Use the definition of an equilibrium constant to explain how autoprotolysis of w

Question

Use the definition of an equilibrium constant to explain how autoprotolysis of water is endothermic at 25 degrees celsius and exothermic at 300 degrees celsius.

Explanation / Answer

In autoprotolysis a proton is transferred between two identical molecules, one of which acts as a Brønsted acid, releasing a proton which is accepted by the other molecule acting as a Brønsted base. For example water undergoes autoprotolysis in the self-ionization of water reaction. H2O + H2O-->OH– + H3O+ at 25 C the equilibrium is not favourable on the products side.So the value of equilibrium constant K is less.at 300 C reaction is favourable to the products side.So the value of K is higher compared to that at 20 C(since ionization increases with temperature) ln(K)= -deltaH/RT + deltaS/R; So as k increases delta H(decreases) becomes negative at 300 C

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