The value of `DeltaG^(ɵ)` for the phosphorylation of glycose in glycolysis is `13.8 kJ mol^(-1)`. Find the value of `K_(c)` at `298 K`

Explanation

`DeltaG^(ɵ) = 13.8 kJ//"mol" = 13.8 xx 10^(3) J//"mol"`
Also, `DeltaG^(ɵ) = - RT"ln"K_(c)`
Hence, In `K_(c) = - 13.8 xx 10^(3)J//"mol"`
`(8.314 K "mol"^(-1)K^(-1) xx 298 K)`
In `K_(c) = -5.569`
`K_(c) = e^(-5.569)`
`K_(c) = 3.81 xx 10^(-3)`