Is the question asking for something specific about the reaction: 2 H2S(g) + SO2(g) ⇌ 3 S(s) + 2 H2O(g)?

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Identify the type of chemical reaction. This is a reversible reaction, as indicated by the double arrow (⇌), meaning it can proceed in both forward and reverse directions.

Determine the stoichiometry of the reaction. The balanced equation shows that 2 moles of H2S react with 1 mole of SO2 to produce 3 moles of S and 2 moles of H2O.

Consider the states of matter for each component. H2S and SO2 are gases, S is a solid, and H2O is a gas in this reaction.

If the question is about equilibrium, consider the equilibrium constant expression (Kc or Kp) for the reaction. For this reaction, Kc = [H2O]^2 / ([H2S]^2 [SO2]), where the concentration of solids (S) is not included.

If the question involves Le Chatelier's Principle, analyze how changes in concentration, pressure, or temperature might shift the equilibrium position of the reaction.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the given reaction, the equilibrium position can shift in response to changes in concentration, temperature, or pressure, which is essential for understanding how the system behaves under different conditions.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced equation. For the reaction provided, stoichiometric coefficients indicate the molar ratios of H2S, SO2, S, and H2O, which are crucial for determining how much of each substance is consumed or produced at equilibrium.

Phase Changes

Phase changes refer to the transitions between solid, liquid, and gas states of matter. In the reaction, sulfur is produced as a solid (S), while water is in the gaseous state (H2O(g)). Understanding these phases is important for analyzing the physical state of reactants and products and their implications on reaction conditions and equilibrium.

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Related Practice

Textbook Question

Consider the exothermic reaction: C₂H₄(g) + Cl₂(g) ⇌ C₂H₄Cl₂(g) If you were trying to maximize the amount of C₂H₄Cl₂produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. increasing the reaction volume b. removing C₂H₄Cl₂from the reaction mixture as it forms c. lowering the reaction temperature d. adding Cl₂

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Textbook Question

Consider the endothermic reaction: C₂H₄(g) + I₂(g) ⇌ C₂H₄I₂(g) If you were trying to maximize the amount of C₂H₄I₂produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. decreasing the reaction volume b. removing I₂ from the reaction mixture c. raising the reaction temperature d. adding C₂H₄ to the reaction mixture

Textbook Question

Consider the reaction: H₂(g) + I₂(g) ⇌ 2 HI(g) A reaction mixture at equilibrium at 175 K contains P_H2 = 0.958 atm, P_I2 = 0.877 atm, and P_HI = 0.020 atm. A second reaction mixture, also at 175 K, contains P_H2 = P_I2 = 0.621 atm and P_HI = 0.101 atm. Is the second reaction at equilibrium? If not, what will be the partial pressure of HI when the reaction reaches equilibrium at 175 K?

Textbook Question

A reaction vessel at 27 °C contains a mixture of SO₂ (P = 3.00 atm) and O₂ (P = 1.00 atm). When a catalyst is added, this reaction takes place: 2 SO₂( g) + O₂( g) ⇌ 2 SO₃( g). At equilibrium, the total pressure is 3.75 atm. Find the value of K_c.

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