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Use bond energy to estimate DeltaH for t...

Use bond energy to estimate `DeltaH` for this rection:
`H_(2)(g)+O_(2)(g)to H_(2)O_(2)(g)`
`{:(Bond,"BondEnergy"),(H-H,436 KJ mol^(-1)),(O-O,142 KJ mol^(-1)),(O=O,499 KJ mol^(-1)),(H-O,460Kj .mol^(-1)):}`

A

`-127KJ`

B

`-209KJ `

C

`-484KJ `

D

`-841 Kj`

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The correct Answer is:
a
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Bond energies can be obtained by using the following relation: DeltaH (reaction) = sum Bond energy of bonds, broken in the reactants -sum Bond energy fo bonds, formed in the products Bond enegry depends on three factors: a. Greater is the bond length, lesser is the bond enegry. b. Bond energy increases with the bond multiplicity. c. Bond enegry increases with electronegativity difference between the bonding atoms. Use the bond enegries to estimate DeltaH for this reaction: H_(2)(g) +O_(2)(g) rarr H_(2)O_(2)(g) {:("Bond","Bond energy"),(H-H,436 kJ mol^(-1)),(O-O,142 kJ mol^(-1)),(O=O, 499kJ mol^(-1)),(H-O,460kJ mol^(-1)):}

Calculate DeltaH for the reaction H_(2)(g)+1//2O_(2)(g)toH_(2)O(g) given the bond energies of H-H and O=O bonds and O-H bond are 433 kJ mol^(-1) , 492 kJ mol^(-1) and 464kJ" "mol^(-1) .

Calculate the heat of combustion of eithene CH_(2) = CH_(2)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(I) The bond energy data are given below C = C = 619 kJ mol^(-1) C - H = 414 kJ mol^(-1) O = O = 499 kJ mol^(-1) C = O = 724 kJ mol^(-1) O - H = 460 kJ mol^(-1)

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The average O-H Bond energy in H_(2)O with the help of following data : (P) H_(2)O(l)toH_(2)O(g)," "DeltaH=+40.6 kJ mol^(-1) (Q) 2H(g)toH_(2)(g)," "DeltaH=-435.0 kJ mol^(-1) (R ) O_(2)(g)to2O(g)," "DeltaH=+489.6 kJ mol^(-1) (S) 2H_(2)(g)+O_(2)(g)to2H_(2)O(l), " "DeltaH=-571.6 kJ mol^(-1)

Calculate the standard enthalpy change (in kJ "mol"^(-1) ) for the reaction H_(2)(g)+O_(2)(g)toH_(2)O_(2)(g) , given that bond enthalpy of H-H, O=O,O-H and O-O (in kJ "mol"^(-1) ) are respectively 438, 498, 464 and 138.

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