Equilibrium and Le Chatelier's Principle

Front

What two factors indicate that a reaction is at equilibrium?

Back

The concentrations are constant; the forward and reverse reactions are equal

Front

Which statement is not correct regarding equilibrium? Equilibrium is achieved when the product and reactant concentrations are the same, Equilibrium is achieved when the concentrations of all reactants is constant, Equilibrium is achieved when the forward and reverse reactions are equal, Equilibrium is achieved when the ratio of products to reactants is constant

Back

Equilibrium is achieved when the product and reactant concentrations are the same

Front

A double sided arrow (↔), indicates that a reaction is:

Back

Reversible

Front

A single sided arrow (→) indicates that a reaction is:

Back

Irreversible

Front

When the forward and reverse reactions are occurring at the same rate, the reaction is said to be at:

Back

Chemical equilibrium

Front

If a reversible reaction has reached equilibrium, what is true about the concentration of the reactants vs the products?

Back

Some reactants are present, as are some products

Front

Adding H₂ to N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat will cause the equilibrium to:

Back

Shift right

Front

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat Increasing the temperature will cause the equilibrium to:

Back

Shift left

Front

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat Removing N₂ will cause the equilibrium to:

Back

Shift left

Front

N₂(g) + 3H₂(g) ↔ 2 NH₃(g) + heat Increasing the volume of the container will cause the equilibrium to:

Back

Shift left