The standard Gibbs free energy of formation is -286.06 kJ / mol for NaI(s),-261.90 kJ / mol

Name: Problem 109, Chapter 15: Chemistry
Uploaded: 2021-07-06T23:45:47-08:00
Duration: 1 min 29 s
Channel: Anthony Han
Description: The standard Gibbs free energy of formation is -286.06 kJ / mol for NaI(s),-261.90 kJ / mol for Na^+(aq ) and -51.57 kJ / mol for I^-(aq) at 25^∘ C. Calculate ΔG^0 for the reaction NaI(s) H2 O⟶ Na^+(aq)+I^-(aq)

step 1 So here we're given information that specific reactions, sodium iodide solid, dissociates into a

Question

The standard Gibbs free energy of formation is $$ -286.06 \mathrm{~kJ} / \mathrm{mol} \text { for } \mathrm{NaI}(\mathrm{s}),-261.90 \mathrm{~kJ} / \mathrm{mol} \text { for } \mathrm{Na}^{+}(\text {aq }) $$ and $-51.57 \mathrm{~kJ} / \mathrm{mol}$ for $\mathrm{I}^{-}(\mathrm{aq})$ at $25^{\circ} \mathrm{C}$. Calculate $\Delta G^{0}$ for the reaction $$ \mathrm{NaI}(\mathrm{s}) \stackrel{\mathrm{H}_{2} \mathrm{O}}{\longrightarrow} \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq}) $$

   The standard Gibbs free energy of formation is
$$
-286.06 \mathrm{~kJ} / \mathrm{mol} \text { for } \mathrm{NaI}(\mathrm{s}),-261.90 \mathrm{~kJ} / \mathrm{mol} \text { for } \mathrm{Na}^{+}(\text {aq })
$$
and $-51.57 \mathrm{~kJ} / \mathrm{mol}$ for $\mathrm{I}^{-}(\mathrm{aq})$ at $25^{\circ} \mathrm{C}$. Calculate $\Delta G^{0}$ for
the reaction
$$
\mathrm{NaI}(\mathrm{s}) \stackrel{\mathrm{H}_{2} \mathrm{O}}{\longrightarrow} \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq})
$$

Chemistry

Kenneth W. Whitten,… 10th Edition

Chapter 15, Problem 109

Instant Answer

Solved by Expert Anthony Han

07/06/2021

Step 1

We can use these values to calculate the standard Gibbs free energy of the reaction, $\Delta G^{0}$, using the formula: $$ \Delta G^{0} = \sum G_{\text{products}} - \sum G_{\text{reactants}} $$ where $\sum G_{\text{products}}$ is the sum of the standard Gibbs free Show more…

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The standard Gibbs free energy of formation is $$ -286.06 \mathrm{~kJ} / \mathrm{mol} \text { for } \mathrm{NaI}(\mathrm{s}),-261.90 \mathrm{~kJ} / \mathrm{mol} \text { for } \mathrm{Na}^{+}(\text {aq }) $$ and $-51.57 \mathrm{~kJ} / \mathrm{mol}$ for $\mathrm{I}^{-}(\mathrm{aq})$ at $25^{\circ} \mathrm{C}$. Calculate $\Delta G^{0}$ for the reaction $$ \mathrm{NaI}(\mathrm{s}) \stackrel{\mathrm{H}_{2} \mathrm{O}}{\longrightarrow} \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq}) $$

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Key Concepts

Gibbs Free Energy Change of Reaction

This refers to the overall change in Gibbs free energy for a chemical reaction and is calculated by taking the difference between the sum of the Gibbs free energies of formation of the products and that of the reactants. A negative value indicates that under standard conditions, the reaction is spontaneous.

Thermodynamic Calculations Using Formation Energies

This concept involves using the standard Gibbs free energies of formation for the reactants and products to compute the reaction’s overall Gibbs free energy change. It is a fundamental approach in chemical thermodynamics to assess reaction feasibility and spontaneity.

Standard Gibbs Free Energy of Formation

This is the change in Gibbs free energy when one mole of a compound is formed from its elements in their standard states (typically at 1 bar pressure and 298 K). It serves as a reference point for calculating the free energy changes in chemical reactions.

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