Equilibrium Worksheet - DOC by parpar

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									                              Equilibrium Worksheet
For the reaction: SiH 4(g) + O2(g)  SiO 2(g) + H2O(g)

1. Write the equilibrium equation in the forward reaction:

2. Write the equilibrium equation in the reverse reaction:

3. What is the equilibrium constant if [SiH 4 ] = 0.45M; [O2] = 0.25M; [SiO2] = 0.15M; and [H2O] = 0.10M at
equilibrium?

4. What is the equilibrium constant in the reverse reaction?

5. If [SiH4] = 0.34M; [O2] = 0.22M; [SiO2 ] = 0.35M; and [H2O] = 0.20M, what would be the reaction
quotient?

6. Which direction would the reaction go? (Towards products or reactants?)

7. H2(g) + CO2(g)  H2O (g) + CO (g)
a) It is found at 986oC that there are 11.2 atm each of CO and water vapor and 8.8atm each of H 2 and CO2 at
   equilibrium. Calculate the equilibrium constant.
b) If there were 8.8 moles of H2 and CO2 in a 500.0mL container at equilibrium, how many moles of CO (g)
   and H2O(g) would be present?


8. The equilibrium constant for the decomposition of COBr 2 : COBr2  CO + Br2 (all gases)
Is 0.190 at 73oC. If the concentrations of both CO and Br2 are 0.402M, and the concentration of COBr 2 is
0.950M, is the system at equilibrium? If not, which way does it proceed?


9. You place some COBr2 in a 5.0 L flask and heat it to form CO and Br2. If you want a Br2 concentration
of 0.0500 M at equilibrium, how many grams of COBr2 will you use in the beginning?

								
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