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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