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