Consider the following reaction:

\[ \text{H}_2\text{O} (g) + \text{Cl}_2\text{O} (g) \rightleftharpoons 2\text{HOCl} (g) \]

At $ K_{298} = 0.090 $.

For $\text{Cl}_2\text{O} (g)$, $\Delta G_f = 97.9 \, \text{kJ/mol}$, $\Delta H = 80.3 \, \text{kJ/mol}$, and $ S = 266.1 \, \text{J/K} \cdot \text{mol}$.

Estimate $\Delta H$ and $ S^o $ for $\text{HOCl} (g)$.

To determine the thermodynamic quantities (∆H and So) for a substance in a given reaction, we need the values of these quantities for all the substances involved in the reaction. Using Hess's law for enthalpy and the formulas for entropy, we could estimate these quantities if all the required data was given.

Explanation:

To estimate the enthalpy change (∆H) for HOCl(g), we need to apply the Hess's law. But here the enthalpy (∆H) for the reaction is not given. However, we know that in a balanced chemical equation, the total energy change is equal to the sum of energy changes for each step of the reaction. If the enthalpy of product (2HOCl) and reactants (H2O and Cl2O) were given, we could have calculated it by subtracting the sum of enthalpies of reactants from the sum of enthalpies of products.

To find the standard entropy change (So) for HOCl(g), we can use the given standard entropy (S) of Cl2O(g). But we need to have the entropy of H2O (g) and 2HOCl(g).

If we have these values we can use the formula (So(products) - So(reactants)).

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