The entropies of `H_(2)` (g) and H (g) are 130.6 and 114.6 J `mol^(-1)K^(-1)` respectively at 298 K. Using the data given below calculate the bond energy of `H_(2)` (in kJ/mol) :
`H_(2)(g)rarr2H(g),DeltaG^(@)=406.6kJ`

The entropies of H_(2)(g) and H(g) are 130.6 and 114.6J mol^(-1) K^(-1) respectively at 298 K. Using the data given below calculate DeltaH^(@) ( in kJ/ mol) of the reaction given below. H_(2)(g) to 2H(g) , DeltaG^(@) = 406.62 kJ//mol

The entropies of H_(2)(g) and H(g) are 60 " and " 50 J"mole"^(-1)K^(-1) respectively at 300 K. Using the data given below calcualate the bond enthalpy of H_(2)(g) in Kcal "mole"^(-1) . " "H_(2)(g) rarr 2H(g)," "DeltaG^(@)=21.6 KJ "mole"^(-1)

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

The molar entropies of HI_((g)), H_((g)) and I_((g)) at 298K 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)) rarr H_((g)) + I_((g)), DeltaG^(@) = 271.8kJ (Give your answer after divide with 49.7)

The enthalpies of formation of C_2H_2(g) and C_6H_6(g) at 298 K are 230 and 85 kJ/mol respectively. The enthalpy change for the reaction 3C_2H_2(g) to C_6H_6(g) is