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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![Activity 2. Solve Me! (LAS 5.b)
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) + Ck (g) = PCI5 (g)
Kc = 1.67 at 500 K
2. At a particular temperature, a 3.0-L flask contains 2.4 moles of Cl, 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 10s 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 H2O(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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9abc4667-7ead-4031-92f5-19ac9871b525%2F7265ebf9-4982-4fcf-8cf0-cef5fdff600a%2Fd8n7t1_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Activity 2. Solve Me! (LAS 5.b)
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) + Ck (g) = PCI5 (g)
Kc = 1.67 at 500 K
2. At a particular temperature, a 3.0-L flask contains 2.4 moles of Cl, 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 10s 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 H2O(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.
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