Chemical Equilibrium

What is chemical equilibrium?

• Chemical equilibrium is a state where reactants are completely consumed and products are formed.

• Chemical equilibrium is 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.

• Chemical equilibrium is a state where the reaction stops completely.

• Chemical equilibrium is a state where the concentration of reactants continuously increases.

State Le Chatelier's Principle.

• Le Chatelier's Principle states that increasing the temperature of a system at equilibrium will cause it to shift towards the reactants.

• Le Chatelier's Principle states that decreasing the pressure of a system at equilibrium will lead to an increase in the concentration of products.

• Le Chatelier's Principle states that a system at equilibrium will always remain unchanged regardless of external factors.

• Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants/products, the system will shift its position to counteract the effect of the change and restore equilibrium.

Explain the concept of dynamic equilibrium.

• Dynamic equilibrium occurs when the reactants are completely consumed.

• Dynamic equilibrium is when the reaction stops completely.

• Dynamic equilibrium is achieved when the rate of the forward reaction equals the rate of the reverse reaction, maintaining constant concentrations of reactants and products.

• Dynamic equilibrium is only achieved in irreversible reactions.

What are the factors that can affect chemical equilibrium?

• Temperature, pressure, concentration of reactants and products, presence of catalysts

• Color of the reactants, Time of day, Phase of the moon

Define equilibrium constant.

• The equilibrium constant relates the concentrations of products and reactants at equilibrium in a chemical reaction.

• The equilibrium constant is the rate at which a reaction occurs.

• Equilibrium constant is the total amount of products formed in a reaction.

• Equilibrium constant is the temperature at which a reaction reaches equilibrium.

How does temperature affect the equilibrium position?

• Temperature has no effect on the equilibrium position

• Temperature causes the equilibrium position to shift to the left

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

• Temperature increases the rate of reaction at equilibrium

Discuss the role of catalysts in chemical equilibrium.

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

• Catalysts only affect the forward reaction in chemical equilibrium.

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

• Catalysts have no impact on chemical equilibrium.

What is the significance of equilibrium in chemical reactions?

• Equilibrium in chemical reactions signifies a state where only the forward reaction occurs

• Equilibrium in chemical reactions signifies a state where reactants are completely consumed

• Equilibrium in chemical reactions signifies a state where the forward and reverse reactions occur at the same rate, leading to a constant concentration of reactants and products.

• Equilibrium in chemical reactions signifies a state where products are not formed

Describe the difference between homogeneous and heterogeneous equilibrium.

• Homogeneous equilibrium involves only reactants, while heterogeneous equilibrium involves only products.

• Homogeneous equilibrium involves all reactants and products being in the same physical state, while heterogeneous equilibrium involves reactants and products being in different physical states.

• Homogeneous equilibrium is reversible, while heterogeneous equilibrium is irreversible.

• Homogeneous equilibrium occurs at high temperatures, while heterogeneous equilibrium occurs at low temperatures.

Explain the concept of reversible reactions in chemical equilibrium.

• Reversible reactions only occur in one direction with no possibility of the products reverting back to the reactants.

• Chemical equilibrium involves the complete consumption of reactants with no products being formed.

• The forward reaction in reversible reactions always proceeds faster than the reverse reaction.

• Reversible reactions in chemical equilibrium involve the products being able to react to form the original reactants, with the rates of the forward and reverse reactions being equal at equilibrium.