Understanding Chemical Equilibrium: A Comprehensive Guide
Chemical equilibrium is a fundamental concept in chemistry that describes the balance between the forward and reverse reactions in a chemical system. It plays a crucial role in various chemical processes, from industrial production to biological systems. In this blog post, we will delve into the intricacies of chemical equilibrium by exploring a challenging exam question commonly encountered at the university level. Through detailed explanation and a step-by-step guide, we aim to provide clarity on this topic and help students grasp its nuances effectively.
Exam Question: Consider the following reversible reaction:
N₂O₄(g) ⇌ 2NO₂(g)
At a certain temperature, the equilibrium constant (Kc) for the reaction is 0.20 mol/L. If the initial concentration of N₂O₄(g) is…
At a certain temperature, the equilibrium constant (K_c) for the reaction is 0.200.20 mol/L. If the initial concentration of N₂O₄(g) is 0.300.30 mol/L, calculate the equilibrium concentrations of N₂O₄(g) and N₂O₄(g).
Concept Explanation: Chemical equilibrium is achieved when the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products over time. The equilibrium constant (K_c) is a numerical value that expresses the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to the power of its stoichiometric coefficient.
Step-by-Step Guide:
- Understanding the Given Data: In this question, we are provided with the equilibrium constant (K_c) and the initial concentration of N₂O₄(g)(g).
- Setting Up the Expression: The equilibrium expression for the given reaction is given by:
Kc= [(NO₂)²/(N₂O₄)](g)
where NO₂ and N₂O₄ represent the equilibrium concentrations of NO₂(g) and N₂O₄(g) respectively.
3. Substituting Values and Solving: We can substitute the known values into the equilibrium expression and solve for the unknown equilibrium concentrations.
0.20=(2x)²/(0.30-x)
Where x represents the change in concentration from the initial concentration of N₂O₄(g) to the equilibrium concentration.
4. Solving for x: After solving the equation, we can determine the value of x, which represents the change in concentration of N₂O₄(g) at equilibrium.
- Calculating Equilibrium Concentrations: Once we have found the value of x, we can use it to calculate the equilibrium concentrations of both N₂O₄(g) and NO₂(g) using the initial concentrations and the change in concentration.
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Conclusion:
Chemical equilibrium is a fundamental concept in chemistry that requires a clear understanding of equilibrium constants and the behavior of reversible reactions. By dissecting a challenging exam question and providing a step-by-step guide, we hope to have demystified this topic for students. With practice and perseverance, mastering chemical equilibrium is within reach, and our exam help website is here to support students every step of the way.
