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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.15 - Chemical EquilibriumProblema 43
Capitolo 15, Problema 43

At 100°C, the equilibrium constant for the reaction COCl2(𝑔) ⇌ CO(𝑔) + Cl2(𝑔) has the value 𝐾𝑐 = 2.19×10−10. Are the following mixtures of COCl2, CO, and Cl2 at 100°C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium.
(a) [COCl2] = 2.00×10−3 M, [CO] = 3.3×10−6 M, [Cl2] = 6.62×10−6 M
(b) [COCl2] = 4.50×10−2 M, [CO] = 1.1×10−7 M, [Cl2] = 2.25×10−6 M
(c) [COCl2] = 0.0100 M, [CO] = [Cl2] = 1.48×10−6 M

Guida verificata passo dopo passo
1
Calculate the reaction quotient, Qc, using the formula Qc = \(\frac{[CO][Cl_2]}{[COCl_2]}\).
Substitute the given concentrations into the expression: Qc = \(\frac{(3.3 \times 10^{-6}\) \(\text{ M}\))(6.62 \(\times\) 10^{-6} \(\text{ M}\))}{2.00 \(\times\) 10^{-3} \(\text{ M}\)}.
Compare the calculated Qc with the given equilibrium constant Kc = 2.19 \(\times\) 10^{-10}.
If Qc < Kc, the reaction will proceed in the forward direction to reach equilibrium. If Qc > Kc, the reaction will proceed in the reverse direction.
If Qc = Kc, the system is already at equilibrium.

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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 reaction at a specific temperature. For the reaction COCl₂(g) ⇌ CO(g) + Cl₂(g), Kc = [CO][Cl₂] / [COCl₂]. A small Kc value, such as 2.19×10⁻¹⁰, indicates that at equilibrium, the concentration of reactants is much greater than that of products, suggesting the reaction favors the reactants.
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Equilibrium Constant Expressions

Reaction Quotient (Q)

The reaction quotient (Q) is calculated using the same formula as Kc but with the current concentrations of the reactants and products, regardless of whether the system is at equilibrium. By comparing Q to Kc, one can determine the direction in which the reaction will proceed to reach equilibrium. If Q < Kc, the reaction shifts to the right (toward products); if Q > Kc, it shifts to the left (toward reactants).
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Reaction Quotient Q

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 helps predict how changes in concentration, pressure, or temperature will affect the position of equilibrium in a chemical reaction, guiding the understanding of how the reaction will shift in response to the concentrations of COCl₂, CO, and Cl₂.
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Le Chatelier's Principle
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(a) If Qc > Kc, how must the reaction proceed to reach equilibrium?

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At 900 K, the following reaction has 𝐾𝑝 = 0.345: 2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?

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(b) At the start of a certain reaction, only reactants are present; no products have been formed. What is the value of Qc at this point in the reaction?

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(b) What condition must be satisfied so that Qc = Kc?

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