Consider the following equilibrium, for which Δ𝐻<0 2 SO 2 (𝑔) + O 2 (𝑔) ⇌ 2 SO 3 (𝑔) (e) the total pressure of the system is increased by adding a noble gas

Hello everyone today. We have the following problem. The initial and equilibrium state of the endo thermic decomposition of p gas molecules. The purple spheres to Q. Gas molecules, which are the orange spheres are illustrated in the diagram below what will happen to the number of p gas molecules if the pressure of the system is increased by adding an inert gas. So first we need to make note of the changes happening, so we are increasing the pressure. However, we are having a constant volume, so since the total pressure increased, but the individual partial pressures did not change, we're going to have no shift in the equilibrium and this is because it is an inert gas and inert gasses are non reactive. So we can conclude that the number of p gas molecules are unchanged and so with that we have answered the question overall, I hope this helped. And until next time.

Ch.15 - Chemical Equilibrium

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Brown 14th Edition

Ch.15 - Chemical Equilibrium

Problem 61e

Chapter 15, Problem 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

Verified step by step guidance

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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Key Concepts

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

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.

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.

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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At 25°C, the reaction CaCrO₄(𝑠) ⇌ Ca²⁺(𝑎𝑞) + CrO₄²⁻(𝑎𝑞) has an equilibrium constant 𝐾_𝑐= 7.1×10⁻⁴. What are the equilibrium concentrations of Ca²⁺ and CrO₄²⁻ in a saturated solution of CaCrO₄?

Textbook Question

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?

Textbook Question

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]

Textbook Question

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

Consider the following equilibrium, for which Δ𝐻<02 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)(e) the total pressure of the system is increased by adding a noble gas

Verified video answer for a similar problem:

Key Concepts

Le Chatelier's Principle

Equilibrium Constant (K)

Effect of Inert Gases on Equilibrium

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