Carbon monoxide replaces oxygen in oxygenated hemoglobin according to the reaction: HbO₂(aq) + CO(aq) ⇌ HbCO(aq) + O₂(aq) a. Use the reactions and associated equilibrium constants at body temperature given here to find the equilibrium constant for the reaction just shown. Hb(aq) + O₂(aq) ⇌ HbO₂(aq) K_c = 1.8 Hb(aq) + CO(aq) ⇌ HbCO(aq) K_c = 306

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Identify the given reactions and their equilibrium constants: Reaction 1: Hb(aq) + O_2(aq) \rightleftharpoons HbO_2(aq) with K_{c1} = 1.8; Reaction 2: Hb(aq) + CO(aq) \rightleftharpoons HbCO(aq) with K_{c2} = 306.

Write the target reaction: HbO_2(aq) + CO(aq) \rightleftharpoons HbCO(aq) + O_2(aq).

Express the target reaction in terms of the given reactions: Reverse Reaction 1 to get HbO_2(aq) \rightleftharpoons Hb(aq) + O_2(aq) with K_{c1}' = \frac{1}{1.8}.

Combine the reversed Reaction 1 with Reaction 2: HbO_2(aq) + CO(aq) \rightleftharpoons Hb(aq) + O_2(aq) + Hb(aq) + CO(aq) \rightleftharpoons HbCO(aq) + O_2(aq).

Calculate the equilibrium constant for the target reaction by multiplying the equilibrium constants of the combined reactions: K_{c} = K_{c1}' \times K_{c2}.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It provides insight into the extent to which a reaction proceeds before reaching equilibrium. A larger Kc indicates a greater concentration of products compared to reactants, while a smaller Kc suggests the opposite.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle is crucial for understanding how changes in concentration, pressure, or temperature affect the position of equilibrium in a chemical reaction.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction, as described by the balanced chemical equation. It is essential for calculating the equilibrium constant and understanding how changes in the concentration of one species affect the others in the reaction, particularly in complex equilibria involving multiple reactions.

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