28. For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are as shown?

22. The equilibrium constant for the formation of calcium carbonate from the ions in solution is 2.2 × 10⁸ according to the reaction:

Ca²⁺(aq) + CO₃^2–(aq) <=> CaCO₃(s) K = 2.2 × 10⁸.

What is the value of the equilibrium constant for the reverse of this reaction?

CaCO₃(s) <=> Ca²⁺(aq) + CO₃ ^2–(aq) K = ?????

Many reactions occur in the formation of photochemical smog, including the reaction of ozone with various volatile organic chemicals, or VOCs. The table in the next column shows the Arrhenius expression for four such reactions.

Identify the highest activation energy (kJ/mol) among the Arrhenius equations above. 

7. The equilibrium constant for the formation of hydrogen iodide from hydrogen and iodine is 45 at a certain temperature.

H2(g) + I2(s) <=> 2 HI(g) K = 45.

Which of the following is true regarding this equilibrium?

I. The reaction is product favored.

II. The reaction is reactant favored.

III. Equilibrium lies to the right.

IV. Equilibrium lies to the left.

2. Which of the following is true regarding the concentration of products, for a chemical reaction that is already at equilibrium, assuming no disruptions to the equilibrium?

50. Which of the following occurs when reactants are removed from a chemical reaction in solution or the gas phase at equilibrium?

33. In the ICE table started for calculating equilibrium concentrations of the reaction shown, the three terms in the “change” row are __________

Many reactions occur in the formation of photochemical smog, including the reaction of ozone with various volatile organic chemicals, or VOCs. The table in the next column shows the Arrhenius expression for four such reactions.

Identify the highest rate constant at 25 ^oC among the Arrhenius equations above. 

35. A reaction X + 2Y → 3Z is started with 1.0 M Z and no X or Y. To calculate the equilibrium concentrations of all species using an ICE table, which of the following would you enter in the Z column for the C row?

The following rate constants were obtained in an experiment in which the decomposition of gaseous N₂O₅ was studied as a function of temperature. The products were NO₂ and NO₃.

   T (^oC)           k (s^-1)       

   41            0,31

   88            7,3

Determine Ea for this reaction in kJ/mol.