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Ch.15 - Chemical Equilibrium
All textbooksBrown 14th EditionCh.15 - Chemical EquilibriumProblem 33a
Chapter 15, Problem 33a

The equilibrium 2 NO(𝑔) + Cl2(𝑔) β‡Œ 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) β‡Œ 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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Key Concepts

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

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) β‡Œ 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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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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Related Practice
Open Question
Mercury(I) oxide decomposes into elemental mercury and elemental oxygen: 2 Hg2O(s) β‡Œ 4 Hg(l) + O2(g). (a) Write the equilibrium-constant expression for this reaction in terms of partial pressures. (b) Suppose you run this reaction in a solvent that dissolves elemental mercury and elemental oxygen. Rewrite the equilibrium-constant expression in terms of molarities for the reaction, using (solv) to indicate solvation.
Open Question
Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g) + 2 H2(g) β‡Œ CH3OH(g). An equilibrium mixture in a 2.00-L vessel is found to contain 0.0406 mol CH3OH, 0.170 mol CO, and 0.302 mol H2 at 500 K. Calculate Kc at this temperature.
Open Question
Gaseous hydrogen iodide is placed in a closed container at 425 Β°C, where it partially decomposes to hydrogen and iodine: 2 HI(g) β‡Œ H2(g) + I2(g). At equilibrium, it is found that [HI] = 3.53 Γ— 10⁻³ M, [H2] = 4.79 Γ— 10⁻⁴ M, and [I2] = 4.79 Γ— 10⁻⁴ M. What is the value of Kc at this temperature?
Textbook Question

The equilibrium 2 NO(𝑔) + Cl2(𝑔) β‡Œ 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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Textbook Question

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3(𝑔) + Cl2(𝑔) β‡Œ 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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Open Question
A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: 2 NO(g) + 2 H2(g) β‡Œ N2(g) + 2 H2O(g). At equilibrium [NO] = 0.062 M. (a) Calculate the equilibrium concentrations of H2, N2, and H2O.