Equilibrium

Front

What is equilibrium in a chemical reaction?

Back

Equilibrium is the state in which the forward and backward reactions occur at the same rate, resulting in constant concentrations of reactants and products.

Front

What does the double arrow (⇌) signify in a chemical equation?

Back

The double arrow indicates that the reaction is reversible, meaning it can proceed in both the forward and backward directions.

Front

What happens to the equilibrium position when pressure is increased in a reaction with equal moles of gas on both sides?

Back

The equilibrium position does not shift, as there are equal moles of gas on both sides of the reaction.

Front

In an exothermic reaction, where does the energy transfer occur?

Back

Energy is transferred from the reactants to their surroundings.

Front

What is Le Chatelier's Principle?

Back

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.

Front

How does increasing temperature affect an exothermic reaction at equilibrium?

Back

Increasing temperature shifts the equilibrium position to the left, favoring the reactants.

Front

What is the effect of adding a catalyst to a reaction at equilibrium?

Back

A catalyst speeds up both the forward and backward reactions equally, but does not change the position of the equilibrium.

Front

What is the relationship between concentration and equilibrium?

Back

Changing the concentration of reactants or products will shift the equilibrium position to favor the side with lower concentration.

Front

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

Back

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

Front

What happens to the concentration of products if the concentration of reactants is increased?

Back

Increasing the concentration of reactants will shift the equilibrium position to the right, increasing the concentration of products.