5.3 Dynamic Equilibria and Calculations Involving Gases

• What happens to the rates of the forward and reverse reactions at dynamic equilibrium?

  They are equal
• Define dynamic equilibrium in a closed system.

  Forward rate equals reverse rate
• In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the concentrations of nitrogen and hydrogen initially?

  They decrease
• What is the core characteristic of dynamic equilibrium in terms of reaction rates?

  Forward equals reverse rate
• The relative amounts of reactants and products at equilibrium are referred to as the equilibrium position
• What is the relationship between the rates of the forward and reverse reactions at equilibrium?

  Equal
• What happens to the concentrations of reactants and products once equilibrium is reached?

  Remain constant
• Why are the rates of the forward and reverse reactions equal at equilibrium?

  Reactants and products interchange
• Order the factors affecting dynamic equilibrium with their effects:

  1️⃣ Concentration: Increasing reactant concentration shifts equilibrium towards products

  2️⃣ Temperature: Increasing temperature shifts towards endothermic side

  3️⃣ Pressure: Increasing pressure shifts towards side with fewer gas molecules
• Increasing reactant concentration shifts equilibrium towards products
• How does increasing pressure affect equilibrium?

  Shifts towards fewer gas molecules
• Increasing temperature in the reaction N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) favors the reactants.


  True
• What is the definition of Kc?

  Ratio of product concentrations
• The relationship between Kc and Kp is $K_{p} =$$K_{c}(RT)^{\Delta n}$, where Δn is the change in the number of moles of gas.


  True
• Match the reaction direction with its rate at equilibrium:

  Forward Reaction ↔️ Equal to the rate of the reverse reaction

  Reverse Reaction ↔️ Equal to the rate of the forward reaction
• What does it mean when reactant and product concentrations are constant at equilibrium?

  Amounts no longer change
• What does the equilibrium position describe?

  Relative amounts of reactants and products
• Decreasing temperature shifts the equilibrium towards the exothermic side.


  True
• Increasing the temperature in the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) favors the reactants because the reverse reaction is endothermic.

  True
• In dynamic equilibrium, the concentrations of reactants and products remain constant.

  True
• Match the reaction direction with its rate at equilibrium:

  Forward Reaction ↔️ Equal to the reverse reaction rate

  Reverse Reaction ↔️ Equal to the forward reaction rate
• In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), the concentrations of all substances stabilize once equilibrium
• In what type of system must dynamic equilibrium occur?

  Closed system
• Dynamic equilibrium occurs when the rate of the forward reaction is equal to the rate of the reverse reaction.

  True
• At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction
• Dynamic equilibrium can only occur in a closed system
• The equilibrium position describes the relative amounts of reactants and products at equilibrium.


  True
• What three factors influence dynamic equilibrium?

  Concentration, temperature, pressure
• Increasing temperature shifts equilibrium towards the exothermic side.

  False
• In the reaction N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g), increasing nitrogen concentration shifts equilibrium towards ammonia
• Match the factor with its effect on equilibrium:

  Concentration ↔️ Shifts towards products or reactants

  Temperature ↔️ Shifts towards endothermic or exothermic side

  Pressure ↔️ Shifts towards fewer gas molecules
• Kp is defined as the ratio of the partial pressures of products to the partial pressures of reactants
• What defines dynamic equilibrium in a closed system?

  Forward rate equals reverse rate
• In dynamic equilibrium, the concentrations of reactants and products remain constant
• Dynamic equilibrium must occur in a closed system to maintain equilibrium conditions.


  True
• Dynamic equilibrium can be influenced by changes in concentration, temperature, and pressure
• Increasing the concentration of nitrogen in the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) shifts the equilibrium towards the production of ammonia
• Increasing the pressure in the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) shifts the equilibrium towards the side with fewer gas molecules
• The relationship between Kc and Kp is expressed as K_{p} = K_{c}(RT)^{\Delta n}</latex>, where Δn is the change in the number of moles of gas
• In the ideal gas law, pressure is measured in Pascals (Pa) or atmospheres