AP Chemistry 2015-2016
ICE Table Group Posters
Name:
Date:
Per:
Directions: Read the problem assigned to your group. Take a few minutes to try to solve it BY
YOURSELF, and then work with your group to find a solution. Once your group has come to consensus,
put your work on the poster paper. Show ALL of your work on the poster legibly – use all of the space! If
your group gets stuck, I will give you a hint. If you finish early, start working some of the other problems.
If you don’t know what group you are, look at the label on your desk 
Group 1
A mixture of 1.374g of H2 and 70.31 g of Br2 is heated in a 2.00 L vessel at 700. K. At equilibrium the
vessel contains 0.566g H2. H2 (g) + Br2 (g) ↔ 2 HBr (g)
Calculate equilibrium pressures and Keq.
Group 2
A mixture of 0.2000 mol of CO2, 0.1000 mol H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. At
500. K, PH2O = 3.51 atm at equilibrium. CO2(g) + H2(g) ↔ CO(g) + H2O(g)
Calculate the equilibrium pressures and Keq.
Group 3
For the reaction N2O4 (g) ↔ 2NO2 (g) Keq = 4.0x10-7at 25⁰C. In an experiment, 1.0 mol of N2O4 is placed in
a 10.0-L vessel. Calculate the equilibrium concentrations of NO2 and N2O4.
Group 4
Phosphorus pentachloride decomposes into Phosphorous trichloride and Chlorine gas. 5.00 moles of
pure phosphorus pentachloride is placed in a 0.10 L bottle. What are the resulting concentrations?
PCl5(g) ↔PCl3(g)+Cl2(g)
Kc = 0.0211 mol
Group 5
A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0-L vessel at 300 K. The
following equilibrium is established: 2NO (g) + 2H2 (g) ↔ N2 (g) + 2H2O (g). At equilibrium PNO = 1.53 atm.
Calculate Keq.
Group 6
At 2000.°C the equilibrium constant for the reaction 2NO (g) ↔ N2 (g) + O2 (g) is Keq = 2.4 x 103. If the
initial partial pressure of NO is 0.50 atm, what are the equilibrium partial pressures of NO, N2, and O2?
𝑥=
−𝑏 ± √𝑏 2 − 4𝑎𝑐
2𝑎
Group 7
Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture is made containing an
initial [SO2Cl2] of 2.2×10−2 M . At equilibrium, [Cl2]= 1.3×10−2 M. Find Kc
Group 8
For the following reaction, Kc = 0.513 at 500 K. N2O4(g) ⇌ 2NO2(g) If a reaction vessel initially contains
an N2O4 concentration of 5.50×10−2 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2
at 500 K?
Group 9
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial
concentrations: [H2S] = 0.225 M , [H2] =0.250 M , and [S2] = 0.00 M. Find the equilibrium concentration of [S2].
Homework:
Review questions 12-16 due Thursday, 10/22
Book problems 51, 52, 53, 55, 57, 59, 61 due Thursday, 10/22
Looking Ahead:
Tomorrow: more practice!
Thursday: AP FRQ
Friday: Quiz on 15.1-15.5
Weekend homework: notes on 15.6
𝑥=
−𝑏 ± √𝑏 2 − 4𝑎𝑐
2𝑎