Textbook Question
Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium.
a. Sucrose(aq) + H2O(l) ⇌ Glucose(aq) + Fructose(aq) K = 1.4 × 105
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Ch.7 Chemical Reactions: Energy, Rate and Equilibrium
McMurry8th EditionFundamentals of GOBISBN: 9780134015187
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Table of contents
- Ch.1 Matter and Measurements27
- Ch.2 Atoms and the Periodic Table20
- Ch.3 Ionic Compounds8
- Ch.4 Molecular Compounds23
- Ch.5 Classification & Balancing of Chemical Reactions12
- Ch.6 Chemical Reactions: Mole and Mass Relationships28
- Ch.7 Chemical Reactions: Energy, Rate and Equilibrium64
- Ch.8 Gases, Liquids and Solids24
- Ch.9 Solutions52
- Ch.10 Acids and Bases25
- Ch.11 Nuclear Chemistry22
- Ch.12 Introduction to Organic Chemistry: Alkanes57
- Ch.13 Alkenes, Alkynes, and Aromatic Compounds47
- Ch.14 Some Compounds with Oxygen, Sulfur, or a Halogen50
- Ch.15 Aldehydes and Ketones45
- Ch.16 Amines42
- Ch.17 Carboxylic Acids and Their Derivatives57
- Ch.18 Amino Acids and Proteins82
- Ch.19 Enzymes and Vitamins63
- Ch.20 Carbohydrates44
- Ch.21 The Generation of Biochemical Energy65
- Ch.22 Carbohydrate Metabolism45
- Ch.23 Lipids42
- Ch.24 Lipid Metabolism33
- Ch.25 Protein and Amino Acid Metabolism24
- Ch.26 Nucleic Acids and Protein Synthesis45
Chapter 7, Problem 14b
The following diagrams represent two similar reactions that have achieved equilibrium:
<IMAGE>
b. Calculate the value for the equilibrium constant for each reaction.
Verified step by step guidance1
Step 1: Identify the chemical equation provided in the diagram. The reaction is A₂ + 3 B ⇌ 2 C₂, where A₂ represents blue molecules, B represents green molecules, and C₂ represents orange molecules.
Step 2: Count the number of molecules for each species in the diagram. For A₂, count the blue pairs; for B, count the green single molecules; and for C₂, count the orange pairs.
Step 3: Write the expression for the equilibrium constant (K_eq) based on the balanced chemical equation. The formula is: K_eq = ([C₂]^2) / ([A₂] × [B]^3), where the concentrations are proportional to the number of molecules.
Step 4: Substitute the counts of molecules into the equilibrium constant expression. Use the counts from Step 2 to represent the concentrations of A₂, B, and C₂.
Step 5: Simplify the expression to calculate the equilibrium constant. Ensure that the values are plugged in correctly and follow the rules of exponents and division.
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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 = [C]^c / ([A]^a * [B]^b), where [C], [A], and [B] are the molar concentrations of the products and reactants, and a, b, and c are their respective coefficients in the balanced equation.
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The Equilibrium Constant Concept 1
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 point, the system is in a state of balance, and any changes in concentration, temperature, or pressure can shift the equilibrium position according to Le Chatelier's principle.
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Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It involves using the coefficients of the balanced equation to determine the proportions of substances involved, which is essential for calculating the equilibrium constant and understanding the relationships between different species in a reaction.
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Related Practice
Textbook Question
Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium.
c. Fe2O3(s) + 3 CO(g) ⇌ 2 Fe(s) + 3 CO2(g) K (at 727 °C) = 24.2
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Textbook Question
The following diagrams represent two similar reactions that have achieved equilibrium:
<IMAGE>
a. Write the expression for the equilibrium constant for each reaction.
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Textbook Question
Is the yield of SO3 at equilibrium favored by a higher or lower pressure? By a higher or lower temperature?
2 SO2(g) + O2 ⇌ 2 SO3(g) ∆H = -47 kcal/mol
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Textbook Question
What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?
C(s) + 2 H2(g) ⇌ CH4(g) ∆H = -18 kcal/mol (-75kJ/mol)
a. Increasing temperature
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Textbook Question
What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?
C(s) + 2 H2(g) ⇌ CH4(g) ∆H = -18 kcal/mol (-75kJ/mol)
b. Increasing pressure by decreasing volume
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