Chemical Equilibrium

What is chemical equilibrium?

• A state in a chemical reaction where the forward and reverse reactions occur at the same rate, resulting in no net change in the concentrations of reactants and products.

• A process where only one reaction occurs

• A condition where products are continuously formed

• A state where reactants are completely consumed

State Le Chatelier's Principle.

• If a system at equilibrium is disturbed, it will remain unchanged

• If a system at equilibrium is disturbed by changing the conditions, the system will shift its equilibrium position to counteract the change.

• Changing conditions in a system at equilibrium will not affect the equilibrium position

• Le Chatelier's Principle states that equilibrium cannot be shifted

Explain the concept of equilibrium constant.

• The equilibrium constant is a measure of the rate of a chemical reaction

• The equilibrium constant changes with temperature

• The equilibrium constant is a value that expresses the ratio of the concentrations of products to reactants at equilibrium in a chemical reaction.

• The equilibrium constant is always equal to 1

How does temperature affect the equilibrium position?

• Temperature affects the equilibrium position by changing the value of the equilibrium constant.

• Temperature only affects the rate of the reaction, not the equilibrium position

• Temperature causes the equilibrium position to shift to the left

• Temperature has no effect on the equilibrium position

Discuss the role of catalysts in chemical equilibrium.

• Catalysts speed up the attainment of equilibrium by lowering activation energy for both forward and reverse reactions.

• Catalysts slow down the attainment of equilibrium by increasing activation energy for both forward and reverse reactions.

• Catalysts have no effect on chemical equilibrium.

• Catalysts only lower activation energy for the forward reaction in chemical equilibrium.

Define the term 'dynamic equilibrium'.

• A state where the reaction has stopped completely

• A state where the concentrations of reactants and products are constantly changing

• A state where only the forward reaction occurs

• A state in which forward and reverse processes occur at the same rate, resulting in no net change in the concentrations of reactants and products over time.

What are the factors that can affect the equilibrium of a reaction?

• Volume, time, color

• Density, mass, shape

• Surface area, pH, solvent

• Temperature, pressure, concentration, catalysts

Describe the difference between homogeneous and heterogeneous equilibrium.

• Homogeneous equilibrium involves multiple phases.

• Heterogeneous equilibrium involves only one substance.

• In homogeneous equilibrium, all substances are in the same phase, whereas in heterogeneous equilibrium, substances are in different phases.

• In homogeneous equilibrium, substances are in different phases.

Explain the significance of the reaction quotient Q in chemical equilibrium.

• Q is a constant value that does not change during a reaction.

• The reaction quotient Q is only relevant in exothermic reactions.

• The reaction quotient Q provides information about the current state of a reaction in terms of concentrations of products and reactants, guiding the system towards equilibrium.

• Q is used to calculate the activation energy of a reaction.

Discuss the relationship between Gibbs free energy and chemical equilibrium.

• Gibbs free energy is always positive at equilibrium

• Gibbs free energy decreases at equilibrium

• Chemical equilibrium is not related to Gibbs free energy

• The relationship between Gibbs free energy and chemical equilibrium is that at equilibrium, the Gibbs free energy change is zero.