΔH0f[S(g)]+6×ΔH0f[F(g)]−ΔH0f[SF6(g)] 6×ES−F=275+6×80−(−1100) 6×ES−F=1855 ES−F=18556 ES−F=309.166≈309

The average S–F bond energy in $k J m o l^{- 1}$ of $S F_{6}$ is______. (Rounded off to the nearest integer)
[Given : The values of standard enthalpy of formation of $S F_{6} (g), S (g) and F (g) are 1100, 275 and 80 k J m o l^{- 1}$ respectively.]