Given the following, 4 NO(g) ⟶ 2 N2O(g)+O2(g) 2 NO(g)+O2(g) ⟶ 2 NO2(g) Δ G^∘=-1

step 1 To calculate the standard delta H for this reaction, we'll use Hess's law. All we need to do is

Given the following, 4 NO(g) ⟶ 2 N2O(g)+O2(g) 2...

Given the following, $$ \begin{array}{l} 4 \mathrm{NO}(g) \longrightarrow 2 \mathrm{~N}_{2} \mathrm{O}(g)+\mathrm{O}_{2}(g) \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \\ \Delta G^{\circ}=-139.56 \mathrm{~kJ} \\ \Delta G^{\circ}=-69.70 \mathrm{~kJ} \end{array} $$ calculate $\Delta G^{\circ}$ for the reaction $$ 2 \mathrm{~N}_{2} \mathrm{O}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}_{2}(g) $$

Given the following,
$$
\begin{array}{l}
4 \mathrm{NO}(g) \longrightarrow 2 \mathrm{~N}_{2} \mathrm{O}(g)+\mathrm{O}_{2}(g) \\
2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \\
\Delta G^{\circ}=-139.56 \mathrm{~kJ} \\
\Delta G^{\circ}=-69.70 \mathrm{~kJ}
\end{array}
$$
calculate $\Delta G^{\circ}$ for the reaction
$$
2 \mathrm{~N}_{2} \mathrm{O}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}_{2}(g)
$$

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Key Concepts

Hess's Law

Hess's Law states that the total Gibbs free energy change for a reaction is independent of the pathway taken, meaning that ?G is additive for a series of reactions that sum to an overall reaction. This property allows the calculation of an unknown ?G by combining known reactions with their respective Gibbs free energy changes.

Reaction Stoichiometry

Reaction Stoichiometry involves the quantitative relationship among reactants and products in a chemical reaction. By appropriately scaling and combining reactions according to their stoichiometric coefficients, one can construct an overall balanced reaction and calculate its thermodynamic properties, such as the total Gibbs free energy change.

Gibbs Free Energy

Gibbs Free Energy (?G) is a state function that indicates the spontaneity of a chemical reaction at constant temperature and pressure. It combines the system’s enthalpy and entropy to predict whether a reaction will occur without needing external energy. A negative ?G indicates a spontaneous process, while a positive ?G indicates non-spontaneity.

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