Unit 11 Quiz--Equiliblrium and Le Chatelier's Principle

Multiple Choice (Choose the best answer.)

1. Which of the below are ways that allow you to recognize equilibrium?

   constant temperature

   constant color

   constant pressure

   All of the above are correct.

   None of the above are correct.

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2. Equiliblrium is a state of dynamic molecular behavior, meaning that

   the reaction eventually comes to a stop.

   reactants continually turn into products at a progressively slower rate.

   products continually turn into reactants at a progressively faster rate.

   reactants turn into products and products turn into reactants at different rates.

   reactants turn into products and products turn into reactants at equal rates.

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   In your lab, Concentration and Temperature Effects on Equilibrium, you studied the aqueous reaction:

   Fe +3 + SCN - FeSCN 2+

   (Light Yellow) (Deep Red)

   
   Use your knowledge of equilibrium to answer questions 3 - 5.

3. Adding Fe(NO₃)₃ produced the following change in the equilibrium:

   The color in the test tube became a deeper red color because the equilibrium shifted to make more reactants.

   The color in the test tube became a deeper red color because the equilibrium shifted to make more products.

   The color in the test tube became a lighter color because the equilibrium shifted to make more reactants.

   The color in the test tube became a lighter color because the equilibrium shifted to make more products.

   None of the above are correct.

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4. Adding AgNO₃ to the test tube removed SCN ^- from the reaction, causing the reaction to

   produce more reactants.

   decrease the amount of products.

   produce a deeper red color.

   A, B, and C are all correct.

   A and B are both correct.

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5. The reaction you studied is became a deeper red color when placed in an ice bath. This means that the reaction is

   exothermic.

   endothermic.

   There is not enough information given to answer the qusestion.

   None of the above are correct.

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6. In the reaction N₂O₄ (g) 2 NO₂ (g), an increase in pressure (by reducing the volume) would make the reaction

   form more products.

   form more reactants.

   Increasing the reaction would have no effect on the equilibrium.

   There is not enough information given to answer the question.

   None of the above are correct.

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7. In the reaction, CO (g) + NO₂ (g) CO₂ (g) + NO (g), which of the following changes would result in the formation of more products at equilibrium?

   increasing the pressure

   removing CO (g) from the reaction

   adding NO₂ (g) to the reaction

   adding CO₂ to the reaction.

   None of the above would result in more products.

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