10.1.1 Characteristics of Dynamic Equilibrium

• Reversible reactions are chemical reactions that can proceed in both forward and reverse directions.
• At equilibrium, the concentrations of reactants and products remain constant in a reversible reaction.
• Reversible reactions differ from unidirectional reactions in that they can have products turning back into reactants.
• Equilibrium is reached in a reversible reaction when the forward and reverse reaction rates are equal.
• Match the reaction characteristic with its type:

  Direction | Reversible Reaction ↔️ Proceeds in both forward and reverse directions

  Completion | Irreversible Reaction ↔️ Goes to completion

  Symbol | Reversible Reaction ↔️ $\rightleftharpoons$
• Reversible reactions go to completion, meaning all reactants are converted to products.

  False
• Dynamic equilibrium occurs when the forward and reverse reaction rates are equal.
• Order the reaction characteristics by type:

  1️⃣ Direction: Reversible Reaction - Proceeds in both forward and reverse directions

  2️⃣ Completion: Irreversible Reaction - Goes to completion

  3️⃣ Equilibrium: Reversible Reaction - Equilibrium is established

  4️⃣ Symbol: Irreversible Reaction - $\rightarrow$
• Irreversible reactions establish an equilibrium state.

  False
• Dynamic equilibrium demonstrates continuous activity at a molecular level.
• Match the condition necessary for dynamic equilibrium with its description:

  Closed System ↔️ No reactants or products can enter or leave the system

  Constant Temperature ↔️ Maintains stable reaction rates

  Equal Forward and Reverse Rates ↔️ Reaction rates are balanced
• A closed system is required for dynamic equilibrium because no reactants or products can enter or leave the system.
• What is a closed system in the context of dynamic equilibrium?

  No matter exchange
• Maintaining a constant temperature is necessary for dynamic equilibrium because it keeps reaction rates stable.
• For dynamic equilibrium, the rates of the forward and reverse reactions must be equal
• Why does a constant temperature prevent changes in reaction rates during dynamic equilibrium?

  Keeps reaction rates stable
• Order the steps to describe the equal rates in dynamic equilibrium.

  1️⃣ Reactants are converted to products

  2️⃣ Products are converted back to reactants

  3️⃣ Forward rate equals reverse rate
• Reversible reactions can proceed in both the forward and reverse directions
• What happens to the concentrations of reactants and products at equilibrium in a reversible reaction?

  They remain constant
• Match the characteristics with the type of reaction.

  Proceeds in both directions ↔️ Reversible reaction

  Goes to completion ↔️ Irreversible reaction
• In dynamic equilibrium, the forward and reverse reaction rates are equal, but the concentrations of reactants and products may differ.
• What is a closed system necessary for dynamic equilibrium?

  No matter exchange
• The equilibrium position indicates whether the equilibrium is shifted towards the reactants or the products
• What is the key difference between reversible and unidirectional reactions?

  Direction
• Reversible reactions allow reactants to form products and products to turn back into reactants
• Reversible reactions go to completion.

  False
• Match the type of reaction with its characteristic:

  Reversible Reaction ↔️ Proceeds in both directions

  Irreversible Reaction ↔️ Proceeds only in one direction
• Dynamic equilibrium is a state where the forward and reverse reaction rates are equal
• At dynamic equilibrium, the concentrations of reactants and products remain constant.
• Conditions necessary for dynamic equilibrium to be established:

  1️⃣ Closed System

  2️⃣ Constant Temperature

  3️⃣ Equal Forward and Reverse Rates
• A closed system allows the exchange of matter with the surroundings.

  False
• The forward reaction rate is the speed at which reactants form products
• Le Chatelier's principle states that a system in equilibrium will shift to relieve stress.
• Adding reactants to a system in equilibrium shifts the equilibrium towards products
• Increasing pressure in a system favors the side with more moles of gas.

  False