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Questions and Answers
What happens to the total pressure in a container when the volume is decreased?
What happens to the total pressure in a container when the volume is decreased?
- Total pressure remains constant regardless of volume change.
- Total pressure decreases due to the exothermic nature of the reaction.
- Total pressure decreases due to increased volume.
- Total pressure increases due to increased concentration of gases. (correct)
According to Le Chatelier’s principle, how does an increase in pressure affect a reaction at equilibrium?
According to Le Chatelier’s principle, how does an increase in pressure affect a reaction at equilibrium?
- The reaction rate increases regardless of direction.
- The equilibrium shifts to the side with fewer gas molecules. (correct)
- The equilibrium shifts to the side with more gas molecules.
- The equilibrium remains unchanged.
What effect does increasing temperature have on an endothermic reaction?
What effect does increasing temperature have on an endothermic reaction?
- The equilibrium remains unchanged.
- Decreases the equilibrium constant.
- Shifts the equilibrium to the left, favoring reactants.
- Shifts the equilibrium to the right, favoring products. (correct)
In an exothermic reaction, what happens when the temperature is decreased?
In an exothermic reaction, what happens when the temperature is decreased?
What role does heat play in an endothermic reaction?
What role does heat play in an endothermic reaction?
How does a decrease in volume affect the reaction equilibrium with respect to gas concentration?
How does a decrease in volume affect the reaction equilibrium with respect to gas concentration?
In the reaction CO + 3H2 ⇌ CH4 + H2O, what happens after compression if the equilibrium shifts?
In the reaction CO + 3H2 ⇌ CH4 + H2O, what happens after compression if the equilibrium shifts?
What effect does increasing the temperature have on the equilibrium constant of an exothermic reaction?
What effect does increasing the temperature have on the equilibrium constant of an exothermic reaction?
What is the first step in calculating equilibrium concentrations?
What is the first step in calculating equilibrium concentrations?
How does adding reactants affect the position of equilibrium in a chemical reaction?
How does adding reactants affect the position of equilibrium in a chemical reaction?
Which of the following methods does NOT alter the equilibrium composition of a gaseous reaction mixture?
Which of the following methods does NOT alter the equilibrium composition of a gaseous reaction mixture?
In the reaction CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g), what happens when additional products are added?
In the reaction CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g), what happens when additional products are added?
When using an ICE table, what do 'Initial', 'Change', and 'Equilibrium' refer to?
When using an ICE table, what do 'Initial', 'Change', and 'Equilibrium' refer to?
What does Le Chatelier’s principle describe?
What does Le Chatelier’s principle describe?
If a gaseous reaction reduces in volume, what effect does this have on equilibrium?
If a gaseous reaction reduces in volume, what effect does this have on equilibrium?
In terms of equilibrium constant, what occurs when a chemical reaction reaches a new equilibrium after disturbance?
In terms of equilibrium constant, what occurs when a chemical reaction reaches a new equilibrium after disturbance?
Study Notes
Calculating Equilibrium Concentrations
- Use an ICE table (Initial, Change, Equilibrium) to organize data for calculations.
- Define initial concentrations, changes in concentration, and final equilibrium concentrations using variable x.
- Substitute these expressions into the equilibrium constant equation to solve for equilibrium concentrations.
Altering Equilibrium Composition
- Changes to affect equilibrium composition in gas reactions:
- Add reactants or remove products to alter concentrations.
- Change volume to affect partial pressure of gases.
- Adjust temperature of the system.
Le Chatelier's Principle
- A system at equilibrium will shift to counteract disturbances in concentration, temperature, or pressure.
- Example reaction: CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g).
- New equilibrium concentrations adjust to maintain the equilibrium constant.
Concentration Changes
- Adding reactants or removing products shifts the equilibrium to the right, increasing product formation.
- Adding products or removing reactants shifts the equilibrium to the left, increasing reactant formation.
Pressure Changes
- Decreasing the container's volume increases gas concentration and pressure.
- The equilibrium shifts towards the side with fewer gas molecules to relieve the pressure.
- In the reaction CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g), compression shifts equilibrium to the right due to fewer gas molecules on that side.
Temperature Effects: Endothermic Reactions
- Endothermic reactions require heat as a reactant and absorb energy.
- Increasing temperature shifts equilibrium right, favoring products and increasing equilibrium constant.
- Decreasing temperature shifts equilibrium left, favoring reactants and decreasing equilibrium constant.
Temperature Effects: Exothermic Reactions
- Exothermic reactions release energy, with heat acting as a product.
- Increasing temperature shifts equilibrium left, favoring reactants and decreasing equilibrium constant.
- Decreasing temperature shifts equilibrium right, favoring products and increasing equilibrium constant.
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Description
Explore the principles of chemical equilibrium, including the use of ICE tables for calculating equilibrium concentrations and the effects of concentration changes on equilibrium composition. Learn how Le Chatelier's Principle helps predict shifts in equilibrium in response to external changes. This quiz will test your understanding of these key concepts in chemistry.
