AEW Assignments

                                   Measurements, Density, and Matter

*Please work in groups, and show your work on separate pieces of paper. Some of these problems may have more than one answer, so keep that mind. Questions marked with an asterisk have a video/demonstration as a complement.

 Review

  1. An area of a football field is 6,400 square yards. What is the area in square meters?
  2. Acetic acid is the acidic component of vinegar. If a 25-mL sample has 1500 milligrams of acetic acid, what is the mass of acetic acid in pounds?
  3. What type of change (physical or chemical) does boiling water undergo? And why?
  4. What is the volume of half a pound of ethanol if its density is 0.789 g/cm3?

Demonstration

*Provide an estimate for the mass of the object.

Problems

  1. The distance from Los Angeles to Las Vegas is 270 miles. The hybrid vehicle you are using for this trip has a mileage of 15.6 km/L with a tank that holds a maximum of 7 gallons. Can the vehicle make the entire trip on one full tank of gas?
  2. You are given a solid sphere that has a diameter of 7 inches, and are told to determine the mass of it. The object in question does not float in water, how much does it weigh?
  3. There is a glass jar in the middle of the room that has a volume of 10 liters. The jar is filled with a liquid, and is immediately sealed after a match is thrown into the jar. A combustion reaction occurs, and the volume of the liquid has been reduced. Did the mass within the sealed jar change?
  4. *Is the use of the boat reasonable? How much would the safe and the gold weigh? Can the boat carry this amount?
  5. There is a silo that is 10 meters in height and has a diameter of 4 meters; it is filled with water. What is the weight of all the water within the silo?
  6. An iceberg has a volume of 1000 ft3, what is the mass of said iceberg?
  7. What are the differences between a chemical property and a physical property?
  8. Why does ice float in water? How is this possible?

 

                                  Energy and Elements

*Please work in groups, and show your work on separate pieces of paper. Some of these problems may have more than one answer, so keep that mind. Questions marked with an asterisk have a video/demonstration as a complement.

Review

  1. Describe the differences between chemical, potential, and kinetic energy?
  2. Convert the freezing point and boiling point of water from Celsius to Fahrenheit.
  3. What are the particles that make up atoms? Describe each particle found in the atom.
  4. Describe the difference between an element and a compound?

Demonstrations

Provide a prediction for each trial:

  • The cup is completely dry.
  • The outer surface of the cup is lightly coated with water.
  • The cup is filled with water.

 

Problems

  1. Why does one pound of aluminum heat up faster than one pound of water? How much energy would be required to heat up both objects to 100°C when both start at room temperature?
  2. A student argues that ions have a positive charge because they gain protons. Is this student correct? If not, explain.
  3. Determine the amount of energy required to force ice to proceed through two phase shifts.
  4. There is a big container that is filled with 2 liters of water at room temperature. Additionally, there is solid sphere of gold that weighs ¾ of a pound. If the sphere was given 840 joules of energy and dropped into the container of water, what would be the final temperature of the sphere and the water? (Assume that the container is perfectly insulated.)
  5. What is mass of the proton in the hydrogen atom? How much does this proton weigh in comparison to the mass of the hydrogen atom?
  6. How much energy is needed to melt a ball of gallium that has a diameter of 0.22 ft?
  7. Rutherford’s atomic model states that protons and neutrons are the core of the atom inside the nucleus. Determine the density of the nucleus of a Ca2+ ion.
  8. California has gone through a very long drought. Farmers have needed to import water for irrigation. A fellow students suggests that the ocean is a potential water source. Is this a good or bad idea? Why?

 

 Isotopes, Atomic Mass, and Chemicals Formulas/Compounds

*Please work in groups, and show your work on separate pieces of paper. Some of these problems may have more than one answer, so keep that mind. Questions marked with an asterisk have a video/demonstration as a complement.

 Review

  1. What are isotopes? How do they affect the atomic mass of elements?
  2. Why do alkali metals lose an electron, whereas halogens gain an electron?
  3. Name the strong acids and bases. Name 3 weak acids and bases.
  4. Name the following elements: Sb, Zr, U, Os, Mn, Fr, and Sn

Demonstration

 

Problems

  1. If an atom of gold loses one proton, what happens to that atom?
  2. Name a couple of elements and compounds that we encounter in everyday life.
  3. Make a question (that is related to chapter 4) to ask your group mates, and let them attempt to answer the question?
  4. Calculate the atomic mass of Pt and determine the percentage of each of its isotopes.
  5. Discuss the differences between an ionic compound and a molecular compound?
  6. What is the molecular mass of glucose? What is the molecular mass of table salt?
  7. Pick two elements and find three examples of its use in industry/ everyday life.
  8. Ask a question regarding the chapter.

 

                                             Chemical Composition

*Please work in groups, and show your work on separate pieces of paper. Some of these problems may have more than one answer, so keep that mind. Questions marked with an asterisk have a video/demonstration as a complement.

 Review

  1. Determine the mass (in grams) of carbon in the following compounds: carbon dioxide, ethanol, phosphoric acid, ammonium bicarbonate.
  2. Discuss the difference between empirical formula and molecular formula.
  3. Determine the mass percentage of oxygen in nitric acid, sulfuric acid, and methyl-benzene.
  4. Hydrolysis of water produces a mixture of H2 and O2 gas. If we ignited this mixture, what would be our product?
  5. Which has more atoms, 393.92 g of Au or 24.02 g of C?

Demonstration

 

Problems

  1. What is the percentage (by mass) of oxygen and nitrogen in 4 g of C7H5N3O6?
  2. What is the identity of a compound whose decomposition produced 24.02 g of carbon and 64 g of oxygen?
  3. What is the mass of 5 Titanium atoms?
  4. Determine the amount of gold atoms necessary to purchase an item valued at $400.
  5. Aluminum can be extracted from bauxite. The aluminum compounds present in bauxite are made into an oxide of aluminum Al2O3 for further extraction. What is the amount of pure aluminum that can be retrieved from 35 pounds of bauxite if every 7 pounds of bauxite supplied 2 kg of Al2O3?
  6. Plutonium is a radioactive element that is made in a laboratory. Its production is extremely expensive, and it is used as a fuel source for nuclear fission. How many atoms of plutonium is necessary to produce a ring that would comfortably fit your finger?
  7. A container is filled to the half-way point with liquid and sealed. As time passes, the amount of liquid in the container decreases, yet the container remains sealed. Has the mass of the contents of the container changed? What happened to the liquid?

 

Course Review

*Please work in groups, and show your work on separate pieces of paper. Some of these problems may have more than one answer, so keep that mind. Questions marked with an asterisk have a video/demonstration as a complement.

Review

  1. How much energy is required to raise the temperature of water from its freezing temperature to its boiling temperature? What states of matter does the water go through?
  2. Is it possible to turn lead into gold?
  3. Which object would be easier to throw; a small ball of gold with a diameter of 4 inches or a ball of titanium with a diameter of 0.5 ft?
  4. What are the products for the following reactions:

(NH4)2CO3 (aq) + Ca(OH)2 (aq) →

Zn (s) + HCl (aq) →

 

Demonstration

 

Problems

  1. How can we use the heat equation (Hint: Ch.3) to determine if a reaction is endothermic or exothermic?
  2. A slab of meat is thrown into a 25% brine solution and allowed to marinate overnight. The slab of meat absorbs 325 mL of the brine in the elapsed time. Determine the mass of sodium that the meat had absorbed?
  3. Tap water contains ions of calcium, magnesium, sodium, potassium, and a few other elements in varying amounts. A study was done a decade ago that discovered that the average amount of Ca2+ found in our drinking sources was 22 mg/L. How much tap water is needed to match the amount of Ca2+ found in 2 kg of CaCO3?
  4. A can of soda is placed on top of an active Bunsen burner, what will happen to the can? Explain why.
  5. There are three cups that are filled with 100 mL of water at 25°C. There are three cubes and each one consists of a different element. The first cube is copper, the second cube is aluminum, and the third cube is iron. If each cube is given 8 kJ of energy and then dropped into one of the cups, what would be the final temperature of the water and cube for each cup?

 

Chemical Reactions

*Please work in groups, and show your work on separate pieces of paper. Some of these problems may have more than one answer, so keep that mind. Questions marked with an asterisk have a video/demonstration as a complement.

Review

  1. What is the difference between the process of oxidation and the process of reduction?
  2. What are the products of the reaction between ammonium chloride and sodium hydroxide?
  3. Which phase of matter are we not able to see through?
  4. What observations can we use to suggest a chemical reaction has transpired within a system?

Demonstration

 

Problem

  1. Acid rain is rain that is unusually acidic due to the increase of H+ within the water. The substance is detrimental to forests and aquatic life. What compounds can we use to neutralize the acid rain? Please provide 3 separate reactions.
  2. A colleague suggests to you that if a pot of water is boiling then there is a chemical reaction occurring due to the production of the gas. Are they correct?
  3. Write out a balanced chemical equation that describes the reaction that occurs within the engine of a car that allows it to move forward.
  4. Antacids are often given to treat heartburn. Examples of the active ingredients include sodium bicarbonate, magnesium hydroxide, aluminum hydroxide, and calcium carbonate. Why are these compounds used to treat heartburn? Please show a balanced chemical equation for each compound.
  5. Predict the products for the following reactions:
    1. C2H5OH (aq) + O2 (g) + heat ⇒
    2. AgNO3 (aq) + NH4Cl (aq) ⇒
    3. Sodium carbonate and sulfuric acid ⇒
    4. Hydrogen gas and oxygen gas in the presence of heat ⇒
    5. Methane and oxygen gas ⇒
  6. Determine the amount of oxygen gas necessary to combust 6.5 grams of propane.
  7. A student has built a miniature automobile that runs on gasoline. How much carbon dioxide is produced from the combustion of 5 L of gas?

 

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