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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.15 - Chemical EquilibriumProblema 61e
Capitolo 15, Problema 61e

Consider the following equilibrium, for which Δ𝐻<0
2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)
(e) the total pressure of the system is increased by adding a noble gas

Guida verificata passo dopo passo
1
Identify the equilibrium reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g). Note that ΔH < 0 indicates the reaction is exothermic.
Understand the effect of adding a noble gas: Adding a noble gas at constant volume increases the total pressure but does not change the partial pressures of the reactants and products.
Apply Le Chatelier's Principle: Since the partial pressures remain unchanged, the position of equilibrium is not affected by the addition of a noble gas at constant volume.
Consider the effect of pressure changes: If the pressure change were due to a change in volume, the equilibrium would shift towards the side with fewer moles of gas. However, in this case, the addition of a noble gas does not affect the equilibrium position.
Conclude the analysis: The addition of a noble gas at constant volume does not shift the equilibrium position of the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g).

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Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In the context of the given reaction, increasing the total pressure by adding a noble gas does not shift the equilibrium position because the noble gas does not react with the components of the equilibrium.
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Equilibrium Constant (K)

The equilibrium constant (K) 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 provided, K is determined by the concentrations of SO3 and the reactants SO2 and O2. Changes in pressure or concentration can affect the position of equilibrium but not the value of K unless temperature changes.
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Effect of Inert Gases on Equilibrium

Inert gases, such as noble gases, do not participate in chemical reactions and do not affect the concentrations of the reactants or products in a chemical equilibrium. When an inert gas is added to a system at constant volume, it increases the total pressure but does not change the partial pressures of the reacting gases, thus having no effect on the position of equilibrium.
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For the equilibrium Br2(𝑔) + Cl2(𝑔) ⇌ 2 BrCl(𝑔) at 400 K, 𝐾𝑐 = 7.0. If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentrations of Br2, Cl2, and BrCl?

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Consider the following equilibrium, for which Δ𝐻<0

2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)

(f) How will each of the following changes affect an equilibrium mixture of the three gases: SO3(𝑔) is removed from the system?

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Consider the reaction 4 NH3(𝑔) + 5 O2(𝑔) ⇌ 4 NO(𝑔) + 6 H2O(𝑔), Δ𝐻 = −904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (d) decrease the volume of the container in which the reaction occurs

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Consider the reaction 4 NH3(𝑔) + 5 O2(𝑔) ⇌ 4 NO(𝑔) + 6 H2O(𝑔), Δ𝐻 = −904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (a) increase [NH3] (b) increase [H2O] (c) decrease [O2]

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