Calculate `a)` `DeltaG^(@)` and `b)` the equilibrium constant for the formation of `NO_(2)` from `NO` and `O_(2)` at `298K`
`NO(g)+1//2O_(2)(g)hArrNO_(2)(g)`
where
`Delta_(f)G^(oplus)(NO_(2))=52.0kJ//mol`
`Delta_(f)G^(oplus)(NO)=87.0kJ//mol`
`Delta_(f)G^(oplus)(O_(2))=0kJ//mol`

For the following cell reaction, Ag | Ag^(+) | AgCl | Cl^(-) | Cl_(2) , Pt Delta G_(f)^(0) (AgCl) =-109 kJ//mol Delta G_(f)^(0) (Cl ) = -129kJ//mol Delta G_(f)^(0) (Ag^(+)) = 78 kJ//mol E^@ of the cell is

Find out the value of equilibrium constant for the following reaction at 298 K. 2NH_(3(g)) + CO_(2(g)) standard Gibbs energy change, DeltaG^@ at the given temperature is - 13.6 kJ mol^(-1) .

Calculate Delta_(r)G^(theta) for conversion of oxygen to ozone (3)/(2)O_(2(g))toO_(3(g)) at 298 K. K_(p) for the reaction is 2.43xx10^(-29) .

Comment on the thermodynamics stability of NO_((g)) given that 1/2N_(2(g))+1/2O_(2(g)) to NO_(g),Delta_(r)H^(theta)=90kJmol^(-1) NO_((g))+1/2O_(2(g))to NO_(2(g)),Delta_(r)H^(theta)d=-74 Kjmol^(-1)

The bond dissociation energy depends upon the nature of the bond and nature of the molecule. If any molecule more than 1 bonds of similar nature are present then the bond energy reported is the average bond energy. Determine C-C and C-H bond enthalpy (in kJ/mol). Given: Delta_(f)H^(0) (C_(2)H_(6),g)= -85kJ//mol, Delta_(f) H^(0) (C_(3)H_(8), g)= -104kJ//mole, Delta_("sub")H^(0) (C,s)= 718kJ//mol , B.E. (H-H)= 436 kJ/mol,