Si les équilibres NH3+5 / 4 O2 ⇌NO+3 / 2 H2 O NO2 ⇌NO+1 / 2 O2 et ont respectivement pour co

step 1 I'm looking to calculate the KC for the reaction. So we have the following KC values. So we have

Si les équilibres NH3+5 / 4 O2 ⇌NO+3 / 2 H2 O NO2 ⇌NO+1 /...

Si les équilibres $$ \begin{gathered} \mathrm{NH}_3+5 / 4 \mathrm{O}_2 \rightleftharpoons \mathrm{NO}+3 / 2 \mathrm{H}_2 \mathrm{O} \\ \mathrm{NO}_2 \rightleftharpoons \mathrm{NO}+1 / 2 \mathrm{O}_2 \end{gathered} $$ et ont respectivement pour constantes d'équilibre $K_1$ et $K_2$, quelle serait l'expression, en fonction de $K_1$ et $K_2$, de la constante d'équilibre $K_3$ pour l'équilibre : $$ 2 \mathrm{NH}_3+7 / 2 \mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO}_2+3 \mathrm{H}_2 \mathrm{O} $$

Si les équilibres
$$
\begin{gathered}
\mathrm{NH}_3+5 / 4 \mathrm{O}_2 \rightleftharpoons \mathrm{NO}+3 / 2 \mathrm{H}_2 \mathrm{O} \\
\mathrm{NO}_2 \rightleftharpoons \mathrm{NO}+1 / 2 \mathrm{O}_2
\end{gathered}
$$
et
ont respectivement pour constantes d'équilibre $K_1$ et $K_2$, quelle serait l'expression, en fonction de $K_1$ et $K_2$, de la constante d'équilibre $K_3$ pour l'équilibre :
$$
2 \mathrm{NH}_3+7 / 2 \mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO}_2+3 \mathrm{H}_2 \mathrm{O}
$$

Key Concepts

Reaction Combination Principle

The reaction combination principle states that when individual reactions are algebraically added to yield an overall reaction, the equilibrium constant for the overall reaction is the product (or appropriate power/product combination) of the equilibrium constants of the individual reactions. By properly scaling and reversing reactions, one can derive the equilibrium expression and constant for a more complex reaction from known simpler equilibria.

Chemical Equilibrium

Chemical equilibrium describes the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction. At equilibrium, the concentrations of reactants and products remain constant over time, and the relationship between these concentrations is expressed using the equilibrium constant. This concept is central to understanding how different reactions balance out and how changes in conditions can shift the equilibrium position.

Reaction Stoichiometry

Reaction stoichiometry involves the use of balanced chemical equations to relate the quantities of reactants and products involved in a reaction. It provides the numerical coefficients that are critical in combining reactions, scaling them appropriately, and ensuring that mass and charge are conserved. When manipulating equilibrium constants, these stoichiometric coefficients dictate how the equilibrium expressions must be adjusted (for example, raising constants to a power when reactions are multiplied).

Equilibrium Constant Manipulation

Equilibrium constant manipulation refers to the set of mathematical operations that can be applied to the equilibrium constants when reactions are reversed, multiplied, or added together. Reversing a reaction inverts its equilibrium constant, multiplying a reaction by a coefficient raises the constant to the corresponding power, and adding reactions results in the multiplication of their equilibrium constants. This principle allows the determination of the overall equilibrium constant for a net reaction derived from simpler reactions.

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