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 298K are 206.5

1.	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)
Answer» 282.4 298.3 290.1 315.4 Solution :`HI RARR H + I` `Delta S^(0) = S_(P) - S_(R ) = (114.6 + 180.7) - (206.5) = 88.8` `Delta G^(0) = Delta H^(0) - T Delta S^(0) = 271.8` `rArr Delta H^(0) = 271.8 + (298)/(1000) xx (88.8) = 298.3`