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Calculate (a) DeltaG^(Theta) and (b) the...

Calculate `(a) DeltaG^(Theta)` and (b) the equilibrium constant for the formation of `NO_(2)` from NO and `O_(2)` at 298 K
`NO(g) +1//2 O_(2) (g) hArr NO_(2)(g)` where
`Delta_(f) G^(Theta) (NO_(2)) =52 .0 kJ//mol, Delta_(f) G^(Theta) (NO) =87.0 kJ//mol, Delta_(f) G^(Theta) (O_(2)) =0kJ//mol.`

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` Delta _(r) G^(@) = sum Delta _(f) G^(@) ("Products") - sum Delta_(f) G^(@) ("Reactants") `
` = Delta _(f) G^(@) (NO_(2)) - [Delta_(f) G^(@)(NO) +1/2 Delta_(f) G^(@) (O_(2)) ] = 52*0 - ( 87*0+1/2 xx 0) = -35*0 "kJ "mol"^(-1)`
(b) ` Delta G^(@) = 2*303" RT log K Hence," -(-35000) = 2*303 xx 8* 314 xx 298 xx "log K"`
or ` " log K" = 6* 1341 or K = 1* 361 xx 10^(6) `
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