Using data from Appendix C , calculate ΔG^∘ for the following reactions. Indicate whether each r

step 1 In this case, we have to determine whether the reaction is spontaneous or non -spontaneous by ca

Using data from Appendix C , calculate ΔG^∘ for the...

Using data from Appendix $\mathrm{C}$ , calculate $\Delta G^{\circ}$ for the following reactions. Indicate whether each reaction is spontaneous at 298 $\mathrm{K}$ under standard conditions. (a) $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)$ (b) $\mathrm{NO}_{2}(g)+\mathrm{N}_{2} \mathrm{O}(g) \longrightarrow 3 \mathrm{NO}(g)$ (c) $6 \mathrm{Cl}_{2}(g)+2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \rightarrow 4 \mathrm{FeCl}_{3}(s)+3 \mathrm{O}_{2}(g)$ (d) $\mathrm{SO}_{2}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{S}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$

Using data from Appendix $\mathrm{C}$ , calculate $\Delta G^{\circ}$ for the following reactions. Indicate whether each reaction is spontaneous at 298 $\mathrm{K}$ under standard conditions.
(a) $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)$
(b) $\mathrm{NO}_{2}(g)+\mathrm{N}_{2} \mathrm{O}(g) \longrightarrow 3 \mathrm{NO}(g)$
(c) $6 \mathrm{Cl}_{2}(g)+2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s) \rightarrow 4 \mathrm{FeCl}_{3}(s)+3 \mathrm{O}_{2}(g)$
(d) $\mathrm{SO}_{2}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{S}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$

Key Concepts

Standard Gibbs Free Energy Change

This is the overall change in Gibbs free energy for a reaction, computed using the standard free energies of formation of the reactants and products. It is calculated by taking the sum of the standard free energies of formation of the products (each multiplied by their stoichiometric coefficients) minus the sum for the reactants, and it indicates the thermodynamic favorability of the reaction.

Standard States and Conditions

These are reference conditions, such as 298 K temperature and 1 atm pressure for gases, under which thermodynamic quantities like Gibbs free energy are defined. Standard states ensure that thermodynamic data are consistent and comparable across different reactions and studies.

Reaction Spontaneity

This concept relates to whether a chemical reaction will proceed without external intervention under standard conditions. A reaction is considered spontaneous if its standard Gibbs free energy change is negative, meaning that the process is energetically favorable.

Standard Gibbs Free Energy of Formation

This concept refers to the change in Gibbs free energy when one mole of a compound is formed from its constituent elements under standard conditions, typically 298 K and 1 atm pressure. It is a fundamental thermodynamic property that provides the basis for calculating the overall free energy change of reactions.

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