Chemistry

Problem

1. (a) The ionization of water has an equilibrium constant

1.00 \times 10^{-14}

at 298 K.

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

Calculate

\Delta G

for this reaction at this temperature. 2. (b) At 313 K the equilibrium constant has a value of

2.92 \times 10^{-14}

. What can you conclude about the enthalpy change,

\Delta H

, of the reaction?