Use the equation in Exercise 71 to determine ΔH^∘ and ΔS^∘ for the autoionization of water: H2 O

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Use the equation in Exercise 71 to determine ΔH^∘ and ΔS^∘...

Use the equation in Exercise 71 to determine $\Delta H^{\circ}$ and $\Delta S^{\circ}$ for the autoionization of water:
$$\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q)$$

Key Concepts

Autoionization

Autoionization is the process through which a neutral molecule, such as a solvent, spontaneously forms ions in a reversible reaction. In the broader context of chemical thermodynamics, it demonstrates how molecular interactions and equilibrium can lead to a very small amount of ion formation even in pure substances.

Standard Enthalpy Change (?H°)

Standard enthalpy change represents the heat absorbed or released by a reaction when it is carried out under standard conditions. It provides insight into whether a reaction is endothermic or exothermic, and its sign and magnitude help predict the energy profile of the reaction and its temperature dependence.

Standard Entropy Change (?S°)

Standard entropy change quantifies the difference in disorder or randomness between the products and reactants in a chemical reaction under standard conditions. It is a key parameter in determining the spontaneity of a reaction when combined with enthalpy in the Gibbs free energy equation.

van't Hoff Equation

The van't Hoff equation establishes a quantitative relationship between the equilibrium constant of a reaction and temperature. By relating the change in logarithm of the equilibrium constant to the inverse temperature, this equation allows for the determination of the standard enthalpy change, which is crucial in studying temperature-dependent reaction behavior.

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