Gen Chem II Le Chateliers Principle
33 flashcards covering Gen Chem II Le Chateliers Principle for the GENERAL-CHEMISTRY-2 Gen Chem II Topics section.
Le Chatelier's Principle is a fundamental concept in General Chemistry II that describes how a system at equilibrium responds to changes in concentration, temperature, or pressure. Defined by the American Chemical Society's guidelines for chemistry education, this principle helps predict the direction in which a chemical reaction will shift to re-establish equilibrium when disturbed.
On practice exams and competency assessments, questions about Le Chatelier's Principle often involve predicting the effects of specific changes on equilibrium concentrations or shifts in reaction direction. Common traps include misinterpreting the effects of temperature changes on exothermic versus endothermic reactions or overlooking the role of inert gases in pressure changes. A frequent pitfall is failing to recognize that adding a reactant or product shifts the equilibrium position, while removing one has the opposite effect.
A practical tip to keep in mind is to always consider the entire equilibrium system when evaluating changes, rather than focusing on isolated components.
Terms (33)
- 01
What does Le Chatelier's Principle state?
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 (Zumdahl, Chemical Equilibrium chapter).
- 02
How does increasing the concentration of reactants affect equilibrium?
Increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products (Brown and LeMay, Chemical Equilibrium chapter).
- 03
What happens to equilibrium when the temperature is increased in an exothermic reaction?
Increasing the temperature of an exothermic reaction will shift the equilibrium position to the left, favoring the reactants (Tro, Chemical Equilibrium chapter).
- 04
How can pressure changes affect gaseous equilibria?
Increasing the pressure in a gaseous equilibrium will shift the equilibrium position toward the side with fewer moles of gas (Zumdahl, Le Chatelier's Principle chapter).
- 05
What is the effect of adding an inert gas to a reaction at equilibrium?
Adding an inert gas at constant volume does not affect the equilibrium position because it does not change the partial pressures of the reactants and products (Brown and LeMay, Chemical Equilibrium chapter).
- 06
When a system at equilibrium is disturbed, what is the first step in predicting the shift?
The first step is to identify the type of disturbance (change in concentration, temperature, or pressure) and determine how it affects the equilibrium position (Tro, Le Chatelier's Principle chapter).
- 07
What is the effect of decreasing the volume of a gaseous equilibrium?
Decreasing the volume of a gaseous equilibrium increases the pressure, which will shift the equilibrium toward the side with fewer moles of gas (Zumdahl, Chemical Equilibrium chapter).
- 08
How does Le Chatelier's Principle apply to temperature changes?
Le Chatelier's Principle indicates that for an endothermic reaction, increasing temperature shifts the equilibrium to the right, while decreasing temperature shifts it to the left (Brown and LeMay, Chemical Equilibrium chapter).
- 09
What happens to equilibrium when a catalyst is added?
Adding a catalyst does not affect the position of equilibrium; it only speeds up the rate at which equilibrium is reached (Tro, Chemical Equilibrium chapter).
- 10
In a reaction at equilibrium, what does a shift to the right indicate?
A shift to the right indicates that the formation of products is favored (Brown and LeMay, Chemical Equilibrium chapter).
- 11
What is the impact of removing a product from an equilibrium mixture?
Removing a product will shift the equilibrium to the right, favoring the formation of more products (Zumdahl, Le Chatelier's Principle chapter).
- 12
How does the addition of a reactant affect equilibrium?
Adding a reactant will shift the equilibrium position to the right, favoring the formation of products (Tro, Chemical Equilibrium chapter).
- 13
What is the role of temperature in exothermic reactions according to Le Chatelier's Principle?
In exothermic reactions, increasing temperature shifts the equilibrium to the left, favoring reactants, while decreasing temperature shifts it to the right, favoring products (Brown and LeMay, Chemical Equilibrium chapter).
- 14
What occurs when a system at equilibrium is subjected to a change in pressure?
A change in pressure will shift the equilibrium toward the side with fewer moles of gas (Zumdahl, Le Chatelier's Principle chapter).
- 15
How does dilution affect a reaction at equilibrium?
Dilution decreases the concentration of all species in the reaction, which can shift the equilibrium position depending on the number of moles of reactants and products (Tro, Chemical Equilibrium chapter).
- 16
What is the effect of increasing the temperature on an endothermic reaction?
Increasing the temperature of an endothermic reaction shifts the equilibrium position to the right, favoring the formation of products (Brown and LeMay, Chemical Equilibrium chapter).
- 17
When a reaction is at equilibrium, how does the system respond to a change?
The system will respond by shifting the equilibrium position to counteract the change, according to Le Chatelier's Principle (Zumdahl, Le Chatelier's Principle chapter).
- 18
What is the relationship between equilibrium constants and temperature?
The equilibrium constant (K) is temperature-dependent; changing the temperature will change the value of K (Tro, Chemical Equilibrium chapter).
- 19
How does the addition of a common ion affect equilibrium?
The addition of a common ion will shift the equilibrium position to the left, favoring the formation of reactants (Brown and LeMay, Chemical Equilibrium chapter).
- 20
What is the effect of decreasing the concentration of reactants on equilibrium?
Decreasing the concentration of reactants will shift the equilibrium position to the left, favoring the formation of reactants (Tro, Chemical Equilibrium chapter).
- 21
How does Le Chatelier's Principle explain the behavior of a saturated solution?
In a saturated solution, if more solute is added, the equilibrium shifts to favor the undissolved solute, maintaining saturation (Zumdahl, Le Chatelier's Principle chapter).
- 22
What happens to equilibrium when a reactant is added to a system?
Adding a reactant shifts the equilibrium to the right, favoring the production of products (Brown and LeMay, Chemical Equilibrium chapter).
- 23
How does pressure affect the equilibrium of a reaction with unequal moles of gas?
Increasing pressure shifts the equilibrium toward the side with fewer moles of gas, while decreasing pressure shifts it toward the side with more moles (Tro, Chemical Equilibrium chapter).
- 24
What is the effect of temperature on the equilibrium constant for an exothermic reaction?
For an exothermic reaction, increasing temperature decreases the equilibrium constant (K) (Brown and LeMay, Chemical Equilibrium chapter).
- 25
How does Le Chatelier's Principle apply to industrial processes?
Le Chatelier's Principle is used in industrial processes to optimize conditions for maximum yield of products by manipulating concentration, pressure, and temperature (Tro, Chemical Equilibrium chapter).
- 26
What is the significance of the equilibrium constant (K) in relation to Le Chatelier's Principle?
The equilibrium constant (K) quantifies the ratio of products to reactants at equilibrium, and shifts in equilibrium will alter the value of K (Brown and LeMay, Chemical Equilibrium chapter).
- 27
What is the effect of temperature on an exothermic reaction according to Le Chatelier's Principle?
Increasing temperature in an exothermic reaction shifts the equilibrium to the left, favoring reactants (Zumdahl, Le Chatelier's Principle chapter).
- 28
How does the addition of a product affect the equilibrium position?
Adding a product shifts the equilibrium to the left, favoring the formation of reactants (Tro, Chemical Equilibrium chapter).
- 29
What is the effect of a catalyst on the equilibrium of a reaction?
A catalyst speeds up the rate of reaching equilibrium but does not change the position of the equilibrium (Brown and LeMay, Chemical Equilibrium chapter).
- 30
What is the impact of increasing the pressure on a reaction with equal moles of gas?
Increasing the pressure has no effect on the equilibrium position if the number of moles of gas on both sides is equal (Tro, Chemical Equilibrium chapter).
- 31
How does Le Chatelier's Principle explain the behavior of a system at equilibrium?
Le Chatelier's Principle explains that a system at equilibrium will adjust to minimize the effect of changes in concentration, temperature, or pressure (Zumdahl, Le Chatelier's Principle chapter).
- 32
What is the relationship between concentration changes and equilibrium shifts?
Changes in concentration of reactants or products will shift the equilibrium position to favor the side that opposes the change (Brown and LeMay, Chemical Equilibrium chapter).
- 33
How does Le Chatelier's Principle relate to chemical reactions in closed systems?
In closed systems, Le Chatelier's Principle indicates that any disturbance will cause the system to shift to restore equilibrium (Tro, Chemical Equilibrium chapter).