Podcast
Questions and Answers
What happens to a reaction if Q is less than K?
What happens to a reaction if Q is less than K?
According to Le Chatelier’s Principle, increasing the concentration of reactants will favor the formation of products.
According to Le Chatelier’s Principle, increasing the concentration of reactants will favor the formation of products.
True
When the reaction quotient Qc is greater than Kc, the reaction will shift to the _____ to reach equilibrium.
When the reaction quotient Qc is greater than Kc, the reaction will shift to the _____ to reach equilibrium.
left
Match the following factors to their effects on equilibrium:
Match the following factors to their effects on equilibrium:
Signup and view all the answers
What is the effect of increasing the pressure on the equilibrium position of the reaction PCl3 (g) + Cl2 (g) ⇌ PCl5 (g) based on Le Chatelier's Principle?
What is the effect of increasing the pressure on the equilibrium position of the reaction PCl3 (g) + Cl2 (g) ⇌ PCl5 (g) based on Le Chatelier's Principle?
Signup and view all the answers
An increase in temperature for an exothermic reaction will shift the equilibrium to the right.
An increase in temperature for an exothermic reaction will shift the equilibrium to the right.
Signup and view all the answers
In the context of the Haber Process, what are the main product and reactants involved?
In the context of the Haber Process, what are the main product and reactants involved?
Signup and view all the answers
According to Le Chatelier's Principle, if the concentration of Cl2 is increased, the reaction will shift to the ______ to counteract the change.
According to Le Chatelier's Principle, if the concentration of Cl2 is increased, the reaction will shift to the ______ to counteract the change.
Signup and view all the answers
Match the following factors with their effects on equilibrium position:
Match the following factors with their effects on equilibrium position:
Signup and view all the answers
What effect does adding heat have on an exothermic reaction at equilibrium?
What effect does adding heat have on an exothermic reaction at equilibrium?
Signup and view all the answers
Adding an inert gas at constant volume affects the equilibrium position of a reaction.
Adding an inert gas at constant volume affects the equilibrium position of a reaction.
Signup and view all the answers
In the reaction N2O4 (g) ⇌ 2 NO2 (g), what happens when the temperature is increased?
In the reaction N2O4 (g) ⇌ 2 NO2 (g), what happens when the temperature is increased?
Signup and view all the answers
In an exothermic reaction, increasing the temperature will cause the equilibrium to shift to the ______.
In an exothermic reaction, increasing the temperature will cause the equilibrium to shift to the ______.
Signup and view all the answers
Match each substance with its property in equilibrium:
Match each substance with its property in equilibrium:
Signup and view all the answers
Which of the following statements about catalysts in chemical equilibrium is true?
Which of the following statements about catalysts in chemical equilibrium is true?
Signup and view all the answers
What occurs when CO2 is added to the equilibrium reaction H2 (g) + CO2 (g) ⇌ H2O (g) + CO (g)?
What occurs when CO2 is added to the equilibrium reaction H2 (g) + CO2 (g) ⇌ H2O (g) + CO (g)?
Signup and view all the answers
The value of Kc for an exothermic reaction increases with increasing temperature.
The value of Kc for an exothermic reaction increases with increasing temperature.
Signup and view all the answers
Study Notes
Chemical Equilibrium (FCH0216) Semester 1, Chapter 6
-
Objectives:
- Explain chemical equilibrium, equilibrium constant and reaction quotient.
- Use equilibrium constants to describe systems at equilibrium.
- Identify factors affecting equilibrium and predict resulting effects.
- Apply the relationship between Kc and Kp.
- Describe heterogeneous equilibrium and write their equilibrium constant.
Outline
- 6.1 Chemical equilibrium
- 6.2 Dynamic equilibrium
- 6.3 Equilibrium constant
- 6.4 Reaction Quotient
- 6.5 Le Chatelier's Principle
- 6.6 Haber Process
6.1 Chemical Equilibrium
- Chemical reactions progress when reactant concentration decreases and product concentration increases over time.
- Irreversible reactions: Complete conversion of reactants to products.
- Reversible reactions: Can proceed in both forward and reverse directions (⇌).
- Chemical equilibrium: A state where the concentrations of reactants and products remain constant, and the rate of the forward reaction equals the rate of the reverse reaction.
- Equilibrium is indicated by a double-headed arrow.
- indicates concentrations.
6.2 Dynamic Equilibrium
- Equilibrium is a dynamic process; reactions do not stop.
- Reactants and products continuously react in both forward and reverse directions at the same rate.
- Equilibrium is characterized by constant concentrations of reactants and products.
6.3 Equilibrium Constant (Kc)
- Equilibrium constant (Kc): A measure of the relative amounts of products and reactants at equilibrium. It's a numerical value that remains constant for a particular reaction at a given temperature.
- For a reaction aA + bB ⇌ cC + dD, Kc = [C]c[D]d / [A]a[B]b.
- If the reaction involves gases, the equilibrium constant can also be expressed in terms of partial pressures (Kp).
- Units of concentration: mol/L
- Unit of partial pressure: atm
6.4 Reaction Quotient (Q)
- The reaction quotient (Q) is a numerical value that can be calculated at any given time during a reaction.
- It helps predict the direction a reaction must proceed to reach equilibrium if its value is calculated using initial concentrations. Qc < Kc, reactions proceed from left to right, Qc = Kc, the reaction is at equilibrium, and Qc > Kc, reactions proceed from right to left.
6.5 Le Chatelier's Principle
- If a stress (change in concentration, pressure, or temperature) is applied to a system in equilibrium, the system will shift to relieve that stress.
- The system may shift towards formation of products or reactants.
- Factors influencing equilibrium: Concentration changes, Pressure changes, Temperature changes, Addition of a catalyst, Addition of inert gases
- Changes in temperature affect K, while other factors do not.
6.6 Haber Process
-
The Haber process is used to manufacture ammonia industrially.
-
The reaction represents a crucial industrial process.
-
N₂(g) + 3H₂(g) ⇌ 2NH₃(g) (ΔH = -ve).
-
Conditions for efficient ammonia production: High pressure, appropriate temperature and appropriate catalyst for efficient manufacturing in industry.
Other Details
- ICE tables and calculations to determine concentrations or pressures at equilibrium.
- Examples of chemical reactions, calculation of K and Kp.
- Importance of heterogeneous equilibrium; concentration terms of pure liquid and pure solids are not included.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
Explore the concepts of chemical equilibrium, including the equilibrium constant and reaction quotient in this quiz. Understand dynamic equilibrium, factors affecting equilibrium, and Le Chatelier's Principle through practical examples and applications. Perfect for students diving into Chapter 6 of their chemistry course.
