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A 0.72-mol sample of PCl5 is put into a 1.00 L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3 (g) and 0.40 mol of Cl2 (g). Calculate the value of the equilibrium constant for the decomposition of PCl5 to PCl3 and Cl2 at this temperature.

A 0.72-mol sample of PCl5 is put into a 1.00 L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3 (g) and 0.40 mol of Cl2 (g). Calculate the value of the equilibrium constant for the decomposition of PCl5 to PCl3 and Cl2 at this temperature.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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A 0.72-mol sample of PCl5 is put into a 1.00 L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3 (g) and 0.40 mol of Cl2 (g). Calculate the value of the equilibrium constant for the decomposition of PCl5 to PCl3 and Cl2 at this temperature.
50. A reaction is represented by this equation: A(aq) + 2B(aq) = 2C(aq) K. = 1 x 103 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations s1 M, identify two sets of concentrations that describe a mixture of A, B, and C at equilibrium. 51. A reaction is represented by this equation: 2W(aq) = X(aq) + 2Y(aq) K. = 5 × 10-4 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of s1 M, identify two sets of concentrations that describe a mixture of W, X, and Y at equilibrium. 52. What is the value of the equilibrium constant at 500 °C for the formation of NH3 according to the following equation? N2(g) + 3H2(g) = 2NH3(g) An equilibrium mixture of NH3(g), H2G), and N2(g) at 500 °C was found to contain 1.35 M H2, 1.15 M N2, and 4.12 x 10-1 M NH3. 53. Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H20(g) = 3H2(g) + CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760 °C? 54. A 0.72-mol sample of PCI5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCI3(g) and 0.40 mol of Cl2g). Calculate the value of the equilibrium constant for the decomposition of PCI5 to PCI3 and Cl2 at this temperature. 55. At 1 atm and 25 °C, NO, with an initial concentration of 1.00 M is 0.0033% decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO,(g) = 2NO(g) + O2(g) 56. Calculate the value of the equilibrium constant Kp for the reaction 2NO(g) + Cl,(g) = 2NOCI(g) from these equilibrium pressures: NO, 0.050 atm; Cl2, 0.30 atm; NOCI, 1.2 atm. 57. When heated, iodine vapor dissociates according to this equation: I2(g) = 21(g) At 1274 K, a sample exhibits a partial pressure of l2 of 0.1122 atm and a partial pressure due to I atoms of 0.1378 atm.
Transcribed Image Text:50. A reaction is represented by this equation: A(aq) + 2B(aq) = 2C(aq) K. = 1 x 103 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations s1 M, identify two sets of concentrations that describe a mixture of A, B, and C at equilibrium. 51. A reaction is represented by this equation: 2W(aq) = X(aq) + 2Y(aq) K. = 5 × 10-4 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of s1 M, identify two sets of concentrations that describe a mixture of W, X, and Y at equilibrium. 52. What is the value of the equilibrium constant at 500 °C for the formation of NH3 according to the following equation? N2(g) + 3H2(g) = 2NH3(g) An equilibrium mixture of NH3(g), H2G), and N2(g) at 500 °C was found to contain 1.35 M H2, 1.15 M N2, and 4.12 x 10-1 M NH3. 53. Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H20(g) = 3H2(g) + CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760 °C? 54. A 0.72-mol sample of PCI5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCI3(g) and 0.40 mol of Cl2g). Calculate the value of the equilibrium constant for the decomposition of PCI5 to PCI3 and Cl2 at this temperature. 55. At 1 atm and 25 °C, NO, with an initial concentration of 1.00 M is 0.0033% decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO,(g) = 2NO(g) + O2(g) 56. Calculate the value of the equilibrium constant Kp for the reaction 2NO(g) + Cl,(g) = 2NOCI(g) from these equilibrium pressures: NO, 0.050 atm; Cl2, 0.30 atm; NOCI, 1.2 atm. 57. When heated, iodine vapor dissociates according to this equation: I2(g) = 21(g) At 1274 K, a sample exhibits a partial pressure of l2 of 0.1122 atm and a partial pressure due to I atoms of 0.1378 atm.
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