Questions: Consider the following reaction at 25.00 °C: Mg(OH)2(s) ⇌ Mg2+(aq) + 2 OH-(aq) Calculate ΔG^0 for the reaction. Be sure your answer has the correct number of significant digits.

Consider the following reaction at 25.00 °C:
Mg(OH)2(s) ⇌ Mg2+(aq) + 2 OH-(aq)

Calculate ΔG^0 for the reaction. Be sure your answer has the correct number of significant digits.

Transcript text: Consider the following reaction at $25.00{ }^{\circ} \mathrm{C}$ : \[ \mathrm{Mg}(\mathrm{OH})_{2}(s) \rightleftharpoons \mathrm{Mg}^{2+}(a q)+2 \mathrm{OH}^{-}(a q) \] Calculate $\Delta G^{0}$ for the reaction. Be sure your answer has the correct number of significant digits.

Solution

Solution Steps

Step 1: Identify the Standard Gibbs Free Energy Change Formula

The standard Gibbs free energy change ($\Delta G^{0}$) for a reaction can be calculated using the standard Gibbs free energies of formation ($\Delta G_f^{0}$) of the reactants and products. The formula is:

\[ \Delta G^{0} = \sum \Delta G_f^{0}(\text{products}) - \sum \Delta G_f^{0}(\text{reactants}) \]

Step 2: Gather Standard Gibbs Free Energies of Formation

We need the standard Gibbs free energies of formation for each species involved in the reaction:

\[ \mathrm{Mg(OH)_2(s)}, \quad \mathrm{Mg^{2+}(aq)}, \quad \text{and} \quad \mathrm{OH^{-}(aq)} \]

From standard tables, we have: