an equilibrium constant of special importance in much aqueous chemistry is that of the autoionization of water:

2H₂O(l) ⇋ H₃O⁺(aq) + OH⁻(aq)

The value of this equilibrium constant at three temperatures near standard temperature is

Kw(293 K) = 0.67 x 10⁻¹⁴M²
Kw(298 K) = 1.07 x 10⁻¹⁴M²
Kw(303 K) = 1.45 x 10⁻¹⁴M²

(a) Assuming that the value of ΔH° and ΔS° are constant over this narrow temperature range, determine their values (in kJ/mol and J/mol:K, respectively for the ionization equilibrium at 298 K based on this information. (Hint: You should use both the relationship between ΔGº and K, and the relationship between the Gibbs energy, enthalpy, and entropy in this problem.)