Equilibrium Flashcard

Front

What is chemical equilibrium?

Back

Chemical equilibrium is a state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products.

Front

What is static equilibrium?

Back

Static equilibrium is a state where all forces acting on an object are balanced, and the object is at rest, meaning there is no movement or change.

Front

How does increasing pressure affect a reversible reaction at equilibrium with equal amounts of gas on both sides?

Back

Increasing pressure will have no effect on the equilibrium position since there is no favored side with less gas.

Front

What is the equilibrium expression for the reaction @@2 ext{C}(s) + O_2(g) ightleftharpoons 2 ext{CO}(g)@@?

Back

Front

When is a chemical reaction considered to be in equilibrium?

Back

A chemical reaction is in equilibrium when the rates of the forward and reverse reactions are equal.

Front

What happens to the equilibrium position when a product is added to a reaction at equilibrium?

Back

The equilibrium will shift to the left (towards the reactants) to counteract the change.

Front

What is Le Chatelier's Principle?

Back

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

Front

What is the significance of the equilibrium constant (K)?

Back

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium, indicating the extent of the reaction.

Front

What does it mean if the equilibrium constant (K) is greater than 1?

Back

If K > 1, it indicates that at equilibrium, the concentration of products is greater than that of reactants, favoring the formation of products.

Front

What does it mean if the equilibrium constant (K) is less than 1?

Back

If K < 1, it indicates that at equilibrium, the concentration of reactants is greater than that of products, favoring the formation of reactants.