Chemistry II
Equilibrium
Name ________________________
Date_____________ Period_______
ICE Tables
Use the ICE table concept to solve the following problems
1. Consider the following reaction:
2 NaNO3 + Ag2SO4  Na2SO4 + 2 AgNO3
Initially for this reaction, there were concentrations of 3.2 M NaNO3 and 2.99 M Ag2SO4. The
final concentration of NaNO3 was 1.98 M. What is the equilibrium constant for this reaction?
2. A student performs a double displacement reaction between magnesium chloride and potassium
bromide.
a. Write out this reaction equation
b. If the initial concentrations were 3.8 M magnesium chloride and 4.22 M potassium
bromide and the final concentration of magnesium bromide was 1.3 M, what was the
equilibrium constant?
3. When hydrogen and iodine combine to make hydrogen iodide, the reaction is as follows:
H2 + I2  HI
If the initial concentration of H2 is 3 M, the initial concentration of Cl2 is 3 M, and the
equilibrium constant is 2.34, what are the final concentrations of the reactants and products?
4. The reaction of interest is below:
H2 + Cl2  2 HCl
The reaction starts with a sample of 6.8 M HCl. The equilibrium constant of this reaction is
0.694. Solve for the final concentration of both all reactants and products involved.