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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 26a
Capitolo 15, Problema 26a

Consider the following equilibrium, for which at 𝐾𝑝 = 0.0752 at 480°C: 2 Cl2(𝑔) + 2 H2O(𝑔) ⇌ 4 HCl(𝑔) + O2(𝑔) (a) What is the value of 𝐾𝑝 for the reaction 4 HCl(𝑔) + O2(𝑔) ⇌ 2 Cl2(𝑔) + 2 H2O(𝑔)?

Guida verificata passo dopo passo
1
Identify that the given reaction is the reverse of the original reaction.
Recall that the equilibrium constant for a reverse reaction is the reciprocal of the equilibrium constant for the forward reaction.
Write the expression for the equilibrium constant of the reverse reaction as 1/K_p.
Substitute the given K_p value of 0.0752 into the expression for the reverse reaction.
Calculate the reciprocal to find the K_p for the reverse reaction.

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Equilibrium Constant (Kp)

The equilibrium constant, Kp, 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. It is calculated using the partial pressures of gases involved in the reaction. A Kp value less than 1 indicates that at equilibrium, reactants are favored, while a value greater than 1 indicates that products are favored.
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Equilibrium Constant Expressions

Reversibility of Reactions

Chemical reactions can proceed in both forward and reverse directions, and the equilibrium constant for the reverse reaction is the reciprocal of the forward reaction's equilibrium constant. This means that if you know Kp for a reaction, you can easily find Kp for the reverse reaction by taking the inverse of that value. This principle is crucial for solving equilibrium problems.
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Reversible Changes in Matter

Stoichiometry in Equilibrium

Stoichiometry refers to the quantitative relationship between reactants and products in a chemical reaction, as represented by the balanced equation. In equilibrium expressions, the coefficients of the balanced equation become the exponents in the Kp expression. Understanding stoichiometry is essential for accurately calculating equilibrium constants and predicting the direction of the reaction.
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Stoichiometry Concept
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Domanda del libro di testo

At 1000 K, 𝐾𝑝 = 1.85 for the reaction SO2(𝑔) + 12 O2(𝑔) ⇌ SO3(𝑔) (c) What is the value of 𝐾𝑐 for the reaction in part (b)?

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Domanda del libro di testo

Consider the equilibrium N2(𝑔) + O2(𝑔) + Br2(𝑔) ⇌ 2 NOBr(𝑔) Calculate the equilibrium constant 𝐾𝑝 for this reaction, given the following information at 298 K:

2 NO(𝑔) + Br2(𝑔) ⇌ 2 NOBr(𝑔) 𝐾𝑐 = 2.02

NO(𝑔) ⇌ N2(𝑔) + O2(𝑔) 𝐾𝑐 = 2.1×1030

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Domanda del libro di testo

Consider the following equilibrium: 2 H2(g) + S2(g) ⇌ 2 H2S(g) Kc = 1.08 × 107 at 700°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H2(g) + 1/2 S2(g) ⇌ H2S(g)

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Domanda del libro di testo

The following equilibria were attained at 823 K:

CoO(s) + H2(g) → Co(s) + H2O(g) Kc = 67

CoO(s) + CO(g) → Co(s) + CO2(g) Kc = 490

Based on these equilibria, calculate the value of 𝐾𝑐 for H2(𝑔)+ CO2(𝑔) ⇌ CO(𝑔) + H2O(𝑔) at 823 K.