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 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 114.6 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 114.6 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 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 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

Compute the value of DeltaS at 298K for the reaction, H_(2)(g)+1//2O_(2)(g)toH_(2)O(g) given that, DeltaG=-228.6kJ and DeltaH=-241.8kJ