3️⃣ Reactants convert to products at same rate products revert to reactants
Dynamic equilibrium is a state where the rate of the forward reaction equals the rate of the reverse reaction, leading to no net change in the concentrations of reactants and products.forward
Match the direction of the reaction with its corresponding process:
Forward Reaction ↔️ Reactants to Products
Reverse Reaction ↔️ Products to Reactants
The equilibrium constant, denoted as K, is a quantitative measure of the position of chemical equilibrium
What is the equilibrium constant related to in terms of reaction rates?
Ratio of rate constants
What effect does high temperature have on the Haber-Bosch process?
Decreases ammonia yield
What type of equilibrium does a hanging object represent?
Static equilibrium
Dynamic equilibrium is a state where the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations
Double arrows in a diagram indicate that both forward and reverse reactions are occurring simultaneously at the same rate.
True
The forward reaction in the equilibrium N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g) forms ammonia.
True
In dynamic equilibrium, the rates of the forward and reverse reactions are constant.
True
What does the equilibrium constant (K) measure in a chemical equilibrium?
Position of equilibrium
Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction
In the equilibrium A + B ⇌ C + D, both reactions maintain constant concentrations of reactants and products.
True
What is the equilibrium constant related to at equilibrium?
Forward and reverse rates
In dynamic equilibrium, both forward and reverse reactions occur simultaneously at the same speed.
True
What remains constant in dynamic equilibrium over time?
Concentrations of reactants and products
A large value of K indicates that the reaction favors the products.
True
Order the effects of temperature, pressure, and catalysts on dynamic equilibrium:
1️⃣ Temperature shifts equilibrium according to endothermic or exothermic changes
2️⃣ Pressure shifts equilibrium based on gas molecules
3️⃣ Catalysts speed up reactions without changing equilibrium position
In the Haber-Bosch process, high pressure favors ammonia production.
Dynamic equilibrium maintains constant concentrations of reactants and products because forward and reverse reactions occur at equal rates.