How do I calculate equilibirum constant (K)

ATP(aq)+H2O(l)--->ADP(aq)+Pi(aq)
deltaGrxn= -30.5 kJ
How do I calculate the equilirium constant for the reaction of adenosine triphosphate at 298 K?

If it's in standard conditions,

Use the equation

deltaG (not) = -RTlnKeq


Isolate Keq


-30500 J = -(8.314)(298K)(lnKeq)

Keq = e^(-30500 / (-8.314)(298K)) = 2.22 * 10^5

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