Hydrogen sulfide decomposes according to the following react reaction, for which Kr​=930×10

Question

Hydrogen sulfide decomposes according to the following reaction, for which Kr​=930×10−K at 700 ” C : 2H2​ S( g)⇌2H2​( g)+S2​( g) If 0.35 mol of H2​ S is placed in a 3.0−L container, what is the equilibrium concentration of H2​( g) at 700∘C7 Be sure your answer has the correct number of significant figures: [H2​]=M

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Answer

Solving Equilibrium Problems: Hydrogen Sulfide Decomposition at 700°C

Introduction

Chemical equilibrium serves as the cornerstone of many chemical processes, providing invaluable insights into the behavior of reacting systems. It describes a dynamic state where the rates of forward and reverse reactions reach a balance, resulting in the establishment of constant concentrations of reactants and products. Equilibrium problems, like the one we’re about to explore involving the decomposition of hydrogen sulfide at 700°C, offer an opportunity to apply equilibrium principles and mathematical techniques to unravel the intricacies of chemical systems. Through careful analysis and problem-solving, we can uncover the factors influencing reaction equilibrium and gain a deeper appreciation for the dynamic nature of chemical reactions.

Understanding the Reaction

The decomposition of hydrogen sulfide (H2S) at high temperatures, such as 700°C, represents a reversible chemical process governed by equilibrium dynamics. The reaction can be represented by the equation: 2H2S(g) ⇌ 2H2(g) + S2(g). Here, hydrogen sulfide breaks down into hydrogen gas (H2) and sulfur (S2) molecules. However, under equilibrium conditions, the forward and reverse reactions occur simultaneously, resulting in a balance between the formation and decomposition of hydrogen sulfide.

At elevated temperatures, hydrogen sulfide undergoes thermal decomposition, leading to the formation of hydrogen gas and elemental sulfur. This process is of particular interest in various industrial applications, including the production of hydrogen gas and sulfur recovery from hydrogen sulfide-containing streams. By studying the equilibrium behavior of this reaction, scientists and engineers can optimize process conditions and maximize product yields, contributing to the efficiency and sustainability of chemical processes.

Given Data and Initial Conditions

We are provided with the following information:

  • Initial moles of hydrogen sulfide (H2S): 0.35 mol
  • Volume of the container: 3.0 L
  • Equilibrium constant (Kr) at 700°C: 930 × 10^(-K)

Approach to Problem Solving

To solve this equilibrium problem, we will employ the following steps:

  1. Calculate the initial concentration of hydrogen sulfide (H2S) using the given moles and volume.
  2. Set up an ICE (Initial, Change, Equilibrium) table to track the changes in concentrations of reactants and products.
  3. Use the equilibrium constant expression to write an equation relating the concentrations of reactants and products at equilibrium.
  4. Substitute the given values and unknowns into the equilibrium constant expression and solve for the equilibrium concentration of hydrogen gas (H2).
  5. Verify the result for accuracy and ensure the correct number of significant figures in the final answer.

Conclusion

Solving equilibrium problems, such as the decomposition of hydrogen sulfide at 700°C, requires a systematic approach and a deep understanding of equilibrium principles. Through careful analysis and mathematical manipulation, we can unravel the complex interplay of reactants and products in chemical systems and predict their behavior under specific conditions. Equilibrium problems not only serve as a valuable tool for honing problem-solving skills but also offer insights into the fundamental principles governing chemical reactions.

By mastering the techniques of equilibrium analysis, students and researchers alike can tackle a wide range of real-world challenges, from designing efficient chemical processes to optimizing reaction conditions for maximum yield. Equilibrium problems provide a bridge between theoretical knowledge and practical applications, fostering a deeper appreciation for the dynamic nature of chemical systems and their role in shaping the world around us. As we continue to explore and apply equilibrium concepts, we contribute to the advancement of science and technology, paving the way for innovation and discovery in the field of chemistry.

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