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# Free Energy of Water Dissociation from Equilibrium Constant

CHEM-8JLFTN

Consider the dissociation of water.

$$\textrm{H}_2\textrm{O}(l) \rightleftharpoons \textrm{OH}^- (aq) +\textrm{H}^+(aq)$$

At $25 °C$, K is $1.00\times10^{-14}$.

What is $\Delta G°$ for this reaction?

A

$0.788 \frac{\textrm{kJ}}{\textrm{mol}}$

B

$67 \frac{\textrm{kJ}}{\textrm{mol}}$

C

$79.9\frac{\textrm{kJ}}{\textrm{mol}}$

D

$788 \frac{\textrm{kJ}}{\textrm{mol}}$

E

$79900\frac{\textrm{kJ}}{\textrm{mol}}$