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Ch.16 - Chemical Equilibrium
Chapter 16, Problem 22a

Find and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]

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Key Concepts

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

Equilibrium Constant Expression

The equilibrium constant expression (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. It is derived from the balanced chemical equation, where the concentrations of gaseous and aqueous species are included, while solids and liquids are omitted. The general form is K = [products]^[coefficients] / [reactants]^[coefficients].
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Stoichiometry in Chemical Reactions

Stoichiometry involves the quantitative relationships between the amounts of reactants and products in a chemical reaction, as dictated by the balanced equation. Each species in the reaction is represented by its coefficient, which indicates the proportion in which they react or are produced. Correct stoichiometric coefficients are essential for accurately writing the equilibrium constant expression.
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Gaseous Equilibrium and Partial Pressures

In reactions involving gases, the equilibrium constant can also be expressed in terms of partial pressures instead of concentrations. The relationship between concentration and partial pressure is given by the ideal gas law, where pressure is proportional to concentration. For gaseous reactions, Kp is used, and it is related to Kc (the concentration-based equilibrium constant) through the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas.
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