Statement`:` `C+(1)/(2)O_(2) rarr CO, DeltaH=-26.0kcal`
`CO+(1)/(2)O_(2) rarr CO_(2), DeltaH=-68.3kcal`
`:. C+O_(2) rarr CO_(2),DeltaH=-94.3 kcal`
Explanation `:` This is an experimental proof of Hess's law.

For the reaction, C+O_(2) rarr CO_(2),DeltaH=-393 J 2Zn + O_(2) rarr 2ZnO, DeltaH=-412 J

If H_(2)S+3/2 O_(2) rarr H_(2)O+SO_(2) , DeltaH=-136.7 Kcal H_(2)+1/2 O_(2) rarr H_(2)O, DeltaH=-68.4 Kcal S+O_(2) rarr SO_(2), DeltaH=-71 Kcal What is DeltaH_(f) of H_(2)S

For the reaction, C+O_(2) rarr CO_(2),DeltaH=-393 J 2Zn + O_(2) rarr 2ZnO, H=-412 J

C(s)+O_(2)(g)toCO_(2)(g),DeltaH=-94 kcal 2CO(g)+O_(2)to2CO_(2),DeltaH=-135.2 kcal The heat of formation of CO(g) is

C(s)+O_(2)(g)toCO_(2)(g),DeltaH=-94 kcal 2CO(g)+O_(2)to2CO_(2),DeltaH=-135.2 kcal The heat of formation of CO(g) is

C+O_(2)rarr CO_(2), Delta H = -94 K.cal, CO+(1)/(2)O_(2) rarr CO_(2), Delta H = -67.7 K.cal . On the basis of the above data, the heat of formation of 'CO' is

The enthalpies for the following reactions (DeltaH^(Theta)) at 25^(@)C are given below. a. (1)/(2)H_(2)(g) +(1)/(2)O_(2)(g) rarr OH(g) DeltaH = 10.06 kcal b. H_(2)(g) rarr 2H(g), DeltaH = 104.18 kcal c. O_(2)(g) rarr 2O(g), DeltaH = 118.32 kcal Calculate the O-H bond energy in the hydroxyl radical.