1. ICE Tables I nitial (Concentrations) C hange E quilibrium (Concentrations)

2. A mixture of 2.00 moles of H 2 (g) and 2.00 moles of I 2 (g) is placed in a 2.00 L container held at a constant temperature. After equilibrium is reached, 3.12 moles of HI(g) are found in the container. Calculate K c for the reaction. H 2 (g) + I 2 (g) 2 HI(g)

3. 0.850M cis-stilbene is placed in a closed container. Calculate the equilibrium concentrations of cis- and trans- stilbene, given the equilibrium constant below. cis-stilbene trans-stilbene Kc = 24.0

4. 2.0 mol of N 2 O 4 and 4.0 mol NO 2 are placed in a 2.0L container at 637K. Given the K c value below, calculate the equilibrium concentrations of N 2 O 4 and NO 2. N 2 O 4 (g) 2NO 2 (g) K c = 40.

5. In air at 25  C and 1.00 atm, [N 2 (g)] = 0.033M and [O 2 (g)] = 0.00810 M. Taking the nitrogen and oxygen concentrations as initial values, calculate the equilibrium concentration of nitrogen monoxide that would exist in our atmosphere at 25  C. N 2 (g) + O 2 (g) 2 NO(g) K= 4.8 x 10 –31

6. A reaction mixture initially contains P I2 = 0.150 atm and P Cl2 = 0.150 atm and P ICl = 0.100 atm. Find the equilibrium partial pressures of all three substances. I 2 (g) + Cl 2 (g) 2IClK p = 81.9

7. K c and K p 3H 2 (g) + N 2 (g) 2NH 3 (g) K c = K p = K c (RT) Δn(gas) How would the value of K p compare to that of K c for the reaction above? K p =

8. K c and K p How would the value of K p compare to that of K c for the following reaction: CaCO 3 (s) CaO(s) + CO 2 (g)