If `DeltaH_(f)^(@)` of `Icl(g)`, `Cl(g)` and `I(g)` is `17.57`, `121.34` and `106.96 J mol^(-1)` respectively. Then bond dissociation energy of `I-Cl` bond is

The standard enthalpies of formation of HCl(g), H(g) and Cl(g) are -92.2 , 217.7 and 121.4 kJ mol^(-1) respectively. The bond dissociation enthalpy of HCl is :

If values of Delta_(f)H^(Theta) of ICl(g),Cl(g) , and I(g) are, respectively, 17.57,121.34 , and 106.96 J mol^(-1) . The value of I-Cl (bond energy) in J mol^(-1) is

If values of DeltaH_f^@ of ICl_((g)), Cl_((g)) and I_((g)) are respectively 17.57, 121.34, 106.96 J mol^(-1) . The value of I - Cl (bond energy) in J mol^(-1) is:

If values of Delta_(f)H^(Theta) of ICI(g),CI(g) , and I(g) are, respectively, 17.57,121,34 , and 106.96 J mol^(-1) . The value of I-CI (bond energy) in J mol^(-1) is

If values of Delta_(f)H^(Theta) of ICI(g),CI(g) , and I(g) are, respectively, 17.57,121,34 , and 106.96 J mol^(-1) . The value of I-CI (bond energy) in J mol^(-1) is

H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g) DeltaH =- 242 kJ mol^(-1) Bond energy of H_(2) and O_(2) is 436 and 500 kJ mol^(-1) , respectively. What is bond energy of O-H bond?

H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g) DeltaH =- 242 kJ mol^(-1) Bond energy of H_(2) and O_(2) is 436 and 500 kJ mol^(-1) , respectively. What is bond energy of O-H bond?

The molar entropies of HI(g), H(g) and I(g) at 298 K are 206.5, 114.6, and 180.7 J mol^(-1)K^(-1) respectively. Using the DeltaG^(@) given below, calculate the bond energy of HI. HI(g)rarrH(g)+I(g)," "DeltaG^(@)=271.8 kJ

The molar entropies of HI(g), H(g) and I(g) at 298 K are 206.5, 114.6, and 180.7 J mol^(-1)K^(-1) respectively. Using the DeltaG^(@) given below, calculate the bond energy of HI. HI(g)rarrH(g)+I(g)," "DeltaG^(@)=271.8 kJ