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This deck focuses on Introduction To Le Chateliers Principle, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.
AP Chemistry Flashcards: Introduction To Le Chateliers Principle
Study Introduction To Le Chateliers Principle in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.
AP Chemistry
Introduction To Le Chateliers Principle
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QUESTION
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How does adding a reactant affect equilibrium in a reaction?
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ANSWER
Shifts right to produce more products. More reactant drives equilibrium toward product formation.
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Flashcard 1: How does adding a reactant affect equilibrium in a reaction?
Answer: Shifts right to produce more products. More reactant drives equilibrium toward product formation.
Flashcard 2: What happens when pressure decreases in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Lower pressure favors side with more gas molecules.
Flashcard 3: What is the effect of adding more product to an equilibrium system?
Answer: Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Flashcard 4: How does increasing pressure affect a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. Higher pressure favors side with fewer gas molecules.
Flashcard 5: How does decreasing the concentration of reactants affect equilibrium?
Answer: Shifts left, favoring reactant formation. Less reactant drives reverse reaction to restore balance.
Flashcard 6: What happens to equilibrium when temperature decreases in an exothermic reaction?
Answer: Shifts right, favoring product formation. Lower temperature favors exothermic (heat-releasing) direction.
Flashcard 7: What is Le Chatelier's Principle?
Answer: A system at equilibrium shifts to counteract applied changes. System responds to minimize disturbance by shifting equilibrium.
Flashcard 8: What is the effect of decreasing the volume of a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. Smaller volume increases pressure, favoring fewer gas molecules.
Flashcard 9: What is the effect of removing a reactant from an equilibrium system?
Answer: Shifts left, producing more reactant. Less reactant causes reverse shift to restore equilibrium.
Flashcard 10: What is the effect of pressure changes on a system with equal moles of gas on both sides?
Answer: No shift in equilibrium position. Equal gas moles means pressure changes don't favor either side.
Flashcard 11: What happens when pressure decreases in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Lower pressure favors side with more gas molecules.
Flashcard 12: Identify the effect of decreasing temperature on an exothermic reaction.
Answer: Shifts right, favoring product formation. Lower temperature favors exothermic (heat-producing) direction.
Flashcard 13: What happens when you increase the volume of a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Larger volume decreases pressure, favoring gas expansion.
Flashcard 14: What effect does increasing the concentration of reactants have on equilibrium?
Answer: Shifts right, favoring product formation. Higher reactant concentration drives forward reaction direction.
Flashcard 15: What happens when you increase the volume of a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Larger volume decreases pressure, favoring gas expansion.
Flashcard 16: What happens when you increase the volume of a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Larger volume decreases pressure, favoring gas expansion.
Flashcard 17: What happens when you increase the volume in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Increased volume lowers pressure, favoring gas molecule production.
Flashcard 18: What is the effect of adding a reactant to an equilibrium system?
Answer: Shifts right to produce more products. Additional reactant drives forward reaction to consume excess.
Flashcard 19: Identify the effect of increasing temperature on an exothermic reaction.
Answer: Shifts left, favoring reactant formation. Higher temperature opposes heat release in exothermic reactions.
Flashcard 20: How does decreasing pressure affect a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Lower pressure favors side producing more gas molecules.
Flashcard 21: What happens to equilibrium when temperature decreases in an exothermic reaction?
Answer: Shifts right, favoring product formation. Lower temperature favors exothermic (heat-releasing) direction.
Flashcard 22: What happens when pressure increases in a system with no gaseous components?
Answer: No shift in equilibrium position. Pressure changes only affect systems with gaseous components.
Flashcard 23: How does decreasing the concentration of reactants affect equilibrium?
Answer: Shifts left, favoring reactant formation. Less reactant drives reverse reaction to restore balance.
Flashcard 24: What happens to equilibrium when temperature decreases in an exothermic reaction?
Answer: Shifts right, favoring product formation. Lower temperature favors exothermic (heat-releasing) direction.
Flashcard 25: What effect does decreasing temperature have on an exothermic reaction at equilibrium?
Answer: Shifts right, favoring product formation. Lower temperature favors heat-producing direction.
Flashcard 26: What effect does increasing the concentration of reactants have on equilibrium?
Answer: Shifts right, favoring product formation. Higher reactant concentration drives forward reaction direction.
Flashcard 27: Identify the effect of decreasing the concentration of products in equilibrium.
Answer: Shifts right, favoring product formation. Less product drives forward reaction to restore balance.
Flashcard 28: What is the effect of increasing temperature on an equilibrium system?
Answer: Shifts to absorb heat, depending on endo- or exothermic nature. Heat acts as reactant or product depending on reaction type.
Flashcard 29: What effect does increasing the concentration of products have on equilibrium?
Answer: Shifts left, favoring reactant formation. Excess product drives reverse reaction to consume it.
Flashcard 30: What is the effect of adding a reactant to an equilibrium system?
Answer: Shifts right to produce more products. Additional reactant drives forward reaction to consume excess.
Flashcard 31: How does decreasing the concentration of reactants impact equilibrium?
Answer: Shifts left, favoring reactant formation. Lower reactant concentration favors reverse reaction direction.
Flashcard 32: Identify the effect of adding more reactant to an equilibrium system.
Answer: Shifts right to produce more product. More reactant drives forward reaction to consume excess.
Flashcard 33: What is the effect of removing a product from an equilibrium system?
Answer: Shifts right, producing more product. System compensates by making more of removed substance.
Flashcard 34: What happens when pressure increases in a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. System minimizes pressure by reducing gas molecules.
Flashcard 35: Identify the effect of adding a catalyst to an equilibrium reaction.
Answer: No shift; only increases rate at which equilibrium is achieved. Catalysts affect reaction rates equally in both directions.
Flashcard 36: What is the effect of increasing temperature on an equilibrium system?
Answer: Shifts to absorb heat, depending on endo- or exothermic nature. Heat acts as reactant or product depending on reaction type.
Flashcard 37: Identify the effect of increasing temperature on an endothermic reaction.
Answer: Shifts right, favoring product formation. Higher temperature favors heat-absorbing direction.
Flashcard 38: What is the effect of adding an inert gas to a constant volume system?
Answer: No shift in equilibrium position. Inert gas doesn't affect partial pressures at constant volume.
Flashcard 39: How does increasing pressure affect a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. Higher pressure favors side with fewer gas molecules.
Flashcard 40: What effect does increasing the concentration of products have on equilibrium?
Answer: Shifts left, favoring reactant formation. Excess product drives reverse reaction to consume it.
Flashcard 41: What happens when pressure increases in a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. System minimizes pressure by reducing gas molecules.
Flashcard 42: What happens when you increase the volume in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Increased volume lowers pressure, favoring gas molecule production.
Flashcard 43: What happens when you increase the volume in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Increased volume lowers pressure, favoring gas molecule production.
Flashcard 44: What happens when you increase the volume of a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Larger volume decreases pressure, favoring gas expansion.
Flashcard 45: Identify the effect of decreasing the concentration of products in equilibrium.
Answer: Shifts right, favoring product formation. Less product drives forward reaction to restore balance.
Flashcard 46: Identify the effect of adding a catalyst to an equilibrium reaction.
Answer: No shift; only increases rate at which equilibrium is achieved. Catalysts affect reaction rates equally in both directions.
Flashcard 47: How does decreasing the concentration of reactants impact equilibrium?
Answer: Shifts left, favoring reactant formation. Lower reactant concentration favors reverse reaction direction.
Flashcard 48: Identify the effect of removing a product on an equilibrium system.
Answer: Shifts right to produce more product. Removing product drives forward reaction to replace it.
Flashcard 49: Identify the effect of removing a product on an equilibrium system.
Answer: Shifts right to produce more product. Removing product drives forward reaction to replace it.
Flashcard 50: What is the effect of pressure changes on a system with equal moles of gas on both sides?
Answer: No shift in equilibrium position. Equal gas moles means pressure changes don't favor either side.
Flashcard 51: What is the effect of adding more product to an equilibrium system?
Answer: Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Flashcard 52: What is the effect of adding more product to an equilibrium system?
Answer: Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Flashcard 53: Identify the effect of increasing temperature on an exothermic reaction.
Answer: Shifts left, favoring reactant formation. Higher temperature opposes heat release in exothermic reactions.
Flashcard 54: How does increasing pressure affect a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. Higher pressure favors side with fewer gas molecules.
Flashcard 55: What is the effect of pressure changes on a system with equal moles of gas on both sides?
Answer: No shift in equilibrium position. Equal gas moles means pressure changes don't favor either side.
Flashcard 56: How does adding a catalyst affect an equilibrium system?
Answer: No shift; only increases rate of reaching equilibrium. Catalysts speed both directions equally without shifting.
Flashcard 57: What happens when pressure decreases in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Lower pressure favors side with more gas molecules.
Flashcard 58: Identify the effect of increasing temperature on an endothermic reaction.
Answer: Shifts right, favoring product formation. Higher temperature favors heat-absorbing direction.
Flashcard 59: Identify the effect of adding more reactant to an equilibrium system.
Answer: Shifts right to produce more product. More reactant drives forward reaction to consume excess.
Flashcard 60: What is the effect of adding more product to an equilibrium system?
Answer: Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Flashcard 61: Identify the effect of decreasing temperature on an exothermic reaction.
Answer: Shifts right, favoring product formation. Lower temperature favors exothermic (heat-producing) direction.
Flashcard 62: What is the effect of removing a product from an equilibrium system?
Answer: Shifts right, producing more product. System compensates by making more of removed substance.
Flashcard 63: Identify the effect of decreasing the concentration of products in equilibrium.
Answer: Shifts right, favoring product formation. Less product drives forward reaction to restore balance.
Flashcard 64: What effect does decreasing temperature have on an exothermic reaction at equilibrium?
Answer: Shifts right, favoring product formation. Lower temperature favors heat-producing direction.
Flashcard 65: Identify the effect of temperature decrease on an endothermic reaction.
Answer: Shifts left, favoring reactant formation. Lower temperature opposes heat absorption in endothermic reactions.
Flashcard 66: Identify the effect of increasing temperature on an endothermic reaction.
Answer: Shifts right, favoring product formation. Higher temperature favors heat-absorbing direction.
Flashcard 67: Identify the effect of temperature decrease on an endothermic reaction.
Answer: Shifts left, favoring reactant formation. Lower temperature opposes heat absorption in endothermic reactions.
Flashcard 68: What happens when pressure increases in a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. System minimizes pressure by reducing gas molecules.
Flashcard 69: What is Le Chatelier's Principle?
Answer: A system at equilibrium shifts to counteract applied changes. System responds to minimize disturbance by shifting equilibrium.
Flashcard 70: How does adding a catalyst affect an equilibrium system?
Answer: No shift; only increases rate of reaching equilibrium. Catalysts speed both directions equally without shifting.
Flashcard 71: Identify the effect of adding a catalyst to an equilibrium reaction.
Answer: No shift; only increases rate at which equilibrium is achieved. Catalysts affect reaction rates equally in both directions.
Flashcard 72: What happens when pressure decreases in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Lower pressure favors side with more gas molecules.
Flashcard 73: How does adding a catalyst affect an equilibrium system?
Answer: No shift; only increases rate of reaching equilibrium. Catalysts speed both directions equally without shifting.
Flashcard 74: What happens when temperature increases in an endothermic reaction at equilibrium?
Answer: Shifts right, favoring product formation. Higher temperature favors endothermic (heat-absorbing) direction.
Flashcard 75: What is the effect of removing a reactant from an equilibrium system?
Answer: Shifts left, producing more reactant. Less reactant causes reverse shift to restore equilibrium.
Flashcard 76: What is the effect of removing a product from an equilibrium system?
Answer: Shifts right, producing more product. System compensates by making more of removed substance.
Flashcard 77: What is the effect of decreasing the volume of a gaseous equilibrium system?
Answer: Shifts to the side with fewer moles of gas. Smaller volume increases pressure, favoring fewer gas molecules.
Flashcard 78: What is the effect of adding a reactant to an equilibrium system?
Answer: Shifts right to produce more products. Additional reactant drives forward reaction to consume excess.
Flashcard 79: What effect does increasing the concentration of products have on equilibrium?
Answer: Shifts left, favoring reactant formation. Excess product drives reverse reaction to consume it.
Flashcard 80: Identify the effect of increasing temperature on an exothermic reaction.
Answer: Shifts left, favoring reactant formation. Higher temperature opposes heat release in exothermic reactions.
Flashcard 81: What happens when pressure increases in a system with no gaseous components?
Answer: No shift in equilibrium position. Pressure changes only affect systems with gaseous components.
Flashcard 82: How does adding a catalyst affect an equilibrium system?
Answer: No shift; only increases rate of reaching equilibrium. Catalysts speed both directions equally without shifting.
Flashcard 83: Identify the effect of decreasing the concentration of products in equilibrium.
Answer: Shifts right, favoring product formation. Less product drives forward reaction to restore balance.
Flashcard 84: What happens when pressure increases in a system with no gaseous components?
Answer: No shift in equilibrium position. Pressure changes only affect systems with gaseous components.
Flashcard 85: How does decreasing pressure affect a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Lower pressure favors side producing more gas molecules.
Flashcard 86: What is the effect of adding more product to an equilibrium system?
Answer: Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Flashcard 87: What is the effect of removing a product from an equilibrium system?
Answer: Shifts right, producing more product. System compensates by making more of removed substance.
Flashcard 88: What is the effect of adding a reactant to an equilibrium system?
Answer: Shifts right to produce more products. Additional reactant drives forward reaction to consume excess.
Flashcard 89: How does adding a reactant affect equilibrium in a reaction?
Answer: Shifts right to produce more products. More reactant drives equilibrium toward product formation.
Flashcard 90: What is the effect of adding an inert gas to a constant volume system?
Answer: No shift in equilibrium position. Inert gas doesn't affect partial pressures at constant volume.
Flashcard 91: What is the effect of adding an inert gas to a constant volume system?
Answer: No shift in equilibrium position. Inert gas doesn't affect partial pressures at constant volume.
Flashcard 92: What happens when you increase the volume in a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Increased volume lowers pressure, favoring gas molecule production.
Flashcard 93: Identify the effect of decreasing temperature on an exothermic reaction.
Answer: Shifts right, favoring product formation. Lower temperature favors exothermic (heat-producing) direction.
Flashcard 94: Identify the effect of removing a product on an equilibrium system.
Answer: Shifts right to produce more product. Removing product drives forward reaction to replace it.
Flashcard 95: How does decreasing pressure affect a gaseous equilibrium system?
Answer: Shifts to the side with more moles of gas. Lower pressure favors side producing more gas molecules.
Flashcard 96: What happens when temperature increases in an endothermic reaction at equilibrium?
Answer: Shifts right, favoring product formation. Higher temperature favors endothermic (heat-absorbing) direction.
Flashcard 97: Identify the effect of decreasing temperature on an endothermic reaction.
Answer: Shifts left, favoring reactant formation. Lower temperature opposes heat absorption in endothermic reactions.
Flashcard 98: What is the effect of adding more product to an equilibrium system?
Answer: Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Flashcard 99: Identify the effect of adding a catalyst to an equilibrium reaction.
Answer: No shift; only increases rate at which equilibrium is achieved. Catalysts affect reaction rates equally in both directions.
Flashcard 100: Identify the effect of decreasing temperature on an exothermic reaction.
Answer: Shifts right, favoring product formation. Lower temperature favors exothermic (heat-producing) direction.