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) + Cl2 (g) = PCI5 (g)Kc = 1.67 at 500 K2. At a particular temperature, a 3.0-L flask contains 2.4 moles of Cl2, 1.0 mole of NOCI, and 4.5 x 103mole 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 reaction2 NO2 (g) = 2NO (g) + O2 (g)PNO2 = 0.55 atmPNO = 6.5 x 10s atmPO2 = 4.5 x 10s atmCalculate the value for the equilibrium constant Kp at this temperature.4. The atmospheric oxidation of nitrogen monoxide, 2 NO (g) + O2 (g) s 2NO2 (g), was studied at 184°Cwith initial pressures of 1.00 atm of NO and 1.000 atm of O2. At equilibrium PO2 = 0.56 atm. CalculateКр.5. To study the reaction between ammonia and oxygen, 4 NH3 (g) + 7 O2 (g) = 2N2O4 (g) + 6 H20(g) aflask was filled with 2.40 M NH3 and 2.40 M O2 at a particular temperature; the reaction proceeds, andat equilibrium [N2O4] = 0.134 M. Calculate Kc.

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1. Calculate Kp for the following reaction: PCI: (g) + Cl2 (g)= PCI5 (g) Kc = 1.67 at 500 K

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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Question

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) + 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 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) s 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.

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