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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.`

Text Solution

Verified by Experts

`NO(g)+1/2O_2(g) hArr NO_2(g)`
`DeltaG^@=Delta_fG^@(NO_2)-[Delta_fG^@(NO)+1/2Delta_fG^@(O_2)]`
`=52.0-87.0-1/2xx0=-35 "kJ mol"^(-1)`
Now log K=`-(DeltaG^@)/(2.303RT)`
`=-(-35xx10^3 "J mol"^(-1))/(2.303xx8.314 "J K"^(-1) "mol"^(-1) xx 298 K)`
=6.314
or `K=1.362xx10^6`.
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