I. 2NOCl (g)< < >  2NO(g) + Cl2(g)                   K= 1.6X 10-5 II. 2NO (g)  < > N2(g) + O2(g)                       K= 1.0 X 1031 Which of the following will you choose to generate the most amount of NO? (Think which of the reactions will favor the formation of NO.) a.Forward reaction of II b.Forward reaction of I c.Reverse reaction of I d.Reverse reaction of II

12. A 2.50 L vessel contains 1.75 mole N₂, 1.75 mol H₂ and 0.346 mole NH3. What is the direction of reaction needed to attain equilibrium at 401 °C? The equilibrium constant Kc for the reaction is 0.50 at this temperature. N₂(g) + 3H₂(g) 2NH3(g)

20. What will happen to the equilibrium when more SO2 (g) is added to the following system? 2502(g) + O2(g) = 250(g) A. It will shift to the right. B. It will shift to the left C. no shift of equilibrium D. cannot be determined 21. For the reaction 2A+B2C the appropriate form for the equilibrium constant expression is: A. [A][B12/ [C] B. [AB]/[C12 C. [C]2/[A][B] D. [ABRIC] 22. Calculate K for the following reaction given the following equilibrium concentrations of H2, CO, and H₂O. PCl3(g) + Cl₂(g) K=? Equilibrium Concentrations (M): PCIs(g) .200 .040 .080 A. 0.16 B.0.016 C.1.6 D.16 23. Which of the following is not omitted when writing the equilibrium constant expression? D. all of the choices A. gas C. solid B. liquid 24. When can we say that the reaction is already at equilibrium? A. When Q is not equal to K. C. When Q is greater than K. D. When Q is lesser than K. B. When Q is equal to K. 25. Where will the equilibrium shift when we increase the pressure of the system? B. towards…

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature.  If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?