4.6.2 Reversible reactions and dynamic equilibrium Flashcards
What are reversible reactions?
Reversible reactions are those in which the products can react to produce the original reactants, represented as A + B ⇌ C + D.
How can the direction of reversible reactions be changed?
The direction of reversible reactions can be changed by altering the conditions.
What is the relationship between exothermic and endothermic reactions in reversible reactions?
If a reversible reaction is exothermic in one direction, it is endothermic in the opposite direction, with the same amount of energy transferred in each case.
What is equilibrium in reversible reactions?
Equilibrium is reached when the forward and reverse reactions occur at exactly the same rate in a closed system.
What does Le Chatelier’s Principle state?
Le Chatelier’s Principle states that if a change is made to any conditions in a system at equilibrium, the system responds to counteract the change.
What happens to equilibrium when the concentration of a reactant is increased?
If the concentration of a reactant is increased, more products will be formed until equilibrium is reached again.
What happens to equilibrium when the concentration of a product is decreased?
If the concentration of a product is decreased, more reactants will react until equilibrium is reached again.
How does an increase in temperature affect an endothermic reaction at equilibrium?
An increase in temperature causes the relative amount of products at equilibrium to increase for an endothermic reaction.
How does a decrease in temperature affect an exothermic reaction at equilibrium?
A decrease in temperature causes the relative amount of products at equilibrium to increase for an exothermic reaction.
What is the effect of increased pressure on gaseous reactions at equilibrium?
An increase in pressure causes the equilibrium position to shift towards the side with the smaller number of molecules.
What is the effect of decreased pressure on gaseous reactions at equilibrium?
A decrease in pressure causes the equilibrium position to shift towards the side with the larger number of molecules.
