Textbook Question
Ammonia reacts slowly in air to produce nitrogen monoxide and water vapor:
NH3(g) + O2(g) ⇌ NO(g) + H2O(g) + Heat
Write the equilibrium equation.
1
views
15. Chemical Equilibrium
The Equilibrium Constant
3:09 minutesProblem 12
Textbook Question
Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium. Fe2O3(s) + 3 CO(g) ⇌ 2 Fe(s) + 3 CO2(g) K (at 727 °C) = 24.2
Verified step by step guidance1
Identify the equilibrium constant (K) given in the problem, which is 24.2 at 727 °C.
Understand that the equilibrium constant (K) indicates the ratio of the concentration of products to reactants at equilibrium. A K value greater than 1 suggests that products are favored.
Since K = 24.2 is greater than 1, this implies that at equilibrium, the concentration of products (Fe and CO2) is greater than the concentration of reactants (Fe2O3 and CO).
Conclude that the reaction favors the formation of products at equilibrium.
Note that the relative concentrations at equilibrium will have more products (Fe and CO2) compared to reactants (Fe2O3 and CO).
Verified video answer for a similar problem:This video solution was recommended by our tutors as helpful for the problem above
Video duration:
3mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Chemical Equilibrium
Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. At this point, the system is in a dynamic state where the concentrations do not change over time, even though both reactions continue to occur. Understanding this concept is crucial for analyzing how reactions shift in response to changes in conditions.
Recommended video:
Guided course
03:42
Chemical Equilibrium Concept 1
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. A large K value (greater than 1) indicates that products are favored at equilibrium, while a small K value (less than 1) suggests that reactants are favored. In this case, K = 24.2 implies that the formation of products is favored.
Recommended video:
Guided course
02:50The Equilibrium Constant Concept 1
Le Chatelier's Principle
Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. This principle helps predict how the concentrations of reactants and products will shift in response to external changes, providing insight into the behavior of the reaction under different conditions.
Recommended video:
Guided course
09:34The following is an endothermic reaction where Kc = 6.73 x 103.For each of the choices below predict in which direction the reaction will proceed
Related Videos
Related Practice