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A sample of solid CaCO3 was added to an empty 1.00 L container at 500K and...

A sample of solid CaCO3 was added to an empty 1.00 L container at 500K and then sealed. Given the value for Kc, find the equilibrium concentration for CO2.

2 CaCO3 (s) ⇌ Ca (s) + CO2 (g) + 2 O2 (g)         Kc = 45.9

Answer the following questions:

  1. What is/are the clue(s) in this problem that indicate an ICE table is needed to solve this?
  2. What assumption needs to be made about the initial concentration of the products?
  3. Why will the initial concentration of the products change?
  4. Calculate Q for the initial conditions.
  5. Compare Q to K to predict which way the reaction will shift to restore equilibrium.
  6. Will the concentration of the products increase or decrease to reach equilibrium?
  7. What needs to be referenced when predicting the values in the “Change” row?
  8. Write the ICE table for this problem, using the template at the bottom.
  9. Why is “x” needed as a placeholder?
  10. Solve for x.
  11. What does the value of “x” represent in this problem?
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