Question

In case of

\mathrm{H}_2 \mathrm{O}

molecule, the enthalpy needed to break the two

\mathrm{O}-\mathrm{H}

bonds is not the same, i.e.

\begin{aligned} & \mathrm{H}_2 \mathrm{O}(\mathrm{g}) \longrightarrow \mathrm{H}(\mathrm{g})+\mathrm{OH(g}) ; \Delta_\mathrm{a} \mathrm{H}_1^{\mathrm{S}}=502 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \mathrm{OH}(\mathrm{g}) \longrightarrow \mathrm{H}(\mathrm{g})+\mathrm{O}(\mathrm{g}) ; \Delta_\mathrm{a} \mathrm{H}_2^{\mathrm{S}}=427 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}

What should be the mean bond enthalpy of

\mathrm{O}-\mathrm{H}

bonds in case of

\mathrm{H}_2 \mathrm{O}

molecule?

Accepted Answer

$464.5 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Answer

$75 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Answer

$-75 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Answer

$929 \mathrm{~kJ} \mathrm{~mol}^{-1}$

NEET UG CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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