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Calculate a) DeltaG^(ɵ) and b) the equil...

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

Text Solution

Verified by Experts

`Delta_(r)G^(Θ)=SigmaDelta_(f)G^(Θ)("Products")-SigmaDelta_(f)G^(Θ)("Reactants")`
`Delta_(f)G^(Θ)(NO_(2))-[SigmaDelta_(f)G^(Θ)(NO)+1/2Delta_(f)G^(@)(O_(2))]`
`=52.0-(87.0+1/2xx0)=-35.0 kJ mol^(-1)`
b. `-DeltaG^(Θ)=2.303RT log K. "Hence", -(-35000)`
`=2.303xx8.314xx298xxlog K`
or `log K=6.1341 or K=1.361xx10^(6)`
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