1) Consider the following diagram for a chemical system containing three substances represented by $A, B$, and $C$ :
a) What feature of the graph indicates that the system reaches equilibrium? (1 marks)
b) Write a balanced equation for the equilibrium reaction. (2 marks)
c) Calculate the $K_{ ext {eq }}$ at equilibrium. ( 3 marks)

Question

1) Consider the following diagram for a chemical system containing three substances represented by $A, B$, and $C$ :
a) What feature of the graph indicates that the system reaches equilibrium? (1 marks)
b) Write a balanced equation for the equilibrium reaction. (2 marks)
c) Calculate the $K_{	ext {eq }}$ at equilibrium. ( 3 marks)

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Identify the equilibrium point**: The feature of the graph that indicates the system reaches equilibrium is the point where the concentrations of all substances become constant over time. ‖ ‖ 2 ⋮ **Determine the balanced equation**: To write a balanced equation for the equilibrium reaction, we need to consider the behavior of substances A, B, and C. Since A decreases and B and C increase, a possible reaction could be $A ightarrow B + C$. However, without additional information about the stoichiometry of the reaction, we can only assume the simplest form where the coefficients of all substances are 1. ‖ ‖ 3 ⋮ **Calculate the equilibrium constant $K_{ ext{eq}}$**: To calculate $K_{ ext{eq}}$, we need the equilibrium concentrations of A, B, and C. Assuming the graph provides these values at the plateau, we use the expression $K_{ ext{eq}} = \frac{[B]_{eq}[C]_{eq}}{[A]_{eq}}$. The exact values need to be read from the graph. If, for example, at equilibrium $[A]_{eq} = 0.40 \, ext{mol/L}$, $[B]_{eq} = 0.60 \, ext{mol/L}$, and $[C]_{eq} = 0.60 \, ext{mol/L}$, then $K_{ ext{eq}} = \frac{(0.60)(0.60)}{0.40}$. ‖ ∻1 Answer∻ ⚹ The graph indicates that the system reaches equilibrium when the concentrations of all substances become constant over time. ⚹ ∻Key Concept∻ ⚹ Equilibrium is reached when the concentrations of reactants and products remain constant over time. ⚹ ∻Explanation∻ ⚹ The graph shows that the concentrations of A, B, and C level off, indicating no further change and thus equilibrium. ⚹ ∻2 Answer∻ ⚹ The balanced equation for the equilibrium reaction is $A ightarrow B + C$. ⚹ ∻Key Concept∻ ⚹ A balanced chemical equation represents the conservation of mass in a reaction. ⚹ ∻Explanation∻ ⚹ Without additional information, the simplest whole number ratio of reactants to products is assumed to be 1:1:1. ⚹ ∻3 Answer∻ ⚹ Assuming the equilibrium concentrations are $[A]_{eq} = 0.40 \, ext{mol/L}$, $[B]_{eq} = 0.60 \, ext{mol/L}$, and $[C]_{eq} = 0.60 \, ext{mol/L}$, the equilibrium constant $K_{ ext{eq}}$ would be 0.90. ⚹ ∻Key Concept∻ ⚹ The equilibrium constant $K_{ ext{eq}}$ quantifies the ratio of product concentrations to reactant concentrations at equilibrium. ⚹ ∻Explanation∻ ⚹ The value of $K_{ ext{eq}}$ is calculated using the equilibrium concentrations of the reactants and products, which must be determined from the graph. ⚹◊What is the mathematical expression for the equilibrium constant $K_{eq}$ in a chemical reaction⍭ Generate me a similar question◊

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