AP Chemistry--Equilibrium Basics Unit 7

How does pressure affect equilibrium in gaseous reactions?

• Increasing pressure shifts the equilibrium position toward the side with fewer moles of gas, while decreasing pressure shifts it toward the side with more moles.

• Increasing pressure has no effect on the equilibrium position of gaseous reactions.

• Decreasing pressure always favors the formation of products in gaseous reactions.

• Pressure changes only affect solid and liquid reactions, not gaseous ones.

Explain the effect of temperature on the equilibrium constant (K).

• Increasing temperature increases K for exothermic reactions.

• Increasing temperature decreases K for exothermic reactions.

• Increasing temperature has no effect on K for both exothermic and endothermic reactions.

• Increasing temperature increases K for endothermic reactions.

How does increasing temperature affect an endothermic reaction at equilibrium?

• It shifts the equilibrium position to the left, favoring the formation of reactants.

• It has no effect on the equilibrium position.

• It shifts the equilibrium position to the right, favoring the formation of products.

• It decreases the rate of the reaction.

What is Le Chatelier's Principle?

• Le Chatelier's Principle states that a system at equilibrium will remain unchanged regardless of disturbances.

• Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium.

• Le Chatelier's Principle states that all chemical reactions are reversible under any conditions.

• Le Chatelier's Principle states that temperature changes do not affect the equilibrium of a reaction.

What is the effect of lowering temperature on an exothermic reaction at equilibrium?

• It shifts the equilibrium position to the left, favoring the formation of reactants.

• It has no effect on the equilibrium position.

• It shifts the equilibrium position to the right, favoring the formation of products.

• It increases the rate of the reaction without affecting equilibrium.

How does decreasing the volume of a gaseous reaction at equilibrium affect the position of equilibrium?

• It has no effect on the position of equilibrium.

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

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

• It causes the reaction to stop completely.

What does a large equilibrium constant (Kc) indicate about a reaction?

• The reaction is at equilibrium and no further changes will occur.

• The reaction favors the formation of reactants at equilibrium.

• A large equilibrium constant indicates that at equilibrium, the reaction favors the formation of products.

• The reaction will proceed to completion without any products formed.

Define dynamic equilibrium in the context of chemical reactions.

• Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products.

• Dynamic equilibrium is a state where reactants are completely converted into products without any reverse reaction.

• Dynamic equilibrium is achieved only when the temperature and pressure are constant throughout the reaction.

• Dynamic equilibrium refers to a situation where the concentration of reactants is greater than that of products.

What is true for a system at equilibrium?

• At equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

• At equilibrium, the concentration of reactants is always greater than that of products.

• At equilibrium, the system is at rest and no reactions occur.

• At equilibrium, the forward reaction occurs faster than the reverse reaction.

Given K = 1.2, [CO2] = 0.846M, and [CH4] = 0.0713M, how do you find [H2O]?

• 0.218 M

• 0.318 M

• 0.418 M

• 0.518 M