PROBLEMS IN CHEMICAL EQUILIBRIUM

PROBLEMS IN CHEMICAL EQUILIBRIUM:

1. Write the Keq expression for each of the following reaction.

a.

b.

c.

d.

e.

2. Calculate the value of Kp for the following reaction, at 333 K.

3. Calculate the value of Kc at 373 K for the following reaction:

4. Calculate the value of the equilibrium constant, Kc , for the system shown, if 0.1908 moles of CO2, 0.0908 moles of H2, 0.0092 moles of CO, and 0.0092 moles of H2O vapor were present in a 2.00 L reaction vessel were present at equilibrium.

5. Initially, a mixture of 0.100 M NO, 0.050 M H2, 0.100 M H2O was allowed to reach equilibrium (initially there was no N2). At equilibrium the concentration of NO was found to be 0.062 M. Determine the value of the equilibrium constant, Kc and KP, for the reaction:

6. A flask is charged with 3.00 atm of dinitrogen tetroxide gas and 2.00 atm of nitrogen dioxide gas at 25oC and allowed to reach equilibrium. It was found that the pressure of the nitrogen dioxide increased by 0.952 atm. Estimate the value of Kp and Kc for this system:

7. What is the value of the equilibrium constant for the reaction 2 NO2(g)  N2O4(g) at 100oC?

N2O4(g)  2 NO2(g) Kc = 0.212 @ 100oC?

8. What is the value of the equilibrium constant for the reaction, 4 ICl (g)  2 I2(g) + 2 Cl2(g) at 25oC?

½ I2(g) + ½ Cl2 (g)  ICl(g) Kc = 4.54 x 102 @ 25oC?

9. Calculate the value of Kc for the reaction: 2 NO(g) + Br2(g)  2 NOBr (g) using the following information.

NO(g)  N2(g) + O2(g) Kc1 = 1 x 1030

N2(g) + Br2(g) + O2(g)  2 NOBr(g) Kc2 = 2 x 10-27

10. Calculate the value of Kc for the reaction:

2 N2O(g) + 3 O2(g)  2 N2O4(g),

using the following information.

Equation Equilibrium Constant

2 N2 (g) + O2(g)  2 N2O(g) Kc = 1.2 x 10-35

N2O4(g)

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