Thursday, October 8, 2015

October 8, 2015

We are going to ask questions for the following reaction according to Le Chatlier's Principle. I will start with a question, the next person should answer it and ask their own question. You can add numbers to the question, but let's try to keep it fairly conceptual.

                                        CaCO3(s) ⇌  CaO(s)  +  CO2(g)                 ∆H = 131.4 kJ
Explain what happens to the value of the equilibrium constant when CaO is added to the reaction at equilibrium.
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12 comments:

  1. UnknownOctober 10, 2015 at 1:03 PM

    This change would not effect the equilibrium constant since solids are not in the equation. However, this would effect the concentration of CaO and since CaO is a product, adding more would off balance the equilibrium in favor of products. The system would compensate for this stress by making more reactants to bring the reaction back to equilibrium.

    Question: If heat was added to this reaction would it result in: A shift towards products, a shift towards reactants, or no effect on reaction? And how would this change effect the equilibrium constant?

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    Replies
    1. UnknownOctober 12, 2015 at 9:51 AM

      answer: if heat is added, the reaction will result in a shift toward products, since it is an endothermic reaction.

      question: if volume is decreased, which way will it drive the equation?

      Delete
    2. UnknownOctober 13, 2015 at 2:13 PM

      Since CaO is a solid it neither affects the equilibrium constant nor the equilibrium position of the reaction. (Unless we were to totally remove all CaO)

      Delete
  2. UnknownOctober 12, 2015 at 2:46 PM

    I think if volume is decreased the pressure will increase, and it will shift to the left because there is fewer moles.

    question: If the reaction is exothermic, and the temperature decreases, then where will the reaction shift?

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    Replies
    1. UnknownOctober 13, 2015 at 2:14 PM

      Correct, but specifically "fewer moles of GAS"

      Delete
  3. UnknownOctober 12, 2015 at 4:06 PM

    I believe that lowering the temperature would favor the exothermic reaction, so the reaction would shift toward products.

    Question: If the pressure is decreased, which way will the reaction shift?

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  4. UnknownOctober 12, 2015 at 10:22 PM

    If the pressure decreases then the reaction would make more reactants as it attempts to move back toward equilibrium by favoring that side.

    Question: What happens in the reaction if CaO2, product is added?

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    Replies
    1. UnknownOctober 13, 2015 at 2:15 PM

      It would actually make more products since we want to bring the pressure back up and there is more moles of gas on the product side than on the reactant side.

      Delete
    2. UnknownOctober 13, 2015 at 2:16 PM

      I think that you mean to ask if we add CO2 to the equilibrium mixture, what would happen to the reaction.

      Delete
  5. UnknownOctober 14, 2015 at 7:05 AM

    Adding CO2 would cause a shift towards reactants.
    How does adding a catalyst shift the the reaction?

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  6. UnknownOctober 20, 2015 at 3:19 PM

    Adding a catalyst to a system at equilibrium would not cause a shift.

    How would removing CO2 affect the system?

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  7. UnknownOctober 22, 2015 at 3:59 AM

    Thanks for your responses!

    ReplyDelete

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