1. In the oxidation of sulfur dioxide to sulfur trioxide: if 1.00mol of SO2 and 1.00mol of O2 are placed in a 1.00L flask at 1000K. At equilibrium; 0.925mol SO3 has been formed. Calculate the K

at equilibrium. Use the ICE to get the value of K.

SO2 (g) + O2 (g) e SO3(g)

2. For the reaction :

H2(g) + I2(g) e 2HI(g) Kc = 55.64

If 1.00 mole of H2 and I2 placed in 0.5L flask at 425oC. What are the concentration of H2, I2, and

HI when at equilibrium?

3. I2(g) e 2I(g), K = 5.6 x 10-12

Assuming the initial I2 concentration is 0.45M; what is the concentration of I and I2 at equilibrium?

4. PCl5(g) e PCl3(g) + Cl2(g)

If initial concentration of PCl5 is 1.60M, what will be the concentration of reactant and products when

the system reaches equilibrium? K = 1.20, Use ICE to solve this problem. (Quadratic equation calc.)

5. Reaction Quotient Q Vs Reaction equilibrium constant Kc

Assume the concentration of H2 and I2 and HI can be measured at any moment in time:

H2 + I 2 e 2HI Kc = 60 at 350oC

For each of the following sets of concentrations, determine whether the reaction is at

equilibrium. If it isn’t, decide in which direction it must go to reach equilibrium.

a. (H2) = (I2) = (HI) = 0.01M

b. (HI) = 0.3M, (H2) = 0.01M, (I2) = 0.15M

c. (H2) = (HI) = 0.1M, (I2) = 0.001M

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