(i) Assuing the reactant and product gases as ideal, show that for a gaseous reaction DeltaH=DeltaE+DeltanRT, where DeltaH and DeltaE indicate the changes of enthalpy and internal energy in the reaction. (ii) the bond energy of any diatomic molecule is defined to be the change in the internal energy for its dissociation. at 298K, O_(2)(g)to2O_(g),DeltaH=498.3kJ*mol^(-1). calculate the bond energy of O_(2) molecule R=8.314J*K^(-1)*mol^(-1).

(i) Assuing the reactant and product gases as ideal, show that for a g

1.	(i) Assuing the reactant and product gases as ideal, show that for a gaseous reaction DeltaH=DeltaE+DeltanRT, where DeltaH and DeltaE indicate the changes of enthalpy and internal energy in the reaction. (ii) the bond energy of any diatomic molecule is defined to be the change in the internal energy for its dissociation. at 298K, O_(2)(g)to2O_(g),DeltaH=498.3kJmol^(-1). calculate the bond energy of O_(2) molecule R=8.314JK^(-1)*mol^(-1).
Answer» Solution :(i) (ii) GIVEN: `O_(2)(g)to2O(g),DeltaH=498.3kJ*mol^(-1)` For the above reaction, `Deltan=2-1=1` We KNOW, `DeltaH=DeltaU+DeltanRT` `THEREFORE 498.3kJ=DeltaU+1xx8.314xx10^(-3)xx298kJ` `therefore DeltaU=495.82kJ` Therefore, bond energy of `O_(2)` molecule=495.82 kJ.