Chem Comm Warm-Up – 4/19/18

  1. Determine the number of grams needed to make 150 mL of 0.20 M NaOH solution.
  2. If you remove 5.00 mL of 0.20 M NaOH solution and evaporate all the water, how many grams of NaOH will remain?
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Chemistry Warm Up – 3/9/18

Complete on separate paper and submit to the In-Box:

Hydrogen gas reacted with oxygen gas producing water vapor in a closed container.  The system then established equilibrium.

  1. Write the balanced equilibrium equation.
  2. Write the equilibrium expression (Keq = ??).
  3. 0.505 grams of hydrogen gas and 4.00 grams of oxygen gas reacted in a 750.0 mL closed container.  The value of Keq is 5.99.  Determine the concentration of water vapor.
  4. Determine the number of grams of water produced.
  5. Describe a way to increase the concentration of water vapor produced?
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Chem Comm Warm Up – 3/8/18

Complete on separate paper and submit to the In-Box when finished.

  1. What are 2 types of mixtures and how are they different?  Make a drawing to support your answers.
  2. What are 2 things that are needed for a chemical reaction to occur?
  3. What is Activation Energy?
  4. Create a graph of Energy vs Time and add Reactants, Products and label the Activation Energy.
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Chemistry – Warm Up – 3/7/18

  1. Nitrogen gas reacted with hydrogen gas producing ammonia gas (NH3) in a closed container.  The system then established equilibrium.
    1. Write the balanced equilibrium equation (remember diatomics?)
    2. Write the equilibrium expression (Keq = ??).
    3. 2.0 grams of nitrogen gas and 0.10 grams of hydrogen gas reacted in a 500.0 mL closed container and produced 2.1 grams ammonia gas.  Determine the value for Keq.
    4. Using your answer to C, which side is favored?
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Chem Comm Warm Up – 3/6/18

  1. Name 4 layers of the Earth’s Atmosphere and list 1 significant fact about each layer.
  2. What do you think is a mixture?  Give 2 examples.
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Chem Comm Warm Up – 2/27/18

Using your textbook, re-read page 148 about each of the 6 Air Quality examples and complete the following:

  1. Write a summary statement about each of the 6 examples.
  2. Write 1 question you have about each example.
  3. When finished, go to each Lab Table and write your summary statement and question on the document.
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Chem Comm Warm Up / Review – 2/14/18

  1. Define Boyle’s, Charles’, and the Ideal Gas Law.
  2. What is held constant in Boyle’s Law?
  3. Make a graph for both Boyle’s and Charles’ Law labeling both axes.
  4. Write the statements of the Kinetic Molecular Theory. (Look here).
  5. A ball has a volume of 2.9 L and temperature of 47 C.  If the ball is put into the freezer where the temperature is -4 C, what will be the new volume?
  6. What is the temperature of 2.5 moles of He gas in a 15 L container at 0.85 atm pressure?
  7. A 4.65 L balloon at 1.5 atm pressure with a temperature of 298 K is taken to a pressure of 5.6 atm pressure.  What is the new volume?
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Chem Comm Warm Up – 2/12/18

  1. 12.5 grams of Neon gas is in a 2.0 L bottle at 745 torr pressure.  What is the temperature in K and C of the gas?  (Remember the steps: make list of givens, determine gas law, isolate unknown, make conversions if needed, plug in and solve)
  2. When completed, begin making corrections to U2 Section A Quiz, U2 Section B Packet and Gas WS.
  3. Begin making 1-page (8.5 inch x 11 inch) of notes to be used on upcoming Beta this Friday.
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Chem Comm Warm-Up – 2/6/18

Complete the following problems in your notes.

  1. A balloon with a volume of 3 L at 25 C is heated to 35 C. Make a drawing of the balloon before and after heating.  Then, determine the new volume?
  2. A 2 L bottle of gas has a pressure of 1.5 atms.  The pressure is raised to 1575 mmHg.  Make a drawing of the bottle before and after the pressure is raised.  Then, determine the new volume?
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Chem Comm Warm Up – 2/1/18

  1. Write the equation for Boyle’s and Charles’ Law.
  2. A basketball with a volume of 8.5 L at 1.0 atm pressure is taken up to a game in Denver where the pressure is 0.85 atm.  The volume in the ball will change.  Do the following to determine the new volume:
    1. Make a list of the given values
    2. Use the list to determine which gas law to use
    3. Before solving, predict if the volume will go up or down
    4. Before solving, isolate the gas law for the new volume
    5. Plug in your values and solve for the new volume
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