The value of `DeltaG^(@)`for the phosphorylation of glucose in glycolysis is `15KJ//mol`. Find the value of `K_(eq) "at" 300 K`.

Explanation

To find the equilibrium constant \( K_{eq} \) for the phosphorylation of glucose in glycolysis, given that \( \Delta G^\circ = 15 \, \text{kJ/mol} \) at \( 300 \, \text{K} \), we can follow these steps:

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

\[ \Delta G^\circ = 15 \, \text{kJ/mol} = 15 \times 10^3 \, \text{J/mol} = 15000 \, \text{J/mol} \]
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