Chemical Equilibrium

Please show all work, identify all parts of equations keep it simple (this is a first year cousre. Some TA's have gone way beyond first year in their answers)  Please send in Word format.




1.   The Reaction Quotient.  The reaction CS2(g) + 4 H2(g)  CH4(g) + 2 H2S(g)  has an equilibrium constant of 0.28 at 900°C.  Fill in the data table below.  
[CS2]o(M)[H2]o(M)[CH4]o(M)[H2S]o(M) Q Directionofshift
1.17    1.42     1.76   0.257
1.56    1.12     0.998  1.33
1.07    1.16     1.23   0.664

2.  Calculating Equilibrium Concentrations.  Consider the reaction SO2(g) + NO2(g)  NO(g) + SO3(g)  at 460°C.  What are the equilibrium concentrations of all reactants and products if the initial concentrations are [SO2]o = [NO2]o = 3.00 x 10-3 M and [NO]o = [SO3]o = 4.00 x 10-2 M?  The value of the equilibrium constant for the reaction is 85.0 at 460°C.  


3.  The Quadratic Equation. Consider the reaction 2 COF2(g)  CO2(g) + CF4(g)  at 1000°C in a 5.00-L container.  Use the quadratic equation to determine the equilibrium concentrations of all reactants and products if the initial amounts are 0.105 mol COF2, 0.220 mol CO2, and 0.055 mol CF4.  The value of the equilibrium constant for the reaction is 2.00 at 1000°C.  

4.  The Quadratic Equation. Consider the reaction N2O4(g)  2 NO2(g) at 25°C in a 5.00-L container.  Use the quadratic equation to determine the equilibrium concentrations of the N2O4 and NO2 if the initial amounts are 0.100 mol N2O4 and 0.00 mol NO2.  The value of the equilibrium constant for the reaction is 4.63 x 10-3 at 25°C.  

5.  Le Chatelier's Principle.  Consider the reaction 4 HCl(g) + O2(g)  2 H2O(g) + 2 Cl2, which has a standard enthalpy change of 30 kJ/mol HCl.  How will the amount of Cl2 present at equilibrium be affected by the following changes?  Briefly explain your answers.  

a. Add HCl
b. Remove O2
c. Increase the pressure by decreasing the container volume.
d. Increase the pressure by adding an inert gas like helium.
e. Increase the temperature.