Learning Objectives: Solve problems involving equilibrium constant. What you need: Pen, paper and calculator. What to do: Solve the following problems. Write your solutions in a separate sheet of paper. 1. Calculate Kp for the following reaction: PCI: (g) + Cl2 (g) = PCI5 (g) Kc = 1.67 at 500 K 2. At a particular temperature, a 3.0-L flask contains 2.4 moles of Cl2, 1.0 mole of NOCI, and 4.5 x 103 mole of NO. Calculate K at this temperature for the following reaction: 2 NOCI (g) = 2NO (g) + Cl2 (g) 3. The following equilibrium pressures at a certain temperature were observed for the reaction 2 NO2 (g) = 2NO (g) + O2 (g) PNO2 = 0.55 atm PNO = 6.5 x 10s atm PO2 = 4.5 x 10 atm Calculate the value for the equilibrium constant Kp at this temperature. 4. The atmospheric oxidation of nitrogen monoxide, 2 NO (g) + O2 (g) – 2NO2 (g), was studied at 184°C with initial pressures of 1.00 atm of NO and 1.000 atm of O2. At equilibrium PO2 = 0.56 atm. Calculate Кр. 5. To study the reaction between ammonia and oxygen, 4 NH3 (g) + 7 O2 (g) = 2N2O4 (g) + 6 H20(g) a flask was filled with 2.40 M NH3 and 2.40 M O2 at a particular temperature; the reaction proceeds, and at equilibrium [N2O4] = 0.134 M. Calculate Kc.

Learning Objectives: Solve problems involving equilibrium constant. What you need: Pen, paper and calculator. What to do: Solve the following problems. Write your solutions in a separate sheet of paper. 1. Calculate Kp for the following reaction: PCI: (g) + Cl2 (g) = PCI5 (g) Kc = 1.67 at 500 K 2. At a particular temperature, a 3.0-L flask contains 2.4 moles of Cl2, 1.0 mole of NOCI, and 4.5 x 103 mole of NO. Calculate K at this temperature for the following reaction: 2 NOCI (g) = 2NO (g) + Cl2 (g) 3. The following equilibrium pressures at a certain temperature were observed for the reaction 2 NO2 (g) = 2NO (g) + O2 (g) PNO2 = 0.55 atm PNO = 6.5 x 10s atm PO2 = 4.5 x 10 atm Calculate the value for the equilibrium constant Kp at this temperature. 4. The atmospheric oxidation of nitrogen monoxide, 2 NO (g) + O2 (g) – 2NO2 (g), was studied at 184°C with initial pressures of 1.00 atm of NO and 1.000 atm of O2. At equilibrium PO2 = 0.56 atm. Calculate Кр. 5. To study the reaction between ammonia and oxygen, 4 NH3 (g) + 7 O2 (g) = 2N2O4 (g) + 6 H20(g) a flask was filled with 2.40 M NH3 and 2.40 M O2 at a particular temperature; the reaction proceeds, and at equilibrium [N2O4] = 0.134 M. Calculate Kc.

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 121CP: If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration...

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