If bond energy of `H_(2),F_(2)` and `HF` are in the ratio `2:1:3` and `DeltaH_(a)(H_(2))=400kJ//mol`. Then `DeltaH_(f)(HF)` is `:`

If the bond dissociation energies of XY , X_(2) and Y_(2) are in the ratio of 1:1:0.5 and DeltaH_(f) for the formation of Xy is -200 KJ//mol . The bond dissociation energy of X_(2) will be :-

If the bond dissociation energies of XY , X_(2) and Y_(2) are in the ratio of 1:1:0.5 and DeltaH_(f) for the formation of Xy is -200 KJ//mol . The bond dissociation energy of X_(2) will be :-

Given that Bond energy of H_(2) and N_(2) are 400KJmol^(-1) and 240KJmol^(-1) respectively and DeltaH_(f) of NH_(3) is -120KJmol^(-1) calculate the bond energy of N-H bond :-

Given that Bond energy of H_(2) and N_(2) are 400KJmol^(-1) and 240KJmol^(-1) respectively and DeltaH_(f) of NH_(3) is -120KJmol^(-1) calculate the bond energy of N-H bond :-

Calculate the DeltaH_(f)^@ of C_(6)H_(12)O_(6) (s) from the following data: DeltaH_(comb)[C_(6)H_(12)O_(6)(s)]=-2816.kJ//mol DeltaH_(f)^(@) of CO_(2)(g)=-393.5kJ//mol DeltaH_(f)^(@) of H_(2)O(l)=-285.9kJ//mol

Nitroglycerine (MW =227.1) denotes according to the following equation : 2C_(3)H_(5)(NO_(3))_(3)I to 3N_(2)(g)+1//2O_(2)(g)+6CO_(2)(g)+5H_(2)O(g) The standard molar enthalpies of formation, DeltaH_(f)^(@) for the compounds are given bellow: DeltaH_(f)^(@)[C_(3)H_(5)(NO_(3))_(3)]= -364 kJ//mol DeltaH_(f)^(@)[CO_(2)(g)]= -395.5 kJ//mol DeltaH_(f)^(@)[H_(2)O(g)]= -241.8 kJ//mol DeltaH_(f)^(@)[N_(2)(g)]= 0 kJ//mol DeltaH_(f)^(@)[O_(2)(g)]= 0 kJ//mol The enthalpy change when 10g of nitroglycerine is detonated is