Dissociation of water takes place in two steps- H2O - H- - OH- - H - -497-8 kJ OH- - H- - O2- - H - -428-5 kJWhat is the bond energy of O - H bond-

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Standard XII

Chemistry

Enthalpy

Dissociation ...

Question

Dissociation of water takes place in two steps:
$H_{2} O \to H^{+} + O H^{-}$ ; $Δ H$ = +497.8 kJ
$O H^{-} \to H^{+} + O^{2 -}$ ; $Δ H$ = +428.5 kJ
What is the bond energy of O - H bond?

463.15 kJ

m o l^{- 1}

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428.5 kJ

m o l^{- 1}

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69.3 kJ

m o l^{- 1}

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926.3 kJ

m o l^{- 1}

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Solution

The correct option is A 463.15 kJ $m o l^{- 1}$
In given 2 reactions, $Δ H$ is basically representing bond energies of H-O bond. So, our answer should be average of these two $Δ H$ values.
Hence, Average of two bond dissociation energies: $\frac{497.8 + 428.5}{2}$ = 463.15kJ $m o l^{- 1}$

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Similar questions

Q. Bond energies of some bonds are given below:
Cl-Cl = 242.8 kJ

m o l^{- 1}

, H-Cl = 431.8 kJ

m o l^{- 1}

,
O-H = 464 kJ

m o l^{- 1}

, O=O = 442 kJ

m o l^{- 1}

Using the B.E.s given, calculate

Δ H

for the given reaction:

2 C l_{2} + 2 H_{2} O \to 4 H C l + O_{2}

Q. 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

Q. The average O-H bond energy with the help of following data is:

(1) 2 H (g) ⟶ H_{2} (g); Δ H = - 435.0 {kJ mol}^{- 1}

(2) O_{2} (g) ⟶ 2 O (g); Δ H = + 489.6 {kJ mol}^{- 1}

(3) \frac{1}{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ O H; Δ H = - 42.09 {kJ mol}^{- 1}

Q. Using the data provided, calculate the multiple bond energy

(k J m o l^{- 1})

of a

C \equiv C

bond in

C_{2} H_{2} .

Given that the heat of formation of

C_{2} H_{2} = 225 k J m o l^{- 1} .

(take the bond energy of

C - H

bond as

350 k J m o l^{- 1}

2 C (s) \to 2 C (g) △ H = 1410 k J m o l^{- 1}

H_{2} (g) \to 2 H (g) △ H = 330 k J m o l^{- 1}

Q. 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

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Dissociation of water takes place in two steps:H2O→H++OH−; ΔH = +497.8 kJOH−→H++O2−; ΔH = +428.5 kJWhat is the bond energy of O - H bond?

The correct option is A 463.15 kJ mol−1In given 2 reactions, ΔH is basically representing bond energies of H-O bond. So, our answer should be average of these two ΔH values.Hence, Average of two bond dissociation energies: 497.8+428.52 = 463.15kJ mol−1

Dissociation of water takes place in two steps:
$H_{2} O \to H^{+} + O H^{-}$ ; $Δ H$ = +497.8 kJ
$O H^{-} \to H^{+} + O^{2 -}$ ; $Δ H$ = +428.5 kJ
What is the bond energy of O - H bond?

The correct option is A 463.15 kJ $m o l^{- 1}$
In given 2 reactions, $Δ H$ is basically representing bond energies of H-O bond. So, our answer should be average of these two $Δ H$ values.
Hence, Average of two bond dissociation energies: $\frac{497.8 + 428.5}{2}$ = 463.15kJ $m o l^{- 1}$