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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.15 - Chemical EquilibriumProblema 51a
Capitolo 15, Problema 51a

At 218°C, 𝐾𝑐 = 1.2×10−4 for the equilibrium NH4SH(𝑠) ⇌ NH3(𝑔) + H2S(𝑔) (a) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218°C and decomposes until equilibrium is reached.

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1
Identify the equilibrium expression for the reaction: NH_4SH(s) ⇌ NH_3(g) + H_2S(g). Since NH_4SH is a solid, it does not appear in the equilibrium expression. Therefore, K_c = [NH_3][H_2S].
Let x be the equilibrium concentration of NH_3 and H_2S. Since the stoichiometry of the reaction is 1:1, [NH_3] = x and [H_2S] = x at equilibrium.
Substitute the equilibrium concentrations into the equilibrium expression: K_c = x * x = x^2.
Set the equilibrium constant equal to the expression: 1.2 \(\times\) 10^{-4} = x^2.
Solve for x by taking the square root of both sides to find the equilibrium concentrations of NH_3 and H_2S.

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Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction NH₄SH(s) ⇌ NH₃(g) + H₂S(g), Kc = [NH₃][H₂S] / [NH₄SH]. Since NH₄SH is a solid, its concentration does not appear in the expression, simplifying the calculation of equilibrium concentrations.
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Equilibrium Constant Expressions

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. In this case, the introduction of solid NH₄SH will shift the equilibrium position to favor the formation of NH₃ and H₂S until the concentrations stabilize according to the Kc value.
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Le Chatelier's Principle

Stoichiometry of the Reaction

Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction. For the decomposition of NH₄SH, the stoichiometry indicates that one mole of NH₄SH produces one mole of NH₃ and one mole of H₂S. This relationship is crucial for calculating the equilibrium concentrations based on the initial amount of solid NH₄SH and the changes that occur as the system reaches equilibrium.
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Stoichiometry Concept
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At 80°C, 𝐾𝑐 = 1.87×10−3 for the reaction PH3BCl3(𝑠) ⇌ PH3(𝑔) + BCl3(𝑔) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80°C and decomposes until equilibrium is reached.

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At 80°C, 𝐾𝑐 = 1.87×10−3 for the reaction PH3BCl3(𝑠) ⇌ PH3(𝑔) + BCl3(𝑔) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80°C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the minimum mass of PH3BCl3(𝑠) that must be added to the flask to achieve equilibrium?

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