First slide

Enthalpy of Atomisation and bond dissociation

Question

For the reaction, $2 H_{2} + O_{2} \to 2 H_{2} O,$ : ΔH = – 571kJ ; Bond energy of (H–H) = 435 kJ and (O=O) =498kJ , the average bond energy of O–H bond using the above data is

Moderate

Solution

$\begin{array}{l} {\Delta _r}(H) = \sum B{E_{reac\tan ts}} - \sum B{E_{products}}\\ - 571KJ = [2B{E_{H - H}} + B{E_{O = O}}] - [4B{E_{O - H}}]\\ - 571 = [2(435) + 498] - [4B{E_{O - H}}]\\ - 571 = 1368 - 4B{E_{O - H}}\\ B{E_{O - H}} = \frac{{1939KJ}}{4} = 484.75KJ \end{array}$

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