Textbook Question
Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium.
Sucrose(aq) + H2O(l) ⇌ Glucose(aq) + Fructose(aq) K = 1.4 x 10^5
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Ch.7 Chemical Reactions: Energy, Rate and Equilibrium
Chapter 7, Problem 14
The following diagrams represent two similar reactions that have achieved equilibrium: <
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Calculate the value for the equilibrium constant for each reaction.
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Count the number of each type of molecule in the diagram: A_2, B, and C_2.
Write the expression for the equilibrium constant (K_c) for the reaction: A_2 + 3B ⇌ 2C_2.
Substitute the concentrations (or counts) of A_2, B, and C_2 into the equilibrium expression.
Calculate the concentration of each species by dividing the number of molecules by the total volume (or area) if needed.
Use the concentrations to find the value of the equilibrium constant K_c.
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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 state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentration of substances involved.
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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.
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: <.>
Write the expression for the equilibrium constant for each reaction.
303
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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)
Allowing CH4 to escape continuously from the reaction vessel
303
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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)
Increasing pressure by decreasing volume
299
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