Si les équilibres et 2 CO2 ⇌2 CO+O2 2 SO2+O2 ⇌2 SO3 ont respectivement pour cons

step 1 Hi, so on this given question, we are given a question and we are given four parts of it. So we

Si les équilibres et 2 CO2 ⇌2 CO+O2 2 SO2+O2...

Si les équilibres $$ \text { et } \quad \begin{aligned} & 2 \mathrm{CO}_2 \rightleftharpoons 2 \mathrm{CO}+\mathrm{O}_2 \\ & 2 \mathrm{SO}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{SO}_3 \end{aligned} $$ ont respectivement pour constantes d'équilibre $K_1$, et $K_2$, quelle serait l'expression de la constante d'équilibre $K_3$ de l'équilibre. $$ \mathrm{SO}_3+\mathrm{CO} \rightleftharpoons \mathrm{SO}_2+\mathrm{CO}_2 $$

Si les équilibres
$$
\text { et } \quad \begin{aligned}
& 2 \mathrm{CO}_2 \rightleftharpoons 2 \mathrm{CO}+\mathrm{O}_2 \\
& 2 \mathrm{SO}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{SO}_3
\end{aligned}
$$
ont respectivement pour constantes d'équilibre $K_1$, et $K_2$, quelle serait l'expression de la constante d'équilibre $K_3$ de l'équilibre.
$$
\mathrm{SO}_3+\mathrm{CO} \rightleftharpoons \mathrm{SO}_2+\mathrm{CO}_2
$$

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Key Concepts

Law of Mass Action

This principle states that at equilibrium, the ratio of the product of the concentrations (or partial pressures) of the products raised to their stoichiometric coefficients to that of the reactants raised to theirs remains constant. It is the basis for defining equilibrium constants and understanding how they are expressed for chemical reactions.

Equilibrium Constant Manipulation Rules

When chemical equations are multiplied, divided, or reversed to obtain a net reaction, their equilibrium constants are adjusted accordingly. For instance, if a reaction is multiplied by a factor, the equilibrium constant is raised to the corresponding power, if a reaction is reversed, the equilibrium constant becomes its reciprocal, and if two reactions are added, the overall equilibrium constant is the product of the individual constants.

Reaction Combination in Equilibrium

When combining multiple chemical reactions to yield a net reaction, the overall equilibrium constant can be determined by multiplying the equilibrium constants of the individual steps (taking into account any reversals or multiplications). This process is key to linking different reactions and expressing the equilibrium of a target reaction in terms of known constants.

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