Based on the values of B.E. given, `Delta_(f)H^(@)` of `N_(2)H_(4)` (g) is :
Given : `N-N = 159 " kJ mol"^(-1)," "H-H=436 " kJ mol"^(-1)`
`N-=N = 941" kJ mol"^(-1), " "N-H=398 " kJ mol"^(-1)`

Based on the values of B.E. given, Delta_(f)H^(0) " of " N_(2)H_(4(g)) is : Given BE of : N- N is 159 kJ mol^(-1) , H-H is 436 kJ mol^(-1), N =- N is 941 kJ mol^(-1), N-H is 398 kJ mol^(-1)

Following are the values of E_(a) and Delta H for three reactions carried out at the same temperature : I: E_(a) =20 kJ mol^(-1), Delta H =-60 kJ mol^(-1) II: E_(a) =10 kJ mol^(-1), Delta H =-20 kJ mol^(-1) III: E_(a) =40 kJ mol^(-1), Delta H=+15 kJ mol^(-1) If all the three reaction have same frequency factor then fastest and slowest reactions are :

Calculate the resonance enegry of NO_(2) ( :O-N=O: ) The measured enthalpy formation of NO_(2)(Delta_(f)H^(Theta)) is 34 kJ mol^(-1) . The bond energies given are: N -O rArr 222 kJ mol^(-1) N -= N rArr 946 kJ mol^(-1) O = O rArr 498 kJ mol^(-1) N = O rArr 607 kJ mol^(-1)

Calculate the resonance enegry of NO_(2) ( :O-N=O: ) The measured enthalpy formation of NO_(2)(Delta_(f)H^(Theta)) is 34 kJ mol^(-1) . The bond energies given are: N -O rArr 222 kJ mol^(-1) N -= N rArr 946 kJ mol^(-1) O = O rArr 498 kJ mol^(-1) N = O rArr 607 kJ mol^(-1)

For the reaction N_(2)+3X_(2) to 2NX_(3) where X=F, Cl (the average bond energies are F-F = 155 kJ "mol"^(-1) N-F = 272 kJ "mlo"^(-1) , Cl-Cl = 242 kJ "mol"^(-1) , N-Cl= 200 kJ "mol"^(-1) and N -=N = 941 kJ "mol"^(-1) ), the heats of formation of NF_(3) and NCl_(3) in kJ "mol"^(-1) , respectively, are closest to