NAME ____________________________________________________
HOUR______
ICE BOX PROBLEMS
Directions: DON’T!!!…..Just DON’T…..Don’t even try to squeeze all your work onto this page.
Solve these problems on a separate sheet of paper. Show all your work so I can follow what you are
doing. Label your numbers with appropriate units and use significant figures properly.
1. For the reaction 2IBr(g)
I2(g) + Br2(g) Keq = 2.5 x 10-3 at 25oC. Calculate the equilibrium
concentration of each species in a 4.0 L vessel starting with 0.60 mol Ibr.
2. The equilibrium constant for the reaction given below is 43.8 at a given temperature. If initially, 2.00
moles of I2(g) and 2.00 moles of H2(g) are put into a container measuring exactly 5.0 liters, what are the
equilibrium concentrations of all species? Also find how many moles of each species are present at
equilibrium.
H2(g) + I2(g)
2HI(g)
3. The equilibrium constant for the reaction of hydrogen gas and iodine gas to form
hydrogen iodide is 57.0 at 700 K. If 1.00 mole of each reactant is put into a 10.0 L
reaction vessel at 700 K, what are the concentrations of each of the 3 gases at
equilibrium? How many moles of each gas are present?
4. Suppose you are given the following equilibrium:
CO(g) + H2 O(g)
CO2 (g) + H2 (g) Keq = 23.2 at 600 K
If initially, you place 0.150 moles of CO and H2O in a 2.00L container, what will be the concentrations of
each reactant and product at equilibrium?
5. Consider the following equation is at equilibrium:
CO(g) + H2O (g) ↔ CO2 (g) + H2 (g)
If a 10.00L vessel initially has 2.50 mol CO and H2O, and 5.00 mol CO2 and H2 gas at 588°K, what are the
equilibrium concentrations of every reactant and product? (Keq = 31.4 at 588°K)