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Questions and Answers
How does Le Châtelier's Principle help predict the shift in equilibrium when a system is disturbed?
How does Le Châtelier's Principle help predict the shift in equilibrium when a system is disturbed?
It states that the system will adjust to counteract the change and restore equilibrium.
Explain why dynamic equilibrium can only be established in a closed system.
Explain why dynamic equilibrium can only be established in a closed system.
A closed system prevents the loss or gain of reactants or products, ensuring that the reaction rates can equalize.
If you increase the concentration of a product in a system at equilibrium, what happens to the rate of the reverse reaction and why?
If you increase the concentration of a product in a system at equilibrium, what happens to the rate of the reverse reaction and why?
The rate of the reverse reaction will increase because there are more product molecules available to react and form reactants.
How does increasing the pressure affect the equilibrium of a reaction where the number of gas molecules is the same on both sides of the equation?
How does increasing the pressure affect the equilibrium of a reaction where the number of gas molecules is the same on both sides of the equation?
For an endothermic reaction, how does decreasing the temperature change the equilibrium and why?
For an endothermic reaction, how does decreasing the temperature change the equilibrium and why?
Describe how you would measure the rate of a reaction in which a gas is produced.
Describe how you would measure the rate of a reaction in which a gas is produced.
Explain the relationship between activation energy and the rate of a chemical reaction.
Explain the relationship between activation energy and the rate of a chemical reaction.
How does increasing the surface area of a solid reactant affect the collision frequency and, consequently, the reaction rate?
How does increasing the surface area of a solid reactant affect the collision frequency and, consequently, the reaction rate?
Explain why increasing the temperature generally increases the rate of a chemical reaction.
Explain why increasing the temperature generally increases the rate of a chemical reaction.
How does a catalyst increase the rate of a reaction?
How does a catalyst increase the rate of a reaction?
Describe the conditions necessary for a reaction to reach dynamic equilibrium.
Describe the conditions necessary for a reaction to reach dynamic equilibrium.
Explain how concentration affects the rate of reaction based on collision theory.
Explain how concentration affects the rate of reaction based on collision theory.
How does pressure influence the rate of reaction in gaseous systems, and why?
How does pressure influence the rate of reaction in gaseous systems, and why?
Explain the difference between a 'fast' and 'slow' reaction in terms of reaction rate.
Explain the difference between a 'fast' and 'slow' reaction in terms of reaction rate.
Describe what happens to the concentrations of reactants and products once a reversible reaction reaches dynamic equilibrium.
Describe what happens to the concentrations of reactants and products once a reversible reaction reaches dynamic equilibrium.
How would decreasing the volume of a container affect a system at equilibrium containing gaseous reactants and products, according to Le Châtelier’s principle?
How would decreasing the volume of a container affect a system at equilibrium containing gaseous reactants and products, according to Le Châtelier’s principle?
Explain why a system at equilibrium must be a closed system, relating it to the definition of equilibrium.
Explain why a system at equilibrium must be a closed system, relating it to the definition of equilibrium.
Describe how a catalyst affects the potential energy diagram of a reaction.
Describe how a catalyst affects the potential energy diagram of a reaction.
Explain the significance of 'correct orientation' in collision theory for a reaction to occur.
Explain the significance of 'correct orientation' in collision theory for a reaction to occur.
How does the addition of an inert gas (that does not participate in the reaction) at constant volume affect a system already at equilibrium?
How does the addition of an inert gas (that does not participate in the reaction) at constant volume affect a system already at equilibrium?
Flashcards
Reversible Reactions
Reversible Reactions
Reactions that can proceed in both directions: reactants to products and products to reactants.
Dynamic Equilibrium
Dynamic Equilibrium
A state where the forward and backward reactions occur at the same rate.
Closed System
Closed System
A system where no substances can enter or leave, essential for equilibrium.
Le Châtelier’s Principle
Le Châtelier’s Principle
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Effect of Concentration Increase
Effect of Concentration Increase
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Effect of Pressure Increase
Effect of Pressure Increase
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Exothermic Reaction (Temperature)
Exothermic Reaction (Temperature)
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Endothermic Reaction (Temperature)
Endothermic Reaction (Temperature)
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Rate of Reaction
Rate of Reaction
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Measuring Reaction Rate
Measuring Reaction Rate
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Collision Theory
Collision Theory
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Activation Energy
Activation Energy
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Effect of Increased Surface Area
Effect of Increased Surface Area
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Effect of Increased Concentration
Effect of Increased Concentration
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Effect of Increased Pressure (Gases)
Effect of Increased Pressure (Gases)
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Effect of Increased Temperature
Effect of Increased Temperature
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Role of a Catalyst
Role of a Catalyst
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Study Notes
Reversible Reactions
- Reversible reactions proceed in both directions, allowing products to revert to reactants.
- The ongoing forward reaction converts reactants into products
- The ongoing backward reaction converts products back into reactants.
Dynamic Equilibrium
- Dynamic equilibrium occurs in a reversible reaction when the forward and backward reactions occur at the same rate.
- Concentrations of reactants and products remain constant
- Reactants and products continue to form at the same rate.
- Equilibrium must take place within a closed system.
- Closed systems prevent reactants or products from escaping.
Le Châtelier’s Principle
- A system at equilibrium will counteract any disturbance to restore equilibrium.
Factors Affecting Equilibrium
- Concentration changes shift equilibrium away from an added substance or toward a removed substance.
- Increasing pressure shifts equilibrium toward the side with fewer gas molecules.
- Decreasing pressure shifts equilibrium toward the side with more gas molecules.
Temperature and Exothermic Reactions
- Exothermic reactions release heat (ΔH < 0).
- Increasing temperature shifts equilibrium left.
- Decreasing temperature shifts equilibrium right.
Temperature and Endothermic Reactions
- Endothermic reactions absorb heat (ΔH > 0).
- Increasing temperature shifts equilibrium right.
- Decreasing temperature shifts equilibrium left.
Effects of Equilibrium Changes
- Changes in concentration, pressure, or temperature disrupt the equilibrium position.
- The equilibrium shifts to oppose the change.
- Increasing reactant concentration or decreasing product concentration shifts equilibrium toward the product side.
- Decreasing reactant concentration or increasing product concentration shifts equilibrium toward the reactant side.
- Increasing pressure favors the side with fewer gas molecules.
- Increasing temperature shifts equilibrium toward the endothermic direction.
- Decreasing temperature shifts equilibrium toward the exothermic direction.
Rate of a Chemical Reaction
- Rate of reaction measures how quickly reactants convert into products.
- Fast reactions complete quickly
- Slow reactions take more time.
Measuring Rate of Reaction
- Rate can be measured by tracking reactant depletion or product formation over time.
- The method depends on the ease of tracking reactants versus products.
- Rate = Amount of reactants used or products formed / Time
Collision Theory and Activation Energy
- Reactions occur when particles collide with sufficient energy.
- Activation energy is the minimum energy needed for a reaction.
- Collision frequency affects reaction rate
- Energy of collisions affects reaction rate
- Correct orientation affects reaction rate
Factors Affecting Rate of Reaction
Surface Area
- Increased surface area of a solid reactant increases the reaction rate.
Concentration
- Higher concentration increases reaction rate due to more frequent collisions.
Pressure (for Gases)
- Increased pressure increases reaction rate by forcing gas particles closer together.
Temperature
- Higher temperature increases reaction rate as particles move faster
- At higher temperature particles collide more frequently and with more energy.
Catalysts
- Catalysts increase reaction rate without being consumed.
- Catalysts lower activation energy.
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