Introduction to Le Chatelier's Principle - AP Chemistry
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Identify the effect of removing a product on an equilibrium system.
Identify the effect of removing a product on an equilibrium system.
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Shifts right to produce more product. Removing product drives forward reaction to replace it.
Shifts right to produce more product. Removing product drives forward reaction to replace it.
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What is the effect of adding more product to an equilibrium system?
What is the effect of adding more product to an equilibrium system?
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Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
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Identify the effect of decreasing temperature on an endothermic reaction.
Identify the effect of decreasing temperature on an endothermic reaction.
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Shifts left, favoring reactant formation. Lower temperature opposes heat absorption in endothermic reactions.
Shifts left, favoring reactant formation. Lower temperature opposes heat absorption in endothermic reactions.
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What happens when temperature increases in an endothermic reaction at equilibrium?
What happens when temperature increases in an endothermic reaction at equilibrium?
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Shifts right, favoring product formation. Higher temperature favors endothermic (heat-absorbing) direction.
Shifts right, favoring product formation. Higher temperature favors endothermic (heat-absorbing) direction.
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What effect does decreasing temperature have on an exothermic reaction at equilibrium?
What effect does decreasing temperature have on an exothermic reaction at equilibrium?
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Shifts right, favoring product formation. Lower temperature favors heat-producing direction.
Shifts right, favoring product formation. Lower temperature favors heat-producing direction.
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What is the effect of removing a reactant from an equilibrium system?
What is the effect of removing a reactant from an equilibrium system?
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Shifts left, producing more reactant. Less reactant causes reverse shift to restore equilibrium.
Shifts left, producing more reactant. Less reactant causes reverse shift to restore equilibrium.
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What effect does increasing the concentration of products have on equilibrium?
What effect does increasing the concentration of products have on equilibrium?
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Shifts left, favoring reactant formation. Excess product drives reverse reaction to consume it.
Shifts left, favoring reactant formation. Excess product drives reverse reaction to consume it.
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How does decreasing the concentration of reactants affect equilibrium?
How does decreasing the concentration of reactants affect equilibrium?
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Shifts left, favoring reactant formation. Less reactant drives reverse reaction to restore balance.
Shifts left, favoring reactant formation. Less reactant drives reverse reaction to restore balance.
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What is the effect of pressure changes on a system with equal moles of gas on both sides?
What is the effect of pressure changes on a system with equal moles of gas on both sides?
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No shift in equilibrium position. Equal gas moles means pressure changes don't favor either side.
No shift in equilibrium position. Equal gas moles means pressure changes don't favor either side.
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What is the effect of decreasing the volume of a gaseous equilibrium system?
What is the effect of decreasing the volume of a gaseous equilibrium system?
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Shifts to the side with fewer moles of gas. Smaller volume increases pressure, favoring fewer gas molecules.
Shifts to the side with fewer moles of gas. Smaller volume increases pressure, favoring fewer gas molecules.
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What is the effect of adding more product to an equilibrium system?
What is the effect of adding more product to an equilibrium system?
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Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
Shifts left to produce more reactant. Excess product drives reverse reaction to consume it.
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What happens when pressure increases in a system with no gaseous components?
What happens when pressure increases in a system with no gaseous components?
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No shift in equilibrium position. Pressure changes only affect systems with gaseous components.
No shift in equilibrium position. Pressure changes only affect systems with gaseous components.
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What is the effect of adding a reactant to an equilibrium system?
What is the effect of adding a reactant to an equilibrium system?
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Shifts right to produce more products. Additional reactant drives forward reaction to consume excess.
Shifts right to produce more products. Additional reactant drives forward reaction to consume excess.
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How does adding a reactant affect equilibrium in a reaction?
How does adding a reactant affect equilibrium in a reaction?
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Shifts right to produce more products. More reactant drives equilibrium toward product formation.
Shifts right to produce more products. More reactant drives equilibrium toward product formation.
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What is the effect of removing a product from an equilibrium system?
What is the effect of removing a product from an equilibrium system?
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Shifts right, producing more product. System compensates by making more of removed substance.
Shifts right, producing more product. System compensates by making more of removed substance.
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What happens when you increase the volume of a gaseous equilibrium system?
What happens when you increase the volume of a gaseous equilibrium system?
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Shifts to the side with more moles of gas. Larger volume decreases pressure, favoring gas expansion.
Shifts to the side with more moles of gas. Larger volume decreases pressure, favoring gas expansion.
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How does decreasing pressure affect a gaseous equilibrium system?
How does decreasing pressure affect a gaseous equilibrium system?
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Shifts to the side with more moles of gas. Lower pressure favors side producing more gas molecules.
Shifts to the side with more moles of gas. Lower pressure favors side producing more gas molecules.
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What is the effect of increasing temperature on an equilibrium system?
What is the effect of increasing temperature on an equilibrium system?
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Shifts to absorb heat, depending on endo- or exothermic nature. Heat acts as reactant or product depending on reaction type.
Shifts to absorb heat, depending on endo- or exothermic nature. Heat acts as reactant or product depending on reaction type.
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Identify the effect of decreasing the concentration of products in equilibrium.
Identify the effect of decreasing the concentration of products in equilibrium.
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Shifts right, favoring product formation. Less product drives forward reaction to restore balance.
Shifts right, favoring product formation. Less product drives forward reaction to restore balance.
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What is Le Chatelier's Principle?
What is Le Chatelier's Principle?
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A system at equilibrium shifts to counteract applied changes. System responds to minimize disturbance by shifting equilibrium.
A system at equilibrium shifts to counteract applied changes. System responds to minimize disturbance by shifting equilibrium.
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What happens when pressure decreases in a gaseous equilibrium system?
What happens when pressure decreases in a gaseous equilibrium system?
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Shifts to the side with more moles of gas. Lower pressure favors side with more gas molecules.
Shifts to the side with more moles of gas. Lower pressure favors side with more gas molecules.
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Identify the effect of adding more reactant to an equilibrium system.
Identify the effect of adding more reactant to an equilibrium system.
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Shifts right to produce more product. More reactant drives forward reaction to consume excess.
Shifts right to produce more product. More reactant drives forward reaction to consume excess.
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How does adding a catalyst affect an equilibrium system?
How does adding a catalyst affect an equilibrium system?
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No shift; only increases rate of reaching equilibrium. Catalysts speed both directions equally without shifting.
No shift; only increases rate of reaching equilibrium. Catalysts speed both directions equally without shifting.
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Identify the effect of decreasing temperature on an exothermic reaction.
Identify the effect of decreasing temperature on an exothermic reaction.
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Shifts right, favoring product formation. Lower temperature favors exothermic (heat-producing) direction.
Shifts right, favoring product formation. Lower temperature favors exothermic (heat-producing) direction.
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Identify the effect of increasing temperature on an endothermic reaction.
Identify the effect of increasing temperature on an endothermic reaction.
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Shifts right, favoring product formation. Higher temperature favors heat-absorbing direction.
Shifts right, favoring product formation. Higher temperature favors heat-absorbing direction.
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What happens when pressure increases in a gaseous equilibrium system?
What happens when pressure increases in a gaseous equilibrium system?
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Shifts to the side with fewer moles of gas. System minimizes pressure by reducing gas molecules.
Shifts to the side with fewer moles of gas. System minimizes pressure by reducing gas molecules.
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How does increasing pressure affect a gaseous equilibrium system?
How does increasing pressure affect a gaseous equilibrium system?
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Shifts to the side with fewer moles of gas. Higher pressure favors side with fewer gas molecules.
Shifts to the side with fewer moles of gas. Higher pressure favors side with fewer gas molecules.
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What is the effect of adding an inert gas to a constant volume system?
What is the effect of adding an inert gas to a constant volume system?
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No shift in equilibrium position. Inert gas doesn't affect partial pressures at constant volume.
No shift in equilibrium position. Inert gas doesn't affect partial pressures at constant volume.
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Identify the effect of adding a catalyst to an equilibrium reaction.
Identify the effect of adding a catalyst to an equilibrium reaction.
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No shift; only increases rate at which equilibrium is achieved. Catalysts affect reaction rates equally in both directions.
No shift; only increases rate at which equilibrium is achieved. Catalysts affect reaction rates equally in both directions.
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What happens to equilibrium when temperature decreases in an exothermic reaction?
What happens to equilibrium when temperature decreases in an exothermic reaction?
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Shifts right, favoring product formation. Lower temperature favors exothermic (heat-releasing) direction.
Shifts right, favoring product formation. Lower temperature favors exothermic (heat-releasing) direction.
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