Given the following reactions and their values of ΔG^∘, calculate the value of ΔGf^∘ for N2 O5(g

step 1 Again, this question is similar to the previous one. We find out the change in Gipz Free Energy

Given the following reactions and their values of ΔG^∘,...

Given the following reactions and their values of $\Delta G^{\circ}$, calculate the value of $\Delta G_{\mathrm{f}}^{\circ}$ for $\mathrm{N}_{2} \mathrm{O}_{5}(g)$ $2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) \quad \Delta G^{\circ}=-474.4 \mathrm{~kJ}$ $\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(l)$ $\Delta G^{\circ}=-37.6 \mathrm{~kJ}$ $\frac{1}{2} \mathrm{~N}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g)+\frac{1}{2} \mathrm{H}_{2}(g) \longrightarrow \mathrm{HNO}_{3}(l)$ $\Delta G^{\circ}=-79.91 \mathrm{~kJ}$

Given the following reactions and their values of $\Delta G^{\circ}$, calculate the value of $\Delta G_{\mathrm{f}}^{\circ}$ for $\mathrm{N}_{2} \mathrm{O}_{5}(g)$
$2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) \quad \Delta G^{\circ}=-474.4 \mathrm{~kJ}$
$\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(l)$
$\Delta G^{\circ}=-37.6 \mathrm{~kJ}$
$\frac{1}{2} \mathrm{~N}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g)+\frac{1}{2} \mathrm{H}_{2}(g) \longrightarrow \mathrm{HNO}_{3}(l)$
$\Delta G^{\circ}=-79.91 \mathrm{~kJ}$

Key Concepts

Calculation of Reaction Gibbs Free Energies

The additivity of free energies means that the overall Gibbs free energy change for a reaction is the sum of the standard Gibbs free energies of formation of the products minus those of the reactants. This relationship is crucial for deducing unknown thermodynamic quantities from known reaction data.

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 elements in their most stable forms under standard conditions. It serves as a fundamental reference point in thermodynamics, allowing the estimation of a compound's stability and spontaneity of formation.

Hess's Law

Hess's Law states that the total change in Gibbs free energy for a reaction is the same whether the reaction occurs in one step or through a series of intermediate steps. This principle allows us to decompose complex reactions into simpler parts, calculate their free energy changes, and then combine them to obtain the overall free energy change.

Reaction Manipulation

This concept involves the mathematical adjustment of chemical equations, including reversing, multiplying, or adding reactions, to derive a new reaction whose Gibbs free energy change can be calculated based on the known values. It is essential for using given reaction data to find unknown formation energies.

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