Ch.15 - Chemical Equilibrium

Tro - Chemistry: A Molecular Approach 4th Edition

Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo

Tro 4th Edition

Ch.15 - Chemical Equilibrium

Problema 31a

Capitolo 15, Problema 31a

Calculate K_c for each reaction. a. I₂(g) ⇌ 2I(g) K_p = 6.26⨉10^-22 (at 298K)

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Identify the given values and the required conversion: You are given the equilibrium constant in terms of pressure (Kp) and need to calculate the equilibrium constant in terms of concentration (Kc) for the reaction at a specific temperature (298K).

Write down the balanced chemical equation for the reaction: I2(g) ⇌ 2I(g).

Use the relationship between Kp and Kc, which is Kp = Kc(RT)^Δn, where R is the gas constant (0.0821 L atm K^-1 mol^-1), T is the temperature in Kelvin, and Δn is the change in moles of gas (moles of products - moles of reactants).

Calculate Δn for the reaction: Δn = 2 (moles of I) - 1 (moles of I2) = 1.

Substitute the values of Kp, R, T, and Δn into the formula to solve for Kc: Kc = Kp / (RT)^Δn.

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Equilibrium Constant (Kc and Kp)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. Kc refers to concentrations in molarity, while Kp refers to partial pressures. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

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02:06

Kp vs. Kc Formula

Relationship Between Kc and Kp

Kc and Kp are related through the ideal gas law and the stoichiometry of the reaction. For reactions involving gases, the conversion between Kc and Kp depends on the difference in the number of moles of gaseous products and reactants. This relationship allows for the calculation of one constant if the other is known, provided the temperature remains constant.

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02:18

Kp vs Kc Relationship

Stoichiometry of the Reaction

Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction. In the given reaction, I2(g) ⇌ 2I(g), the stoichiometry indicates that one mole of iodine gas dissociates into two moles of iodine atoms. This stoichiometric ratio is crucial for calculating Kc from Kp, as it directly influences the value of Δn in the Kp-Kc relationship.

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01:16

Stoichiometry Concept

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Domanda del libro di testo

This reaction has an equilibrium constant of K_p = 2.2⨉10⁶ at 298 K. 2 COF₂(g) ⇌ CO₂(g) + CF₄(g) Calculate K_p for each reaction and predict whether reactants or products will be favored at equilibrium.

b. 6 COF₂(g) ⇌ 3 CO₂(g) + 3 CF₄(g)

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Domanda del libro di testo

Consider the reactions and their respective equilibrium

constants:

NO(g) + 1/2 Br (g) ⇌ NOBr(g) K_p = 5.3

2 NO(g) ⇌ N₂(g) + O₂(g) K_p = 2.1⨉10³⁰

Use these reactions and their equilibrium constants to predict

the equilibrium constant for the following reaction: N₂(g) + O₂(g) + Br₂(g) ⇌ 2 NOBr(g)

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