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Chapter 13 | Fundamental Equilibrium Concepts 717
18. The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium.
(a) (b)
= 10.00 atm
(c)
(d) = 0 atm
(e) NOCl = 0 atm
[NH3] = 0.50 M, [N2] = 0.15 M, [H2] = 0.12 M
initial pressures: NH3 = 2.00 atm, N2 = 10.00 atm, H2
[SO3] = 2.00 M, [SO2] = 2.00 M, [O2] = 2.00 M
initial pressures: SO2 = 1.00 atm, O2 = 1.130 atm, SO3
initial pressures: NO = 1.00 atm, Cl2 = 1.00 atm, [N2] = 0.100 M, [O2] = 0.200 M, [NO] = 1.00 M
(f)
19. The following reaction has KP = 4.50 10−5 at 720 K.
If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach
equilibrium? P(NH3) = 93 atm, P(N2) = 48 atm, and P(H2) = 52
20. Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium?
[SO2Cl2] = 0.12 M, [Cl2] = 0.16 M and [SO2] = 0.050 M. Kc for the reaction is 0.078.
21. Which of the systems described in Exercise 13.15 give homogeneous equilibria? Which give heterogeneous equilibria?
22. Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?
23. For which of the reactions in Exercise 13.15 does Kc (calculated using concentrations) equal KP (calculated using pressures)?
24. For which of the reactions in Exercise 13.16 does Kc (calculated using concentrations) equal KP (calculated using pressures)?
25. Convert the values of Kc to values of KP or the values of KP to values of Kc.
(a)
(b)
(c) (d)
26. Convert the values of Kc to values of KP or the values of KP to values of Kc. (a)
(b)
(c)
(d)
27. What is the value of the equilibrium constant expression for the change at 30 °C? (See Appendix E.)
28. Write the expression of the reaction quotient for the ionization of HOCN in water.
