The average $O - H$ bond energy in $H_{2} O$ with the help of following data:
(P) $H_{2} O (l) ⟶ H_{2} O (g); ΔH = + 40 .6 kJ {mol}^{- 1}$
(Q) $2 H (g) ⟶ H_{2} (g); ΔH = - 435 .0 {kJmol}^{- 1}$
(R) $O_{2} (g) ⟶ 2 O (g); ΔH = + 489 .6 kJ {mol}^{- 1}$
(S) $2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l); ΔH = - 571 .6 kJ {mol}^{- 1}$

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$584.9 kJ {mol}^{- 1}$

$279.8 kJ {mol}^{- 1}$

$925 kJ {mol}^{- 1}$

$462.5 kJ {mol}^{- 1}$

answer is C.

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Detailed Solution

$- 571.6 = 2 \times 435 + 489.6 - 2 \times 40.6 - 4 x$

$\Rightarrow x = 462.5 kJ / {mol}^{- 1}$

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