Factors Affecting Chemical Equilibrium

What happens to equilibrium when temperature increases?

• Equilibrium remains unchanged.

• Equilibrium is disrupted and cannot be restored.

• Equilibrium shifts to favor the endothermic direction.

• Equilibrium shifts to favor the exothermic direction.

How does decreasing the concentration of reactants affect equilibrium?

• It has no effect on equilibrium.

• It shifts the equilibrium to favor reactants.

• It shifts the equilibrium to favor products.

• It increases the rate of the reaction.

What is the effect of increasing pressure on gaseous reactions?

• It has no effect on the reaction.

• It shifts the equilibrium towards the side with fewer moles of gas.

• It increases the rate of the reaction regardless of moles.

• It shifts the equilibrium towards the side with more moles of gas.

Explain how temperature can shift the position of equilibrium.

• Increasing temperature always favors the reverse reaction.

• Temperature changes only affect the rate of reaction, not equilibrium.

• Temperature changes can shift the position of equilibrium by favoring either the forward or reverse reaction, depending on whether the reaction is exothermic or endothermic.

• Temperature has no effect on equilibrium position.

What is Le Chatelier's principle?

• Le Chatelier's principle describes how a system at equilibrium responds to changes in concentration, temperature, or pressure.

• Le Chatelier's principle states that all chemical reactions are irreversible.

• Le Chatelier's principle only applies to gases and not to liquids or solids.

• Le Chatelier's principle explains the behavior of non-equilibrium systems.

How does adding more reactants influence the equilibrium position?

• The equilibrium position remains unchanged regardless of reactant concentration.

• Adding more reactants has no effect on the equilibrium position.

• The equilibrium position shifts to the left, favoring reactant formation.

• The equilibrium position shifts to the right, favoring product formation.

What role does pressure play in reactions involving gases?

• Pressure influences gas reactions by affecting volume and concentration, shifting equilibrium.

• Pressure has no effect on gas reactions.

• Pressure only affects solid reactions, not gases.

• Higher pressure always increases reaction rates.

Describe the impact of temperature on exothermic reactions at equilibrium.

• Exothermic reactions always favor products regardless of temperature changes.

• Temperature has no effect on the position of equilibrium in exothermic reactions.

• Increasing temperature shifts equilibrium to the right (favoring products); decreasing temperature shifts it to the left (favoring reactants).

• Increasing temperature shifts equilibrium to the left (favoring reactants); decreasing temperature shifts it to the right (favoring products).

What happens to equilibrium if the volume of the container is decreased?

• The equilibrium shifts towards the side with fewer moles of gas.

• The equilibrium remains unchanged.

• The equilibrium shifts towards the side with more moles of gas.

• The reaction stops completely.

How can we predict the shift in equilibrium with changes in concentration?

• The equilibrium shifts towards the side with lower concentration when a substance is added.

• The equilibrium shifts towards the side with higher concentration when a substance is removed.

• Adding a substance always shifts the equilibrium to the right.

• The equilibrium remains unchanged regardless of concentration changes.