5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams.

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1 CHEMISTRY TEST NAME: MASS AND VOLUME DATE: EQUATION RELATIONSHIPS Directions: For each of the following questions, choose the number that best answers the question and place it on your answer sheet. Directions: For each of the following questions, all major steps must be show to receive full credit. Mass and Volume Equation Relationships Level 1 Multiple Choice 1. For the reaction, S + O2 SO3, the number of grams of oxygen required to produce 64 grams of sulfur trioxide is 1) 2 grams; 2) 16 grams; 3) 38 grams; 4) 55 grams; 5) 64 grams. 2. For the reaction, C + O2 CO2, the number of grams of oxygen needed to produce 88 grams of carbon dioxide is 1) 16 grams; 2) 32 grams; 3) 48 grams; 4) 64 grams; 5) 72 grams. 3. What mass of water is produced by the complete combustion of 126 grams of propene, C3H6? C3H6 + O2 H2O + CO2. 1) 18.0 grams 2) 54.0 grams 3) 126 grams 4) 162 grams 5) none of these 4. How many grams of calcium phosphate will react with 100 grams of magnesium nitrate? 1) g. 2) g. 3) 98.2 g. 4) 69.7 g. 5) none of these 5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams. 6. How many grams are there in 2.50 moles of chromium? 1) g. 2) 20.8 g. 3) 41.6 g. 4) 60.0 g. 5) 130 g. 7. How many grams of water are produced when 100 grams of methane, CH4, undergo complete combustion with oxygen? Carbon dioxide is also produced in this reaction. 1) 44.4 g. 2) g. 3) g. 4)337.5 g. 5) none of these 8. How many grams of magnesium metal are produced by the decomposition of 9.5 grams of magnesium chloride? 1) 0.12 gram 2) 0.24 gram 3) 2.4 grams 4) 3.6 grams 5) 4.8 grams 9. The sum of the molecular masses on one side of an equation is 1) greater than; 2) less than; 3) equal to; 4) sometimes more and sometimes less than; the sum of the molecular masses on the other side of the equation.

2 10. As far as can be detected by analytical balances, in any chemical reaction, the sum of the masses of all the reactants 1) always equals the sum of the masses of all the products. 2) is less than that of the products if a precipitate is formed. 3) never equals that of the products. 4) is greater than that of the products if a gas forms. 11. The Law of Conservation of Matter states that in an ordinary chemical change 1) the elements lose their identity. 2) matter can neither be created nor destroyed. 3) elements combine to form compounds. 4) compounds always have a definite proportion by mass. 12. In the reaction between calcium nitrate and sodium bromide, how much calcium nitrate is needed to produce 93.3 grams of sodium nitrate? 1) 76.5 grams 2) 90.1 grams 3) grams 4) grams. 13. When 8 grams of hydrogen are chemically combined with oxygen to form water, the amount of oxygen needed is 1) 1 gram; 2) 16 grams; 3) 32 grams; 4) 64 grams; 5) 48 grams. 14. For all practical purposes in ordinary chemical changes the total mass of the reacting materials compared to the total mass of the products is: 1) always less; 2) always more; 3) always equal; 4) sometimes more and sometimes less; 5) can not be determined. 15. When copper foil is heated in air: 1) the substance formed weighs less than the reacting substances; 2) the copper loses mass; 3) the mass of the substance formed equals the mass of the reacting substances; 4) no change occurs. 16. Calculate the mass of hydrogen nitrate that reacts with iron (II) sulfide to produce 50.0 grams of ferrous nitrate. 1) 17.5 grams 2) 35.0 grams 3) 71.3 grams 4) 86.4 grams 17. In the reaction between chromium and sulfuric acid, H2SO4, how many grams of chromium are required to produce 10.0 grams of hydrogen? 1) 43.4 grams 2) 86.7 grams 3) grams 4) grams 18. How many grams of zinc carbonate are needed to react with sodium phosphate to produce 180 grams of sodium carbonate?

3 1) 88.7 grams 2) grams 3) grams 4) grams 19. In a chemical reaction, the total mass of the reactants 1) is greater than the total mass of the products; 2) is equal to the total mass of the products; 3) is less than the total mass of the products; 4) cannot be determined. 20. Which property is always conserved during a chemical reaction? 1) mass 2) volume 3) pressure 4) solubility 21. When wood burns completely, the products formed weigh 1) less than, 2) more than, 3) the same as, 4) sometimes less and sometimes more than, the original piece of wood. 22. The total mass of the substances taking part in a chemical change 1) always increases; 2) always decreases; 3) remains unchanged; 4) sometimes increases and sometimes decreases. 23. How many grams of mercury can be obtained from the decomposition of 25 grams of mercuric oxide? 1) 5.86 g. 2) 5.98 g. 3) 11.8 g. 4) 17.9 g. 5) 23.1 g. 24. What mass of sodium sulfate may be obtained by heating grams of sodium chloride with sulfuric acid, H2SO4? 1) 97.5 grams 2) grams 3) grams 4) grams 25. How much zinc chloride can react with 100 grams of hydrogen phosphate? 1) 10.7 grams 2) 27.4 grams 3) 57.6 grams 4) grams 5) grams 26. What is the maximum mass of water that can be produced from 34.0 grams of ammonia? 4 NH3 (g) + 5 O2 (g) 6 H2O (g) + 4 NO(g) 1) 9.0 grams 2) 18.0 grams 3) 36.0 grams 4) 54.0 grams 5) 108 grams 27. How many grams of barium are needed to react with 80.0 grams of aluminum chlorate? 1) 39.6 grams 2) 59.4 grams 3) 75.4 grams 4) grams 5) grams 28. How many grams of magnesium are required to react with 75.0 grams of bromine? 1) 11.2 grams 2) 22.4 grams 3) 33.7 grams 4) grams 5) grams 29. When 7.8 grams of potassium react with an excess of KOH, 1) 9.4 grams of K2O form. 3) 5.6 grams of KOH form.

4 2) 0.2 gram of H2 forms. 4) the resulting solution is acidic. 30. Calculate the number of grams of zinc which will react completely with 146 grams of HC1. 1) 130 grams 2) 156 grams 3) 163 grams 4) 175 grams 31. What mass of magnesium must be burned so as to form 40.0 grams of magnesium oxide? 1) 8.0 grams 2) 12.0 grams 3) 20.0 grams 4) 24.0 grams 5) 40.0 grams 32. How many grams of hydrogen will be formed from complete reaction of 6.5 grams of zinc with sulfuric acid, H2SO4? 1) 0.2 gram 2) 6.5 grams 3) 10.0 grams 4) 20.0 grams 33. How much phosphoric acid, H3PO4, will react with 15.0 grams of calcium carbonate? 1) 9.8 grams 2) 14.7 grams 3) 23.0 grams 4) 29.4 grams 34. What is the maximum mass of ozone, O3, that can be prepared from 16.0 grams of oxygen according to the reaction: O2 (g) O3 (g)? 1) 10.7 grams 2) 22.4 grams 3) 24.0 grams 4) 32.0 grams 5) none of these 35. How many grams of hydrogen will react with 20.0 grams of oxygen? 1) 1.3 grams 2) 2.2 grams 3) 2.5 grams 4) 3.0 grams 5) 7.4 grams 36. How many grams of potassium chlorate must be decomposed to produce 30 grams of oxygen? Potassium chloride is also formed. 1) 76.6 grams 2) grams 3) grams 4) grams 5) grams 37. For the reaction N2H4 (1) + N2O4 (l) N2 (g) + H2O(l), determine the mass of H2O formed when 20.0 grams of N2O4 react. 1) 3.6 grams 2) 7.8 grams 3) 8.6 grams 4) 15.6 grams 5) none of these 38. What mass of sulfur must combine with aluminum to form 600 grams of aluminum sulfide? l) grams 2) grams 3) grams 4) grams 5) none of these 39. How many grams of aluminum chloride are needed to react with 10 grams of silver nitrate? l) 2.6 grams 2) 3.7 grams 3) 7.9 grams 4) 9.7 grams 5) 11.1 grams 40. If 112 grams of calcium oxide react completely with carbon to form CaC2 and CO, how much carbon is needed?

5 1) 16.8 grams 2) 24.0 grams 3) 47.9 grams 4) 71.9 grams 5) none of these 41. Find the mass of chromium which is formed when 30 grams of hydrogen react with chromium (III) oxide. l) grams 2) grams 3) grams 4) grams 5) 1,560 grams 42. If 10.0 grams of iron, Fe, and 10.0 grams of sulfur, S, are heated together, how many grams of iron (II) sulfide, FeS, could be formed? 1) 10.0 grams 2) 15.7 grams 3) 27.6 grams 4) 88.0 grams 43. Mg + 2 H + Mg +2 + H2. The equation shows that 1) Mg is less active than H2; 2) Mg is more stable than Mg +2 ; 3) one mole of Mg reacts with one mole of H + ; 4) one mole of Mg helps to produce one mole of H In the reaction H2 (g) + Cl2 (g) 2 HC1 (g) + heat 1) no bonds are broken; 2) to form 2 moles of HC1, 1 mole of H-H and 1 mole of Cl-Cl bonds must be broken; 3) bonds between molecules must first be broken; 4) an increase in potential energy takes place. 45. What happens to carbon in a candle when the candle burns? 1) It changes into oxygen and goes into the air. 2) It becomes part of a compound which goes into the air. 3) It gets slightly heavier and runs down the candle. 4) It is destroyed by the flame. 46. What mass of water will be produced according to the equation CaCO3 + 2 HC1 CaCl2 + CO2 + H2O when 1.64 liters of CO2 at STP are produced? 1) 324 g. 2) 12.3 g. 3) 2.34 g. 4) 78.9 g. 5) 1.32 g. 47. What volume of dry H2S is produced at STP when 39.0 grams of Na2S react with an excess of HC1 as shown in the equation: Na2S + 2 HC1 H2S + 2 NaCl? 1) 34.0 liters 2) 22.4 liters 3) 17.0 liters 4) 11.2 liters 48. How many grams of aluminum are needed to react with hydrochloric acid, HC1, to make 100 liters of hydrogen? Assume standard conditions exist. 1) 80.4 grams 2) grams 3) grams 4) grams 49. Consider the reaction CH4 + O2 CO2 + H2O. The number of liters of oxygen at S.T.P. that will react with 8.0 grams of CH4 is approximately: 1) 4; 2) 10; 3) 20; 4) 45; 5) none of these.

6 50. One liter of a certain gas weighs 1.25 grams. The molecular mass of the gas is 1) 12; 2) 14; 3) 28; 4) 56; 5) none of these. 51. The molar volume is used in directly solving 1) percentage composition problems; 2) mass-mass problems; 3) mass-volume problems; 4) volume-volume problems. 52. How many grams of calcium carbonate must be decomposed to produce 8.0 liters of CO2 at STP conditions? CaO is also a product. 1) 100 g. 3) 100 g L. 8.0 L 2) 100 g. x 8.0 L 4) 100 g. x 22.4 L 5) 8.0 L x 22.4 L 22.4 L 8.0 L 100 g. 53. The number of liters of NH3 at STP which can be produced from 321 grams of ammonium chloride is represented by which expression? 1) 321 x 17 2) 53.5 x ) 321 x 2 4) 17 x 321 x 2 5) 321 x What volume of chlorine is needed to react with 150 grams of chromium? The reaction takes place at standard conditions of temperature and pressure. 1) 48.4 liters 2) 67.2 liters 3) 96.9 liters 4) liters 55. How many liters of oxygen does it take to react with 325 grams of silver iodide at standard conditions? 1) 7.8 liters 2) 15.5 liters 3) 31.0 liters 4) 36.6 liters 56. When carbon burns in a plentiful supply of air, the product formed is 1) CO; 2) CO2; 3) C2O; 4) CN; 5) CO The reaction between sodium chloride and hydrogen sulfate produces 1) Cl2; 2) HC1; 3) SO2; 4) SO3; 5) none of these. 58. Calculate the mass of calcium needed to produce 15 liters of hydrogen at S.T.P. by passing hydrogen chloride over the solid. 1) 26.8 grams 2) 38.1 grams 3) 41.3 grams 4) 44.9 grams 5) 71.1 grams 59. Given: Fe + O2 Fe3O4. How many liters of oxygen at standard temperature and pressure are required to react with 6.4 grams of iron?

7 1) 1.2 liters 2) 1.7 liters 3) 2.4 liters 4) 3.6 liters 5) 7.3 liters 60. How many liters of oxygen at S.T.P. conditions are needed to produce 75.0 grams of carbon monoxide? 1) 30.0 liters 2) 36.5 liters 3) 42.8 liters 4) 60.0 liters 61. How many liters of oxygen will react with 100 grams of barium at standard conditions of temperature and pressure? 1) 8.2 liters 2) 9.8 liters 3) 16.4 liters 4) 20.2 liters 62. What volume oxygen can be obtained from the decomposition of 100 grams of ferric oxide? Calculate the volume at S.T.P. conditions. 1) 4.8 liters 2) 14.0 liters 3) 18.6 liters 4) 21.1 liters 63. What mass of propane, C3H8, will react with 250 liters of oxygen at standard conditions? Carbon dioxide and water are produced. 1) 98.2 grams 2) grams 3) grams 4) grams 64. Calculate the mass of aluminum that will react with 38.6 liters of fluorine measured at S.T.P. conditions. 1) 48.0 grams 2) 46.5 grams 3) 31.0 grams 4) 22.4 grams 65. How many liters of oxygen at S.T.P. conditions are needed in the production of 60.0 grams of sulfur trioxide? 1) 16.8 liters 2) 25.2 liters 3) 37.6 liters 4) liters 66. What volume of CO may be obtained by igniting 53.6 grams of CaC2O4 in the following reaction? CaC2O4 (s) CaCO3 + CO (g). 1) 7.4 liters 2) 10.4 liters 3) 14.7 liters 4) 17.9 liters 5) none of these 67. An excess of hydrogen will react with 21 grams of nitrogen to produce how many liters of ammonia, NH3, at standard temperature and pressure? 1) 16.8 liters 2) 24.2 liters 3) 25.5 liters 4) 33.6 liters 5) 42.0 liters 68. The equation for the fermentation of glucose to alcohol is: C6H12O6 C2H6O + CO2. How many liters of CO2 will be formed from 100 grams of this sugar at STP conditions? 1) 12.4 liters 2) 17.7 liters 3) 24.9 liters 4) 48.9 liters 5) 52.3 liters 69. The type of problem in which the atomic masses are not used in the calculations is 1) weight-weight; 2) weight-volume; 3) volume-weight; 4) volume-volume.

8 70. What volume is occupied by 1.5 moles of oxygen, O2, gas at S.T.P.? 1) 11.2 liters 2) 22.4 liters 3) 33.6 liters 4) 44.8 liters 5) 67.2 liters 71. In the reaction CO (g) + 2 H2(g) CH3OH (l) 1) the volumes are conserved; 2) the volumes of CO and CH3OH are equal; 3) the volume of hydrogen is twice the volume of carbon monoxide; 4) the numbers of moles of molecules are conserved. 72. The number of milliliters of hydrogen produced for every 8 ml. of oxygen obtained by the electrolysis of water is 1) 1; 2) 8; 3) 48; 4) 64; 5) none of these. 73. A mixture composed of 10 ml. of hydrogen and 10 ml. of oxygen is placed in a eudiometer over mercury. After an electric spark is passed through the mixture, the volume of gas remaining is: 1) 0 ml; 2) 5 ml; 3) 9 ml; 4) 15 ml; 5) 20 ml. 74. If a mixture of 16 ml. of oxygen and 32 ml. of hydrogen is burned, the volume of uncombined gas remaining is 1) zero; 2) 16 ml; 3) 30 ml; 4) 48 ml. 75. The complete chemical combination of one liter of H2 with one liter of Cl2 yields a gaseous product whose volume is 1) 1 liter; 2) 2 liters; 3) 3 liters; 4) 4 liters. 76. Given the equation: Kr (g) + F2(g) KrF6 (s). How many moles of fluorine, F2, are required to form 3 moles of krypton hexa fluoride, KrF6? 1) 1 mole 2) 1/3 mole 3) 3 moles 4) 6 moles 5) 9 moles 77. In the following equation, which is the limiting reactant if 2.6 moles of aluminum are reacted with 5.2 moles of HC1? 1) Al 2) HC1 3) H 4) Cl 78. In the following equation, which substance is in short supply, if 3.7 moles of potassium are reacted with 3.7 moles of nickel sulfate? 1) K 2) K2SO4 3) Ni 4) NiSO In the following equation, which reactant is in excess if 3.2 moles of nickel are reacted with 5.6 moles of HNO3? 1) Ni 2) HNO3 3) Ni(NO3)2 4) H2

9 80. What mass of iron oxide, Fe3O4, is produced from 2.0 moles of iron? Fe(s) + H2O (g) Fe3O4 (s) + H2 (g). 1) 154 grams 2) 231 grams 3) 462 grams 4) 693 grams 81. In the following equation, which reactant is in excess if 4.5 moles of silver are reacted with 3.0 moles hydrogen phosphate? 1) hydrogen phosphate 2) silver phosphate 3) silver 4) hydrogen 82. The equation N2 (g) + 3 H2(g) 2 NH3 (g) + heat shows a change in l) state; 2) the number of atoms; 3) the number of moles of atoms; 4) the number of moles. 83. Given the balanced equation: 3 PbC12 + Al2(SO4)3 3 PbSO4 + 2 A1C13. How many moles of PbSO4 will be formed when 0.4 mole of A12(SO4)3 is consumed? 1) 0.6 mole 2) 1.2 moles 3) 1.6 moles 4) 2.0 moles 84. Consider the equation CH4(g) + O2 (g) CO2 (g) + H2O (g). The number of moles of H2O formed from the burning of 5 moles of CH4 is: 1) 4 moles; 2) 10 moles; 3) 20 moles; 4) 45 moles. 85. How many moles of oxygen are produced from 3.0 moles of potassium chlorate in this equation? 2 KC1O3 (s) 2 KC1 (s) + 3O2 (g) 1) 6.0 moles 2) 9.0 moles 3) 3.0 moles 4) 4.5 moles

9. The ratio of the volume of nitrogen to that of the ammonia in the reaction N2 + 3 H2 2 NH3 is 1) 1:2; 2) 1:3; 3) 3:2; 4) 2:3.

9. The ratio of the volume of nitrogen to that of the ammonia in the reaction N2 + 3 H2 2 NH3 is 1) 1:2; 2) 1:3; 3) 3:2; 4) 2:3. 1. In a balanced chemical equation l) coefficients are equal; 2) atoms are conserved; 3) molecules are equal; 4) energy is always produced; 5) none of these. 2. Which of the following statements about