SAMPLE THIRD NINE WEEKS EXAM


This test consists of seven parts. You are required to do all seven. Each part has a value of 20 points.

PART I

  1. WRITE THE LAW OF CHEMICAL EQUILIBRIUM. (4pts)
  2. WRITE BOYLE'S LAW. (4pts)
  3. WRITE GUY-LUSSAC'S LAW. Not the law of Charles' & Gay-Lussac (4pts)
  4. WRITE CHARLES' LAW. (4pts)
  5. WRITE AVOGADRO'S LAW. (4pts)

PART II

NAME FIVE INDVIDUALS YOU HAVE READ ABOUT AND WHAT THEY WERE NOTED FOR. (5pts)

1.

2.

3.

4.

5.

GIVE THE FORMULA FOR THE FOLLOWING ACIDS. (5pts)

  1. Hypochlorous Acid
  2. Perchloric Acid
  3. Chlorous Acid
  4. Hydrochloric Acid
  5. Chloric Acid

GIVE THE FORMULA OF THE ANNYDRIDE FOR EACH OF THE FOLLOWING: (5pts)

  1. Barium Hydroxide
  2. Calcium Hydroxide
  3. Sulfurous Acid
  4. Sulfuric Acid
  5. Phosphoric Acid

DEFINE EACH OF THE FOLLOWING: (5pts)

  1. NORMALITY
  2. MOLARITY
  3. GRAM-EQUIVALENT WEIGHT
  4. MOLE
  5. ION

PART III

  1. WHAT IS THE PERCENTAGE OF IONIZATION IN PROBLEM NO. 3? (4pts)
  2. WHAT IS THE pH OF A 4 MOLAR SOLUTION OF ACETIC ACID? (4pts)
  3. WHAT IS THE HYDROGEN ION CONC. OF A 4 MOLAR SOLUTION OF ACETIC ACID? (4pts)
  4. USING THE COMBINED GAS LAW EQUATION - WHAT MASS OF OXYGEN GAS WILL BE REQUIRED TO OCCUPY 10 LITERS AT 735 TORRS AND 27 DEGREES CENTIGRADE? (4pts)
  5. USING THE IDEAL GAS LAW EQUATION - WHAT MASS OF NITROGEN GAS WILL BE REQUIRED TO OCCUPY 8 LITERS AT 725 TORRS AND 37 DEGREES CENTIGRADE? (4pts)

PART IV

  1. ____ Pressure is defined as a) energy per unit volume b) weight per unit volume c) push per unit volume d) force per unit area e) energy per unit area.
  2. ____ An instrument used to measure gas pressure is a a) calorimeter b) thermometer c) barometer d) speedometer e) hygrometer.
  3. ____ Gas pressure may be expressed in all of the following units except a) Torr b) atmospheres c) lbs. per sq. in. d) mm of Hg. e) g/ml.
  4. ____ When two quantities are said to vary inversly it means that a) if one increases the other increases b) if one decreases the other increases c) if one increases the other remains the same d) as the quantities vary, their product changes e) as the quantities vary their sum remains the same.
  5. ____ Which statement about two equal volumes of gases having the same temperature and pressure is not true? a) They contain the same number of molecules. b) They weigh the same. c) They are buoyed up by the same amount of air. d) They displace the same volume of air. e) They displace the same volume of water.
  6. ____ The volume of a gas is not affected by a) number of molecules b) temperature c) pressure d) kinds of molecules e) none of these.
  7. ____ If 586 ml. of a gas is heated from 20 degrees celsius to 40 degrees celsius (pressure and number of molecules constant) the resulting volume would be a) 1172 ml. b) 293 ml. c) 7383 ml. d) 1758 ml. e) 626 ml.
  8. ____ The Partial pressure exerted by each individual gas in a mixture of gases is a) the sum of the individual gas pressures b) the product of the individual gas pressures c) is the difference between the individual pressures d) the difference between the total pressure and the pressure exerted by the other gases e) none of these.
  9. ____ 700 ml. of a gas at 740 Torr pressure will occupy what volume at a pressure of 1400 Torr? a) 370 ml. b) 740 ml. c) 350 ml. d) 500 ml. e) 185 ml.
  10. ____ All of the statements concerning a mole are true except a) it is the number of molecules in 32 grams of oxygen gas b) it is used only for gases c) it contains Avogadro's number of atoms d) it is the number of atoms in two grams of hydrogen gas e) it is the same as the gram-formula weight.

PART V

  1. ____ All of the following gases are diatomic except a) fluorine b) oxygen c) chlorine d) magnesium e) nitrogen.
  2. ____ Charles' Law concerns a) pressure and volume b) volume and number of molecules c) volume and temperature d) number of molecules and temperature e) none of these.
  3. ____ Boyle's Law concerns a) pressure and volume b) partial pressure of gases c) temperature and volume d) number of molecules and temperature e) volume and number of molecules
  4. ____ Which statement concerning a mole of ammonia gas at STP is not true? a) It occupies a volume of 22.4 liters b) It weighs 28 grams c) it contains Avogadro's number of molecules d) It has a temperature of zero degrees celsius e) It has a pressure of 760 Torr.
  5. ____ Which statement is not true of absolute zero? a) It is the lowest possible temperature b) It is zero on the Kelvin thermometer c) It is equal to -273 degrees celsius d) It is the temperature at which gas molecules have no kinetic energy e) It is sometimes called Celsius temperature.
  6. ____ A 2.5 liter sample of air in a cylinder exerts pressure of 5 atm. at room temperature. With no change in temperature, the volume is changed until the pressure is 1 atm. The volume of the cylinder is now a) 5 liters b) 12.5 liters c) 0.5 liters d) 10 liters e) 1 liter.
  7. ____ If one liter of a gas at STP weighs 4.8 grams, its molecular weight is a) 48 grams b) 67.8 grams c) 107.5 grams d) 1.2 grams e) 24 grams.
  8. ____ The number of moles of oxygen gas contained in a 50 liter cylinder at 100 atm. pressure and zero degrees celsius is a) 22.3 moles b) 223 moles c) 2230 moles d) 0.223 moles e) 230 moles.
  9. ____ The discovery of the barometer is attributed to a) Robert Boyle b) Jacques Charles c) Lord Kelvin d) Evangelista Torricelli e) Antoine Lavoisier.
  10. ____ The pressure-volume relationship of gases was developed by a) Charles b) Amedeo Avogadro c) Boyle d) Lord Kelvin e) Torricelli.

PART VI

  1. ____ The temperature-volume relationship of gases was developed by a) Lord Kelvin b) Robert Boyle c) Jacques Charles d) Evangelista Torricelli e) Gilbert Newton Lewis
  2. ____ The concept of absolute temperature was developed by a) Lord Kelvin b) Torricelli c) Boyle d) Charles e) Guy-Lussac.
  3. ____ Who determined the number of particles in a mole? a) Lavoisier b) Lord Kelvin c) Boyle d) Avogadro e) Svante Arrhenius.
  4. ____ STP represents which of the following temperature-pressure conditions? a) 760 Torr and Zero degrees Kelvin b) 1 atmosphere and 25 degrees Celsius c) 760 Torr and 273 degrees Kelvin d) the difference between the total pressure and the pressure exerted by the other gases e) none of these.
  5. ____ A temperature of 500 degrees Kelvin is equal to a temperature of a) -227 centigrade b) -773 centigrade c) +227 centigrade d) +773 centigrade e) zero degrees absolute.

1. Determine mass of solute. 0.50M Na2SO4

2. Determine Molality of solution. 100 g CuSO4 in 500 g H2O

3. Determine mass of solute. 250 ml. of 0.50M H2SO4

4. Determine Molarity of solution. 84 g KOH in 250 ml.

5. Determine mass of the number of equivalents. 1.5 eq. HC2H3O2

PART VII

  1. Determine the number of equivalents for each. 54.0 g Na2SO4
  2. Determine mass of solute. 750 ml of 0.10 N Al2(SO4)3
  3. Determine Normality of solution. 60 g CuSO4 in 300 ml
  4. Convert Molarity to Normality. 0.50 M HC2H3O2
  5. Convert Normality to Molarity. 2.0 N Na3PO4
  6. WRITE DALTON'S LAW OF PARTIAL PRESSURES.
  7. WRITE GRAHAM'S LAW OF DIFFUSION.
  8. EXPLAIN THE BRONSTED-LOWRY THEORY.
  9. EXPLAIN THE LEWIS THEORY.
  10. EXPLAIN THE ARRHENIUS THEORY.

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Created by James R. Fromm (jfromm@3rd1000.com)