Calculate (a)Delta G^(@) and (b) the equilibriumconstantfor theformation of NO_(2) " from"NO and NO_(2)and O_(2) at 298 K NO (g) +1/2 O_(2) (g) hArr NO_(2) (g)whereDelta _(f) G^(@) (NO_(2)) = 52*0 "kJ//mol ", Delta_(f) G^(@) (NO) = 87*0"kJ//mol," Delta _(f) G^(@) (O_(2)) = 0 "kJ//mol.

Calculate (a)Delta G^(@) and (b) the equilibriumconstantfor theformati

1.	Calculate (a)Delta G^(@) and (b) the equilibriumconstantfor theformation of NO_(2) " from"NO and NO_(2)and O_(2) at 298 K NO (g) +1/2 O_(2) (g) hArr NO_(2) (g)whereDelta _(f) G^(@) (NO_(2)) = 520 "kJ//mol ", Delta_(f) G^(@) (NO) = 870"kJ//mol," Delta _(f) G^(@) (O_(2)) = 0 "kJ//mol.
Answer» SOLUTION :` Delta _(r) G^(@) = sum Delta _(f)G^(@) ("Products") - sumDelta_(f) G^(@)("REACTANTS") ` ` = Delta _(f) G^(@) (NO_(2)) - [Delta_(f) G^(@)(NO) +1/2 Delta_(f) G^(@)(O_(2)) ] = 520 - ( 870+1/2 xx 0) = -350 "kJ "MOL"^(-1)` (b) ` Delta G^(@)= 2303" RT log K Hence," -(-35000) = 2303 xx 8 314 xx 298 xx "log K"` or ` " log K"= 6* 1341 or K = 1* 361 xx 10^(6) `