In the following process,
`H_(2)(g) to 2H(g), " "Delta_(H-H)H^(ө)=435.0" kJ "mol^(-1)` the enthalpy change involved is the

Calculate the C-C bond enthalpy from the following data : 2C("graphite") + 3H_(2)(g), to C_(2)H_(6)(g) Delta_(r)H^(@) = -84.67mkJ C("graphite"), to C(g) Delta_(r)H^(@) = 716.7kJ H_(2)(g), to 2H(g) Delta_(r)H^(@) = 435.9 kJ Assume 416 kJ as the C-H bond enthalpy.

The average O-H Bond energy in H_(2)O with the help of following data : (P) H_(2)O(l)toH_(2)O(g)," "DeltaH=+40.6 kJ mol^(-1) (Q) 2H(g)toH_(2)(g)," "DeltaH=-435.0 kJ mol^(-1) (R ) O_(2)(g)to2O(g)," "DeltaH=+489.6 kJ mol^(-1) (S) 2H_(2)(g)+O_(2)(g)to2H_(2)O(l), " "DeltaH=-571.6 kJ mol^(-1)

The enthalpy change (DeltaH) for the process, N_(2)H_(4)(g)to 2N(g)+4H(g) is is 1724 kJ mol^(-1) . If the bond energy of N-H bond in ammonia is 391 kJ mol^(-1) , what is the bond energy for N-N bond in N_(2)H_(4) ?

The enthalpy change (DeltaH) for the process, N_(2)H_(4)(g)to 2N(g)+4H(g) is is 1724 kJ mol^(-1) . If the bond energy of N-H bond in ammonia is 391 kJ mol^(-1) , what is the bond energy for N-N bond in N_(2)H_(4) ?

Calculate the standard enthalpy of formation of CH_3OH_((l)) from the following data : (i) CH_3OH_((l)) +3//2 O_(2(g)) to CO_(2(g)) + 2H_2O_((l)) , Delta_r H^(Ө)=-726 "kJ mol"^(-1) (ii) C_((s)) + O_(2(g)) to CO_(2(g)) , Delta_c H^(Ө)=-393 "kJ mol"^(-1) (iii) H_(2(g)) +1//2O_(2(g)) to H_2O_((l)) , Delta_f H^(Ө)=-286 "kJ mol"^(-1)

Given that (at 25^(@)C) : (1)/(2)H_(2)(g)+(1)/(2)O_(2)(g) to OH(g), Delta H^(0)= 38.95 " kJ mol"^(-1) H_(2)(g)+(1)/(2)O_(2)(g) to H_(2)O (g), Delta H^(0) = -241.8 " kJ mol"^(-1) H_(2)(g) to 2H(g), Delta H^(0)= 436.0 " kJ mol"^(-1) O_(2)(g) to 2O (g), Delta H^(0)= 498.3 " kJ mol"^(-1) Calculate Delta H^(0) for the following reaction - (a) OH(g) to H(g)+O(g) (b) H_(2)O(g) to 2H(g)+O(g)

Delta H_(1)^(@) for CO_(2)(g) , CO(g) and H_(2)O(g) are -393.5,-110.5 and -241.8 kJ mol^(-1) respectively. Standard enthalpy change for the reacion CO_(2)(g)+H_(2)(g) rarr CO(g) + H_(2)O(g) is