Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

7. Energy, Rate and Equilibrium

The Equilibrium Constant

GOB Chemistry

7. Energy, Rate and Equilibrium

The Equilibrium Constant

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1:02 minutes

Problem 14a

Textbook Question

The following diagrams represent two similar reactions that have achieved equilibrium:
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a. Write the expression for the equilibrium constant for each reaction.

Verified step by step guidance

Identify the general form of the equilibrium constant expression. For a reaction of the form \( aA + bB \rightleftharpoons cC + dD \), the equilibrium constant \( K_{eq} \) is expressed as \( K_{eq} = \frac{[C]^c[D]^d}{[A]^a[B]^b} \), where the square brackets represent the concentrations of the species at equilibrium, and the exponents correspond to their stoichiometric coefficients.

Examine the first reaction diagram and determine the chemical equation it represents. Identify the reactants and products, as well as their stoichiometric coefficients.

Write the equilibrium constant expression for the first reaction using the general form \( K_{eq} = \frac{[products]}{[reactants]} \), substituting the appropriate species and their coefficients.

Repeat the process for the second reaction diagram. Determine the chemical equation, identify the reactants and products, and their stoichiometric coefficients.

Write the equilibrium constant expression for the second reaction using the same general form \( K_{eq} = \frac{[products]}{[reactants]} \), ensuring the correct species and coefficients are used.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It is calculated using the formula K = [products]^[coefficients] / [reactants]^[coefficients], where the brackets denote concentration. A large K value indicates a reaction that favors products, while a small K value suggests a preference for reactants.

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products over time. At this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentrations. Understanding this concept is crucial for writing equilibrium expressions accurately.

Stoichiometry

Stoichiometry is the study of the quantitative relationships between the amounts of reactants and products in a chemical reaction. It involves using the coefficients from a balanced chemical equation to determine the proportions of substances involved. This concept is essential for formulating the equilibrium constant expression, as the coefficients dictate how concentrations are raised to powers in the K expression.