The enthalpie...

Question

The enthalpies of formation of $O H (g)$ , $H (g)$ and $O (g)$ are 21 $k J m o l^{- 1}$ , 109 $k J m o l^{- 1}$ and 124 $k J m o l^{- 1} .$ The value of bond enthalpy $O - H$ is

424 k J m o l^{- 1}

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212 k J m o l^{- 1}

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- 424 k J m o l^{- 1}

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- 212 k J m o l^{- 1}

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Solution

The correct option is B $212 k J m o l^{- 1}$
The enthalpy of formations of the given gases are :
$△_{f} H (H, g) = 109 k J m o l^{- 1}$
$△_{f} H (O, g) = 124 k J m o l^{- 1}$
$△_{f} H (O H, g) = 21 k J m o l^{- 1}$
We have to calculate $△ H$ for the equation,
$O H (g) \to H (g) + O (g)$
$△ H = △_{f} H (H, g) + △_{f} H (O, g) - △_{f} H (O H, g)$
$△ H = (109 + 124 - 21) k J m o l^{- 1} △ H = 212 k J m o l^{- 1}$

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Similar questions

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Standard XII Chemistry

The enthalpies of formation of OH(g), H(g) and O(g) are 21 kJ mol−1, 109 kJ mol−1and 124 kJ mol−1. The value of bond enthalpy O−H is

The enthalpies of formation of $O H (g)$ , $H (g)$ and $O (g)$ are 21 $k J m o l^{- 1}$ , 109 $k J m o l^{- 1}$ and 124 $k J m o l^{- 1} .$ The value of bond enthalpy $O - H$ is