1.) Consider the following reaction: 2 ClF (g) → Cl2 (g) + F2 (g) Assume that an experiment is carried out in which the starting concentration of ClF (g) is 0.100 mol/L. No products are present at the beginning of the reaction. When equilibrium is established, the concentration of Cl2 (g) is 2.89 x 10-6 mol/L. Calculate the equilibrium constant for the above reaction

2.)  A mixture of gases is at equilibrium: C2H4 (g) + H2 (g) →  C2H6 (g)      ∆H = -136.94 kJ (a) Does the equilibrium shift to the left or to the right when some C2H4 (g) is removed from the reaction mixture? (b) Does the equilibrium shift to the left or to the right when some C2H6 (g) is removed from the reaction mixture? (c) In which direction does the equilibrium shift as the temperature is raised? (d) In which direction does the equilibrium shift as pressure is applied to the system?

3.)  Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.870 mol N2 and 0.300 mol O2 are mixed in a 5.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small—less than 10% of the starting amounts—and check your assumption when you have solved the equation.