Chemistry

Final Exam Review GuideSPRING 2012

Textbook Chapter 8 (Ionic Compounds)

  1. Naming Ionic Compounds
  2. NH4Cl______
  1. Fe(NO3)3______
  1. Cu3P______
  1. Al(CN)3______
  1. Pb(SO4)2______
  1. Formula of Ionic Compounds (CRISSCROSS!!)
  2. lead (II) nitride______
  1. silver bromide______
  1. chromium (VI) phosphate______
  1. vanadium (V) sulfide______
  1. potassium bicarbonate______

Naming Acids

  1. Naming Acids
  2. HBr______
  1. H2SO3______
  1. H2CO3______
  1. HF ______
  1. Formula of Acids (CRISSCROSS!!)
  2. Hydroiodic acid______
  1. Sulfuric Acid______
  1. Hydrochloric Acid______
  1. Phosphorous Acid______
  1. Naming Gases
  2. What are the seven diatomic molecules (name and formula)?

Textbook Chapter 10 (Chemical Reactions)

  1. Balance the following chemical equations:
  1. ____ Mg + ____ Fe2O3 ____ Fe + ____ MgO
  1. ____ C2H4 + ____ O2 ____ CO2 + ____ H2O
  1. ____ PbSO4 ____ PbSO3 + ____ O2
  1. ____ H2O+ ____ SO3  ____ H2SO4
  1. ____ H2SO4 + ____ NH4OH  ____ H2O + ____ (NH4)2SO4
  1. ____ Fe + ____ Cl2____ FeCl3
  1. ____ Cr + ____ O2 ____ Cr2O3
  1. ____ Na + ____ H2O ____ NaOH + ____ H2
  1. ____ Ca(CN)2 + ____ AlF3 ____ CaF2 + ____ Al(CN)3

Energy Unit

  1. When a sample of liquid is cooled, its kinetic energy______.
  1. While a sample of liquid freezes, its kinetic energy ______.
  1. Use the diagram on the right to show the phase changes listed below. Also include the name of the process:
  2. Solid becomes a Liquid B: Melting .
  3. Liquid becomes a Gas ______
  4. Liquid becomes a Solid ______
  5. Gas becomes a Liquid ______
  6. Solid becomes as Gas ______
  7. Gas becomes a Solid ______

The graph at right represents the temperature time behavior of what was initially a sample of ice at 0˚C.

  1. Label how the kinetic and potential energy are changing during regions A, B and C using the graph above.
  1. During region Aof the graph above the energy being absorbed is:
  2. increasing the velocity of the water molecules
  3. increasing the distance between the water molecules and reducing their potential energy.
  4. increasing the distance between the water molecules and increasing their potential energy.
  5. decreasing the velocity of the water molecules
  1. During region B of the graph above the energy being absorbed is:
  2. increasing the velocity of the water molecules
  3. increasing the distance between the water molecules and reducing their potential energy.
  4. increasing the distance between the water molecules and increasing their potential energy.
  5. decreasing the velocity of the water molecules
  1. A sample of water in a pan is brought to a boil. Which of the following is true?
  2. The temperature of the boiling water gradually increases.
  3. The liquid water immediately flashes into gaseous water.
  4. The temperature of the boiling water remains constant.
  5. The liquid water begins to break down into hydrogen and oxygen gases

For Questions 8-13 Use Q= mCpΔT

Q= heat: Joules, Calories or calories

m= mass of water (g)

Cp= Specific Heat (water is 4.184J/g0C or 1 calorie/g0C)

ΔT= Change of temperature Tfinal-Tinitial

  1. A 12.5 g sample of water is put into a calorimeter and heated until its temperatureincreases from 20.0°C to 46.5°C. If the specific heat of water is 4.184 J/(g°C), calculate the heat absorbed by the water

  1. A 10.00 g piece of lead at 170.0°C and a 40.00 g piece of aluminum at 130.0°C are placed in a container of cold water. The final temperature of the water reads 50.0°C. Which metal lost the most heat? The specific heat of lead is 0.129 J/(g°C) and the specific heat of aluminum is 0.897 J/(g°C).
  1. When 435 joules of heat energy is added to 2.75 grams of olive oil at 27°C, the temperature goes to 95°C. What is the specific heat capacity of olive oil?
  1. Find the heat (in calories) involved when raising 275 grams of water from 45°Cto 85°C. Was the heat gained or lost by the water?
  1. If a sample of chloroform is initially at 32°C, what is its final temperature if 225.0 g of chloroform absorbs 725 Joules of heat, and the specific heat of chloroform is 0.96 J/(g°C)?
  1. What mass of iron can be cooled from 95°Cto 20°Cif 2452.7 J is given off? The specific heat of iron is 0.45J/g°C.

Textbook Chapter 11 (Moles and Stoichiometry)

  1. Calculate the molar mass for each of the following compounds
  2. Calcium nitrate
  1. Lead (II) iodide
  1. Define “Mole”

  1. Convert mass to moles
  2. How many moles does 45.0 grams of C6H12O6 represent?
  1. Convert moles to mass
  2. What is the mass of 5.0 moles of Ba(CN)2 ?
  1. Convert moles to number of particles/molecules/atoms
  2. How many molecules are in 0.25 moles of CH4?
  1. Convert number of particles/molecules/atoms to moles
  2. How many moles of CaCl2 do 2.41 x 1024 particles represent?
  1. Convert from number of particles/molecules/atoms to mass
  2. What would be the mass of 2.41 x 1024 particles of barium hydroxide?
  1. Convert from mass to number of particles/molecules/atoms
  2. How many molecules does 11.0 grams of CO2 represent?
  1. Convert moles of gases to volume at STP
  2. What would be the volume of 0.25 moles of chlorine gas at STP?
  1. Convert volume to moles of gases at STP
  2. How many moles does 44.8 L of Hydrogen gas at STP represent?

Textbook Chapter 12 (Stoichiometry)

  1. Using the following equation:

2 NaOH + H2SO4 2 H2O + Na2SO4

  1. How many moles of sodium sulfate will be formed when 11.5 moles of sodium hydroxide reacts with excess amount of sulfuric acid?
  1. Using the following equation:

Pb(SO4)2 + 4 LiNO3 Pb(NO3)4 + 2 Li2SO4

  1. What is the mass of lithium sulfate produced when 250 grams of lithium nitrate reacts with excess amount of lead (IV) sulfate.
  1. Using the following equation:

2H2 + O2 2 H2O

  1. How many grams of water can be formed if 15 grams of hydrogen reacts with 64 grams of oxygen? (hint: you can only make as much product as the limiting reactant allows!)
  1. b. What is the limiting reactant?
  1. Percent by mass
  2. What is the percent by mass of hydrogen chloride is hydrogen?
  1. Percent Yield
  1. The theoretical yield of hydrogen in a chemical reaction is 25 grams. If 7.5 grams of hydrogen is actually produced in a reaction, what is the percent yield of hydrogen?
  1. The theoretical yield of carbon dioxide in a chemical reaction is 450 grams. If 353 grams of carbon dioxide is actually produced in a reaction, what is the percent yield of carbon dioxide?

Textbook Chapter 19 (Acids, Bases and Solutions)

  1. List the properties of acids and bases
  1. Write all the formulas involved in pH, pOH, [H+], [OH-] calculations (there are 6 total)
  1. pH and pOH Calculations
  2. Calculate the pH of 0.09 M solution of HBr (hydrobromic acid)
  1. Calculate the pH of a 7.98 x 10-2 M solution of HNO3 (nitric acid).

  1. Calculate the pOH of a 2.34 x 10-5 M NaOH solution
  1. Calculate the hydrogen ion (H+) concentration of the following aqueous solutions:
  2. Calculate the H+ concentration of an aqueous solution, given the concentration of OH – is 1x10-8 M (Kw = 1x10-14).
  1. What is the pH of an aqueous solution given the concentration of H+ ion is 1 x 10 -7.8 M.
  1. At 298 K, the H+ ion concentration of an aqueous solution is 1.00 x 10-6. What is the pH of the solution?
  1. Calculate the molarities of the following solutions:
  2. 2.3 moles of sodium chloride in 0.45 liters of solution.
  1. 98 grams of sodium hydroxide is dissolved in water to make 220mL of solution. What is the molarity?
  1. How many grams of copper (II) fluoride are needed to make 6.7 liters of a 1.2 M solution?
  1. A 340 mL of 0.5 M sodium bromide solution is used to make 560 mL of solution. What is the molarity of the new solution?

Use the information on the solubility curves to answer the following 4 questions.

1.Between 10oC and 40oC, which substance will dissolve the fastest?

2.Between 10oC and 40oC, which substance will dissolve the slowest?

3.Kyle needs a saturated solution of potassium nitrate at 40oC. How many grams of potassium nitrate will he need to mix with 150 g of water to make his saturated solution?

4.A mass of 10 g of potassium nitrate is dissolved in 100 ml of water at 20oC. The solution is heated to 60oC. How many more grams of potassium nitrate must be added to saturate the solution?

5.70 grams of sodium nitrate is dissolved at 10oC with 100 g of water. Is this solution saturated, unsaturated or supersaturated?

Chapter 12: Gases

  1. What are the equations for the following:

Boyles LawCharles LawCombined Gas LawIdeal Gas Law

Boyles Law

  1. The pressure on 3.0L of a gas is changed from 740torr to 2atm. What will be the new volume of the gas?

Charles Law

  1. A 2.45L sample of nitrogen gas is collected at 273K and heated to 325K. Calculate the volume of the nitrogen gas at 325K. Assume constant pressure.

Ideal Gas Law:

  1. If 0.126 g of a gas are contained in a 25mL tank at 25ºC and 3.25 atm, what is the molar mass of the gas? What is the gas?

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