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

To find the equilibrium constant \( K_c \) for the phosphorylation of glucose in glycolysis given that \( \Delta G^{\circ} = 13.8 \, \text{kJ mol}^{-1} \) at \( 298 \, \text{K} \), we can follow these steps:

### Step 1: Convert \( \Delta G^{\circ} \) from kJ to J
Since the standard Gibbs free energy change is given in kilojoules, we need to convert it to joules for consistency with the gas constant \( R \).

\[ \Delta G^{\circ} = 13.8 \, \text{kJ mol}^{-1} \times 1000 \, \text{J/kJ} = 13800 \, \text{J mol}^{-1} \]
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