The value of `DeltaH_(O-H)` is `109 kcal mol^(-1)`. Then formation of one mole of water in gaseous state from `H(g)` and `O(g)` is accompanied by

The value of DeltaH_(O-H) is 109Kcal//mol . The enthalpy of formation of 1 mole of water in gaseous state will be

The bond energy of an O-H bond is109 kcal mol^(-1) . When a mole of water is formed

H_(2)(g)+1//2O_(2)(g)=H_(2)O(l) , Delta H_(298 K)=-68.32 Kcal. Heat of vapourisation of water at 1 atm and 25^(@)C is 10.52 Kcal. The standard heat of formation (in Kcal) of 1 mole of water vapour at 25^(@)C is

H_(2)(g)+1//2O_(2)(g)=H_(2)O(l) , Delta H_(298 K)=-68.32 Kcal. Heat of vapourisation of water at 1 atm and 25^(@)C is 10.52 Kcal. The standard heat of formation (in Kcal) of 1 mole of water vapour at 25^(@)C is

H_(2)(g)+1//2O_(2)(g)=H_(2)O(l) , Delta H_(298 K)=-68.32 Kcal. Heat of vapourisation of water at 1 atm and 25^(@)C is 10.52 Kcal. The standard heat of formation (in Kcal) of 1 mole of water vapour at 25^(@)C is

H_2(g)+1/2O_2(g)=H_2O(l) , triangleH_298k =-68.32 kcal. Heat of vaporisation of water at 1 atm and 25^@C is 10.52 kcal. The standard heat of formation(in kcal) of 1 mole of water vapour at 25^@C is: