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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 33a
Capitolo 15, Problema 33a

The equilibrium 2 NO(𝑔) + Cl2(𝑔) ⇌ 2 NOCl(𝑔) is established at 500.0 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (a) Calculate 𝐾𝑝 for this reaction at 500.0 K.

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Identify the balanced chemical equation: 2 NO(g) + Cl_2(g) ⇌ 2 NOCl(g).
Write the expression for the equilibrium constant K_p for the reaction: K_p = (P_NOCl^2) / (P_NO^2 * P_Cl2).
Substitute the given equilibrium partial pressures into the K_p expression: P_NO = 0.095 atm, P_Cl2 = 0.171 atm, and P_NOCl = 0.28 atm.
Calculate the numerator of the K_p expression: (P_NOCl)^2.
Calculate the denominator of the K_p expression: (P_NO)^2 * P_Cl2.

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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 this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentrations of the substances involved.
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Chemical Equilibrium Concepts

Equilibrium Constant (Kp)

The equilibrium constant, Kp, is a numerical value that expresses the ratio of the partial pressures of the products to the partial pressures of the reactants at equilibrium, each raised to the power of their coefficients in the balanced equation. For the reaction 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g), Kp is calculated using the formula Kp = (P_NOCl^2) / (P_NO^2 * P_Cl2), where P represents the partial pressures of the gases.
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Equilibrium Constant Expressions

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In equilibrium calculations, knowing the partial pressures of each gas allows for the determination of the equilibrium constant.
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Partial Pressure Calculation
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Domanda del libro di testo

The equilibrium 2 NO(𝑔) + Cl2(𝑔) ⇌ 2 NOCl(𝑔) is established at 500.0 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.

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Domanda del libro di testo

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3(𝑔) + Cl2(𝑔) ⇌ PCl5(𝑔). A 7.5-L gas vessel is charged with a mixture of PCl3(𝑔) and Cl2(𝑔), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are 𝑃PCl3 = 0.124 atm, 𝑃Cl2 = 0.157 atm, and 𝑃PCl5 = 1.30 atm. (a) What is the value of 𝐾𝑝 at this temperature?

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