Skip to main content
Pearson+ LogoPearson+ Logo
Ch.15 - Chemical Equilibrium
All textbooksBrown 15th EditionCh.15 - Chemical EquilibriumProblem 61f
Chapter 15, Problem 61f

Consider the following equilibrium, for which Δ𝐻<0
2 SO2(𝑔) + O2(𝑔) β‡Œ 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?

Verified step by step guidance
1
insert step 1> Identify the type of reaction and the effect of removing a product on the equilibrium. This is an exothermic reaction (Δ𝐻 < 0), and removing a product will shift the equilibrium to the right according to Le Chatelier's Principle.
insert step 2> Apply Le Chatelier's Principle: When a product (SO3) is removed, the system will try to counteract this change by producing more SO3.
insert step 3> Predict the shift in equilibrium: The equilibrium will shift to the right, favoring the formation of more SO3 from SO2 and O2.
insert step 4> Consider the effect on concentrations: As the equilibrium shifts to the right, the concentration of SO2 and O2 will decrease, while the concentration of SO3 will increase.
insert step 5> Conclude the effect on the system: The removal of SO3 results in the system adjusting to restore equilibrium by producing more SO3, thus shifting the equilibrium to the right.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2m
Was this helpful?

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 position of equilibrium shifts to counteract the change. In the context of the given reaction, removing SO₃ will decrease its concentration, prompting the equilibrium to shift to the right to produce more SO₃, thereby restoring balance.
Recommended video:
Guided course
07:32
Le Chatelier's Principle

Equilibrium Constant (K)

The equilibrium constant (K) quantifies 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, SOβ‚‚, and Oβ‚‚. Changes in concentration, such as the removal of SO₃, can affect the system's ability to reach a new equilibrium state.
Recommended video:
Guided course
01:14
Equilibrium Constant K

Endothermic vs. Exothermic Reactions

Reactions are classified as endothermic or exothermic based on the heat exchange with the surroundings. The given reaction is exothermic (Ξ”H < 0), meaning it releases heat. Understanding this helps predict how temperature changes might affect the equilibrium; for instance, removing a product like SO₃ can shift the equilibrium to the right, potentially releasing heat and favoring the formation of more products.
Recommended video:
Guided course
02:30
Endothermic & Exothermic Reactions
Related Practice
Textbook Question

At 373 K, 𝐾𝑝 = 0.416 for the equilibrium 2 NOBr(𝑔) β‡Œ 2 NO(𝑔) + Br2(𝑔) If the equilibrium partial pressures of NOBr(𝑔) and Br2(𝑔) are both 0.100 atm at 373 K, what is the equilibrium partial pressure of NO(𝑔)?

Textbook Question

Consider the following equilibrium, for which Δ𝐻<0

2 SO2(𝑔) + O2(𝑔) β‡Œ 2 SO3(𝑔)

(e) the total pressure of the system is increased by adding a noble gas

Textbook Question

Consider the reaction 4 NH3(𝑔) + 5 O2(𝑔) β‡Œ 4 NO(𝑔) + 6 H2O(𝑔), Δ𝐻 = βˆ’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) β‡Œ 4 NO(𝑔) + 6 H2O(𝑔), Δ𝐻 = βˆ’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

Textbook Question

Consider the reaction 4 NH3(𝑔) + 5 O2(𝑔) β‡Œ 4 NO(𝑔) + 6 H2O(𝑔), Δ𝐻 = βˆ’904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (e) add a catalyst