The required heat for dissociation of 1 mole `H_(2)O` into its atoms (H and oxygen) is `Delta H_("Dissociation")`. Then calculate the bond energy of O - H bond.
`H_(2)O(g)rarr O(g)+2H(g) , Delta H_("Dissociation")`

The H - O - O bond angle in H_(2)O_(2) (g) is

The H - O - O bond angle in H_(2)O_(2) (g) is

Energy required to dissociate 4 gms of H_(2)(g) into free atoms is 208 K.cals at 25^(@)C . The H-H bond energy will be

In the reaction 2H_(2)(g) + O_(2)(g) rarr 2H_(2)O (l), " "Delta H = - xkJ

In the reaction 2H_(2)(g) + O_(2)(g) rarr 2H_(2)O (l), " "Delta H = - xkJ

Energy required to dissociate 4 g of gaseous H_(2) into free gaseous atoms is 872 kJ at 25^(@)C . The bond energy of H-H bond will be

The bond dissociation energy between H-O in H2O molecule (in KJ/mol)

Dissociation of water takes place in two steps : H_(2)OrarrH+OH," "DeltaH=+497.8kJ OH rarr H+O," "DeltaH=428.5kJ Water is the bond energy of O-H bond ?

The standard molar enthalpies of formation of H_(2)O(l) " and " H_(2)O_(2)(l) are -286 and -188 "kJ"//"mol", respectively. Molar enthalpies of vaporisation of H_(2)O(l) " and "H_(2)O_(2)(l) are 44 and 53 kJ respectively. The bond dissociation enthalpy of O_(2)(g) is 498 "kJ"//"mol" . calculate the bond dissociation enthalphy ("in" "kJ"//"mol" ) of O-O bond in H_(2)O_(2) , assuming that the bond dissociation ethalpy of O-H bond is same in both H_(2) " and " H_(2)O_(2) .