[" The enthalpy of combustion of "H_(2)(g)" at "298K" to give "H_(0)g" ) is "-249kJmol" molar concentration "],[" of "H-H" and "O=O" are "433kJmol^(-1)" and "492kJ" ,respectively.The bond bond enthalpie "],[" Latent beat of vanecenis "]

The enthalpy of combustion of H_(2(g)) to give H_(2)O_((g)) is -249 kJ mol^(-1) and bond enthalpies of H-H and O=O are 433 mol^(-1) and 492 kJ mol^(-1) respectively. The bond enthalpy of O-H is

Calculate the enthalpy of formation of water, given that the bond energies of H-H, O=O and O-H bond are 433 kJ mol^(-1), 492 kJ mol^(-1) , and 464 kJ mol^(-1) , respectively.

Calculate the enthalpy of formation of water, given that the bond energies of H-H, O=O and O-H bond are 433 kJ mol^(-1), 492 kJ mol^(-1) , and 464 kJ mol^(-1) , respectively.

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) .