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Homework answers / question archive / Chapter 5: Chemical Reactions and Equations 1)  Identify which image in the figure represents the reactants and which image therefore represents the products in the reaction between xenon gas and fluorine gas to form xenon tetrafluoride gas

Chapter 5: Chemical Reactions and Equations 1)  Identify which image in the figure represents the reactants and which image therefore represents the products in the reaction between xenon gas and fluorine gas to form xenon tetrafluoride gas

Chemistry

Chapter 5: Chemical Reactions and Equations

1)  Identify which image in the figure represents the reactants and which image therefore represents the products in the reaction between xenon gas and fluorine gas to form xenon tetrafluoride gas.

           

 

            A)      upper left image = reactants, lower right image = products

            B)      upper left image = reactants, lower left image = products

            C)      upper left image = reactants, upper right image = products

            D)      upper right image = reactants, upper left image = products

            E)      lower left image = reactants, upper left image = products

 

        2.  Identify which image in the figure represents the reactants and which image therefore represents the products in the reaction between ozone gas (O3) and carbon monoxide gas to form oxygen gas and carbon dioxide gas.

           

 

            A)      upper left image = reactants, lower right image = products

            B)      upper left image = reactants, lower left image = products

            C)      upper left image = reactants, upper right image = products

            D)      upper right image = reactants, upper left image = products

            E)      lower left image = reactants, lower right image = products

        3.  The figure shows the chemical reaction between nitrogen gas and hydrogen gas to produce ammonia (NH3) gas.  Which of the following changes would make the diagram correctly represent conservation of mass?

           

 

            A)      Remove one H2 molecules from the image on the left.

            B)      Add one H2 molecule from the image on the left.

            C)      Add three H2 molecules t the image on the right.

            D)      Remove one NH3 molecule from the image on the left.

            E)      Add three NH3 molecules to the image on the right.

 

        4.  The figure shows a reaction between methane gas (natural gas, CH4) and oxygen to produce carbon dioxide and water.  Is the diagram accurate, and if not, what is wrong with it, and how could it be fixed?

           

 

            A)      The diagram is accurate as shown.

            B)      There are too many oxygen atoms on the right-hand side of the reaction arrow.  Remove one oxygen atom from the carbon dioxide.

            C)      There are too many hydrogen atoms on the right-hand side of the reaction arrow.  Remove one hydrogen atom from each water molecule.

            D)      There are not enough carbon atoms on the left-hand side of the reaction arrow.  Add another methane molecule on the left, and then another carbon dioxide molecule on the right of the arrow.

            E)      There are not enough oxygen molecules on the left-hand side of the reaction arrow.  Add another oxygen molecule on the left of the arrow, and another water molecule on the right.

        5.  The figure shows a reaction between hydrogen and oxygen gases to produce water.  Is the diagram accurate, and if not, what is wrong with it, and how could it be fixed?

           

 

            A)      The diagram is accurate as shown.

            B)      There are too many oxygen atoms in the image on the left.  Remove one oxygen molecule.

            C)      There are not enough oxygen atoms on the right.  Add one more water molecule to the right image.

            D)      There are not enough hydrogen atoms on the right.  Add one more water molecule to the left image, and one more hydrogen molecule to the right image.

            E)      There are too many water molecules on the right.  Remove one water molecule from the image on the right.

 

        6.  The figure shows a reaction between xenon gas and fluorine gas.  Is the diagram correct, and if not, how could it be modified to show that the law of conservation of mass is obeyed?

           

 

            A)      The diagram is accurate as shown.

            B)      Add three more XeF4 molecules and one more Xe atom to the right image.

            C)      Add four more XeF4 molecules to the right image.

            D)      Add two more XeF4 molecules and two more Xe atoms to the right image.

            E)      Add one more XeF4 molecule and three more Xe atoms to the right image.

 

        7.  Sulfur dioxide gas reacts with oxygen gas to form sulfur trioxide gas.  What would the products of the reaction be, if the reactants are those shown in the figure?

           

 

            A)      4 molecules of sulfur trioxide

            B)      3 molecules of sulfur trioxide, and 1 molecule of oxygen

            C)      4 molecules of sulfur trioxide, and 1 molecule of oxygen

            D)      2 molecules of sulfur trioxide, and 2 molecules of sulfur dioxide

            E)      3 molecules of sulfur trioxide, and 1 molecule of sulfur dioxide

 

        8.  Gaseous nitrogen monoxide reacts with oxygen gas to form brown nitrogen dioxide gas.  What would the products of the reaction be, if the reactants are those shown in the figure?

           

 

            A)      6 molecules of nitrogen dioxide

            B)      5 molecules of nitrogen dioxide, and 1 molecule of oxygen

            C)      6 molecules of nitrogen dioxide, and 1 molecule of oxygen

            D)      4 molecules of nitrogen dioxide, and 2 molecules of nitrogen monoxide

            E)      3 molecules of nitrogen dioxide, and 3 molecules of nitrogen monoxide

 

        9.  Which of the following changes represents a physical change, rather than evidence of a chemical reaction?

            A)      When a solution of KI is mixed with a solution of Pb(NO3)2, a yellow solid is formed.

            B)      When a piece of copper wire is placed in a solution of AgNO3, a silvery solid begins to form on the surface of the wire, and the solution turns blue.

            C)      When a piece of zinc metal is placed in a solution of HCl, bubbles begin to form, and the zinc begins to dissolve.

            D)      When dry ice (solid CO2) is allowed to stand at room temperature, a white cloud and gaseous CO2 are formed.

            E)      When solid ammonium carbonate, (NH4)2CO3, is heated, the solid disappears, and gaseous ammonia (NH3), carbon dioxide (CO2), and water (H2O) are formed.

 

      10.  Which of the following changes represents a physical change, rather than evidence of a chemical reaction?

            A)      When solutions of AgNO3 and NaCl are mixed, a white solid forms.

            B)      When concentrated HNO3 is placed in contact with copper metal, a brown gas is formed, the copper dissolves, and a green solution is formed.

            C)      When water and a yellow solution of antifreeze are mixed, the resulting solution is a lighter shade of yellow than the original antifreeze solution.

            D)      When a piece of zinc metal is placed in a blue solution of copper sulfate, the solution turns from blue to colorless, the zinc dissolves, and copper metal is formed.

            E)      When an egg is fried, the clear part becomes white, and the egg becomes a solid.

 

      11.  In the figure shown, is a chemical reaction occurring? 

           

 

            A)      No, because there are the same number of atoms in both images.

            B)      Yes, because the atoms have rearranged, and therefore the formulas of the products and reactants are different.

            C)      Yes, because the reactants are gases, but the product is a solid.

            D)      No, because there are oxygen atoms and nitrogen atoms in both images.

            E)      No, because both the reactants and products are colorless gases.

 

      12.  In the figure shown, is a chemical reaction occurring? 

           

 

            A)      No, because the Na+ and Cl? ions are simply being surrounded by the water molecules as the salt dissolves.

            B)      Yes, because the Na+ and Cl? ions are being removed from their ionic lattice as they are dissolved.

            C)      Yes, because the water molecules are reacting with the Na+ and Cl? ions to form a gas.

            D)      No, because there is no change occurring.

            E)      Yes, because a precipitate will be formed when the water and NaCl are mixed.

      13.  In the figure shown, is a chemical reaction occurring? 

           

 

            A)      No, because there are the same number of atoms in both images.

            B)      Yes, because the atoms have rearranged, and therefore the formulas of the products and reactants are different.

            C)      Yes, because the reactants are gases, but the product is a solid.

            D)      No, because there are oxygen atoms and carbon atoms in both images.

            E)      No, because both the reactants and products are colorless gases.

 

      14.  Consider the following chemical equations.  Select the equations that represent chemical reactions, rather than physical changes.

              I. CH4(g) + O2(g) ® CO2(g) + H2O(g)

             II.  C2H5OH(l) ® C2H5OH(g)

            III.  NaOH(s) ® Na+(aq) + OH?(aq)

            A)      I, II, and III                                          D)      II and III only

            B)      I and II only                                          E)      I only

            C)      I and III only                                                 

 

      15.  Consider the following chemical equations.  Select the equations that represent chemical reactions, rather than physical changes.

              I. 2NO(g) + O2(g) ® 2NO2(g)

             II.  CO2(s) ® CO2(g)

            III.  Pb(NO3)2(aq) + 2AgCl(aq) ® PbCl2(s) + 2AgNO3(aq)

            A)      I, II, and III                                          D)      II and III only

            B)      I and II only                                          E)      I only

            C)      I and III only                                                 

 

      16.  Consider the following chemical equations.  Select the equations that represent chemical reactions, rather than physical changes.

               I. KNO3(s) ® K+(aq) + NO3?(aq)

              II.  2O3(g) ® 3O2(g)

             III.  HCl(g) + NH3(g) ® NH4Cl(s)

            A)      I, II, and III                                          D)      II and III only

            B)      I and II only                                          E)      II only

            C)      I and III only                                                 

 

      17.  Write a complete, balanced equation for the reaction that occurs when sodium metal reacts with water to form hydrogen gas and aqueous sodium hydroxide.

            A)      Na(s) + H2O(l) ® NaOH(aq) + H(g)

            B)      Na(s) + H2O(l) ® NaOH(aq) + H2(g)

            C)      Na(s) + 2H2O(l) ® NaOH(aq) + 2H2(g)

            D)      Na(s) + 2H2O(l) ® 2NaOH(aq) + 2H2(g)

            E)      2Na(s) + 2H2O(l) ® 2NaOH(aq) + H2(g)

 

      18.  Fireworks which give off bright flashes of white light often contain magnesium metal.  When the magnesium burns in the presence of oxygen, it forms solid magnesium oxide, and emits a bright white light.  Write a complete, balanced equation for this reaction.

            A)      Mg(s) + O2(g) ® MgO2(s)                    D)      2Mg(s) + O2(g) ® 2MgO(s)

            B)      Mg(s) + O(g) ® MgO(s)                       E)      4Mg(s) + O2(g) ® 2Mg2O(s)

            C)      Mg(s) + O2(g) ® MgO(s)                              

 

      19.  Zinc metal will react with aqueous hydrochloric acid to produce aqueous zinc chloride and hydrogen gas.  Write a complete, balanced equation for this reaction.

            A)      Zn(s) + HCl(aq) ® ZnCl(aq) + H(g)

            B)      Zn(s) + HCl(aq) ® ZnCl(aq) + H2(g)

            C)      Zn(s) + 2HCl(aq) ® ZnCl(aq) + H2(g)

            D)      Zn(s) + 2HCl(aq) ® ZnCl2(aq) + H2(g)

            E)      2Zn(s) + 2HCl(aq) ® 2ZnCl(aq) + H2(g)

 

      20.  When solid ammonium carbonate is heated, it decomposes to form ammonia gas, carbon dioxide gas, and water vapor, so that the solid completely disappears.  Write a complete, balanced equation for this reaction.

            A)      NH4CO3(s) ® NH3(g) + CO2(g) + H2O(g)

            B)      NH4CO3(s) ® NH2(g) + CO2(g) + H2O(g)

            C)      (NH4)2CO3(s) ® NH3(g) + CO2(g) + H2O(g)

            D)      (NH4)2CO3(s) ® NH3(g) + CO2(g) + 3H2O(g)

            E)      (NH4)2CO3(s) ® 2NH3(g) + CO2(g) + H2O(g)

 

      21.  Write a balanced equation to represent the reaction shown in the figure.

           

 

            A)      N2  + Cl2  ® 2NCl3                               D)      2N2  + 6Cl2  ® 3NCl4

            B)      N2  + 6Cl2  ® 4NCl3                             E)      2N2  + 5Cl2  ® 3NCl3

            C)      2N2  + 6Cl2  ® 4NCl3                                    

 

      22.  Write a balanced equation to represent the reaction shown in the figure.

           

 

            A)      4CH3 + 6O2 ® 4CO2 + 6H2O               D)      3CH4 + 6O2 ® 3CO + 6H2O

            B)      3CH3 + 6O2 ® 3CO2 + 6H2O               E)      3CH4 + 5O2 ® 3CO2 + 5H2O

            C)      3CH4 + 6O2 ® 3CO2 + 6H2O                       

 

      23.  The gases carbon dioxide and hydrogen can react together to form carbon monoxide gas and water vapor.  Which of the diagrams in the figure could be used to represent this reaction?

           

 

            A)  A    B)  B    C)  C    D)  D    E)  none of these

 

      24.  Balance the following skeletal equation:  C3H8(g) + O2(g) ® CO2(g) + H2O(g).

            A)      C3H8(g) + O2(g) ® 3CO2(g) + 2H2O(g)

            B)      C3H8(g) + O2(g) ® 3CO2(g) + 4H2O(g)

            C)      C3H8(g) + 3O2(g) ® 3CO2(g) + 4H2O(g)

            D)      C3H8(g) + 4O2(g) ® 3CO2(g) + 4H2O(g)

            E)      C3H8(g) + 5O2(g) ® 3CO2(g) + 4H2O(g)

 

      25.  Balance the following skeletal equation:  C2H5OH(l) + O2(g) ® CO2(g) + H2O(g).

            A)      C2H5OH(l) + O2(g) ® CO2(g) + 3H2O(g)

            B)      C2H5OH(l) + O2(g) ® 2CO2(g) + 3H2O(g)

            C)      C2H5OH(l) + 2O2(g) ® 2CO2(g) + 3H2O(g)

            D)      C2H5OH(l) + 3O2(g) ® 2CO2(g) + 3H2O(g)

            E)      2C2H5OH(l) + 3O2(g) ® 4CO2(g) + 3H2O(g)

 

      26.  Balance the following skeletal equation:  Li(s) + H2O(l) ® LiOH(aq) + H2(g).

            A)      Li(s) + H2O(l) ® LiOH(aq) + H2(g)

            B)      Li(s) + 2H2O(l) ® LiOH(aq) + H2(g)

            C)      Li(s) + 2H2O(l) ® 2LiOH(aq) + H2(g)

            D)      Li(s) + 2H2O(l) ® 2LiOH(aq) + 2H2(g)

            E)      2Li(s) + 2H2O(l) ® 2LiOH(aq) + H2(g)

 

      27.  Balance the following skeletal equation:  NH3(g) + O2(g) ® NO2(g) + H2O(g).

            A)      4NH3(g) + 7O2(g) ® 4NO2(g) + 6H2O(g)

            B)      2NH3(g) + 2O2(g) ® 2NO2(g) + 3H2O(g)

            C)      2NH3(g) + O2(g) ® NO2(g) + 2H2O(g)

            D)      NH3(g) + O2(g) ® NO2(g) + 2H2O(g)

            E)      NH3(g) + O2(g) ® NO2(g) + H2O(g)

 

      28.  Balance the following skeletal equation:  CH4(g) ® C2H2(g) + H2(g).

            A)      CH4(g) ® C2H2(g) + H2(g)                   D)      2CH4(g) ® C2H2(g) + 3H2(g)

            B)      2CH4(g) ® C2H2(g) + H2(g)                 E)      4CH4(g) ® 2C2H2(g) + 5H2(g)

            C)      2CH4(g) ® C2H2(g) + 2H2(g)                        

      29.  Balance the following skeletal equation:  

            Pb(NO3)2(aq) + KI(aq) ® PbI2(s) + KNO3(aq)

            A)      Pb(NO3)2(aq) + KI(aq) ® PbI2(s) + KNO3(aq)

            B)      Pb(NO3)2(aq) + 2KI(aq) ® PbI2(s) + KNO3(aq)

            C)      Pb(NO3)2(aq) + 2KI(aq) ® PbI2(s) + 2KNO3(aq)

            D)      2Pb(NO3)2(aq) + 2KI(aq) ® PbI2(s) + 4KNO3(aq)

            E)      2Pb(NO3)2(aq) + 2KI(aq) ® 2PbI2(s) + 4KNO3(aq)

 

      30.  Balance the following skeletal equation:

            Ba(NO3)2(aq) + K2SO4(aq) ® BaSO4(s) + KNO3(aq)

            A)      Ba(NO3)2(aq) + K2SO4(aq) ® BaSO4(s) + KNO3(aq)

            B)      2Ba(NO3)2(aq) + K2SO4(aq) ® 2BaSO4(s) + KNO3(aq)

            C)      2Ba(NO3)2(aq) + 2K2SO4(aq) ® 2BaSO4(s) + 2KNO3(aq)

            D)      2Ba(NO3)2(aq) + 2K2SO4(aq) ® 2BaSO4(s) + 3KNO3(aq)

            E)      Ba(NO3)2(aq) + K2SO4(aq) ® BaSO4(s) + 2KNO3(aq)

 

      31.  Balance the following skeletal equation: 

            HCl(g) + O2(g) ® H2O(l) + Cl2(g)

            A)      HCl(g) + O2(g) ® H2O(l) + Cl2(g)

            B)      2HCl(g) + O2(g) ® H2O(l) + Cl2(g)

            C)      2HCl(g) + O2(g) ® 2H2O(l) + Cl2(g)

            D)      4HCl(g) + O2(g) ® 2H2O(l) + 2Cl2(g)

 

      32.  After the following equation is properly balanced, what is the coefficient in front of O2?   

            S8(s)   +   O2(g)   ®    SO3(g)

            A)  2    B)  3    C)  8    D)  12    E)  16

 

      33.  After the following equation is properly balanced, what is the coefficient in front of O2(g)?   

            PbS(s)  +  O2(g®    PbO(s)   +   SO2(g)

            A)  1    B)  2    C)  3    D)  4    E)  6

 

      34.  When the equation shown is balanced properly, what is the coefficient in front of O2(g)?    

            C6H14(l)  +   O2(g®   CO2(g)  +   H2O(g)

            A)  6    B)  7    C)  9    D)  12    E)  19

 

      35.  When aqueous solutions of hydrochloric acid and sodium carbonate are mixed,

            A)      H2 gas is formed.                                   D)      a precipitate is formed.

            B)      CO2 gas is produced.                            E)      no reaction occurs.

            C)      sodium metal is formed.                                

 

      36.  A reaction which has two elements as reactants and one compound as a product is:

            A)      a decomposition reaction.                     D)      a double-displacement reaction.

            B)      a combination reaction.                         E)      a combustion reaction.

            C)      a single-displacement reaction.                      

 

      37.  A reaction which has one element and one compound as reactants and one element and one compound as products is:

            A)      a decomposition reaction.                     D)      a double-displacement reaction.

            B)      a combination reaction.                         E)      a combustion reaction.

            C)      a single-displacement reaction.                      

      38.  A reaction which has one compound as a reactant and two elements as products is:

            A)      a decomposition reaction.                     D)      a double-displacement reaction.

            B)      a combination reaction.                         E)      a combustion reaction.

            C)      a single-displacement reaction.                      

 

      39.  A reaction which has two compounds as reactants and two compounds as products is:

            A)      a decomposition reaction.                     D)      a double-displacement reaction.

            B)      a combination reaction.                         E)      a combustion reaction.

            C)      a single-displacement reaction.                      

 

      40.  A solution of silver nitrate is mixed with a solution of sodium chloride, resulting in a precipitate of silver chloride and a solution of sodium nitrate.  The class of this reaction is:

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      41.  A piece of magnesium metal is placed in a solution of hydrochloric acid, resulting in the formation of hydrogen gas and a solution of magnesium chloride.  The class of this reaction is:

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      42.  A piece of magnesium metal is burned in air (containing oxygen gas), and a white powder of magnesium oxide is formed. 

            The class of this reaction is:

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

            Ans:  B

 

43. Crystals of red mercury(II) oxide, when heated, form liquid mercury and oxygen gas. 

            The class of this reaction is:

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      44.  Classify the following reaction:  2C8H18(l)  +  25O2(g)  ®  16CO2(g)  +  18H2O(g)

            A)      combination                                           D)      double-displacement

            B)      decomposition                                       E)      combustion

            C)      single-displacement                                        

 

      45.  The class of the reaction shown in the figure is:

           

 

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      46.  The class of the reaction shown in the figure is:

           

 

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      47.  The class of the reaction shown in the figure is:

           

 

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      48.  The class of the reaction shown in the figure is:

           

 

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      49.  The class of the reaction shown in the figure is:

           

 

            A)      decomposition reaction.                        D)      double-displacement reaction.

            B)      combination reaction.                            E)      combustion reaction.

            C)      single-displacement reaction.                         

 

      50.  When aqueous solutions of H2SO4 and NaOH are mixed, _______ will occur.

            A)      a combination reaction                          D)      a double-displacement reaction

            B)      a decomposition reaction                      E)      no reaction

            C)      a single-displacement reaction                       

 

      51.  Sodium metal reacts with water in a single-displacement reaction.  Which of the following best describes the identity of the products of this reaction?

            A)      NaH(aq) and O2(g)                               D)      NaOH(aq) and H2(g)

            B)      NaH2(aq) and O(g)                                E)      NaOH2(aq)

            C)      NaOH(aq) and H(g)                                      

 

      52.  What is the product of the combination reaction that occurs when magnesium metal reactions with oxygen gas?

            A)  MgO2(s)    B)  MgO(s)    C)  Mg2O(s)    D)  Mg2O3(s)    E)  Mg2O2(s)

 

      53.  What is the correct formula for the product of the combination reaction between calcium metal and oxygen gas?

            A)  CaO(s)    B)  CaO2(s)    C)  Ca2O(s)    D)  Ca2O2(s)    E)  Ca2O3(s)

 

      54.  What are the products of the combustion reaction of methane, CH4, with oxygen?

            A)      CO2(g) only                                           D)      CO2(g) and H2O(g)

            B)      CO(g) and H2(g)                                   E)      H2CO3(aq)

            C)      C(s), and H2O(g)                                            

 

      55.  Write and balance the equation for the decomposition reaction that occurs when Mercury(II) oxide decomposes to its elements.

            A)      2HgO(s®  2Hg(l)  + O2(g)                D)      HgO2(s®  Hg(l)  + 2O(g)

            B)      Hg2O(s®  2Hg(l)  + O2(g)                 E)      2Hg(l)  +O2(g) ® HgO2(s)

            C)      HgO(s®  Hg(l)  + O2(g)                             

 

      56.  When heated, calcium carbonate (limestone) undergoes a decomposition reaction.  Write a balanced equation for this reaction.

            A)      CaCO3(s) ®  Ca(s) + CO3(g)                D)      2CaCO3(s) ®  2CaO(s) + CO2(g)

            B)      CaCO3(s) ®  Ca(s) + CO2(g)                E)      2CaCO3(s) ®  2CaO(s) + 3CO2(g)

            C)      CaCO3(s) ®  CaO(s) + CO2(g)                     

 

      57.  Write and balance the equation for the decomposition reaction that occurs when solid copper(II) hydroxide, Cu(OH)2, is heated.

            A)      Cu(OH)2(s) ®  Cu(s) + 2OH(g)           D)      Cu(OH)2(s) ®  CuO(s) + H2O(g)

            B)      Cu(OH)2(s) ®  Cu(s) + (OH)2(g)          E)      2Cu(OH)2(s) ®  2CuO(s) + H2O(g)

            C)      Cu(OH)2(s) ®  Cu(s) + H2O(g)                     

 

      58.  Write and balance the equation for the decomposition reaction that occurs when solid magnesium sulfate trihydrate, MgSO4?3H2O, is heated.

            A)      MgSO4?3H2O(s) ® Mg(s) +  SO4?3H2O(s)

            B)      MgSO4?3H2O(s) ® MgSO4?3H2O(s)

            C)      MgSO4?3H2O(s) ® MgSO4(s)  + 3H2O(g)

            D)      MgSO4?3H2O(s) ® MgSO4(s)  + H2O(g)

            E)      MgSO4?3H2O(s) ® MgS(s)  + 6H2O(g)

 

      59.  Write and balance the equation for the combination reaction that occurs when solid potassium metal reacts with chlorine gas.

            A)      K(s) + Cl(g) ® KCl(s)                          D)      2K(s) + Cl2(g) ® 2KCl(s)

            B)      K(s) + Cl2(g) ® KCl(s)                         E)      2K(s) + Cl2(g) ® 2ClK(s)

            C)      2K(s) + Cl2(g) ® KCl(s)                                

 

      60.  Which of the following equations best describes the reaction that occurs when potassium metal reacts with oxygen gas in a combination reaction?

            A)      K(s)  +  O(g®  KO(s)                        D)      2K(s)  +  O(g®  K2O(s)

            B)      K(s)  +  O2(g®  KO2(s)                     E)      K(s)  +  O2(g®  KO(s)  + O(g)

            C)      4K(s)  +  O2(g®  2K2O(s)                          

 

      61.  Write and balance the equation for the combination reaction that occurs when sulfur dioxide gas, SO2, reacts with oxygen gas.

            A)      SO2(g) + O2(g) ® SO4(g)                     D)      2SO2(g) + 2O2(g) ® 2SO3(g)

            B)      SO2(g) + O2(g) ® SO3(g)                     E)      3SO2(g) + 2O2(g) ® 3SO3(g)

            C)      2SO2(g) + O2(g) ® 2SO3(g)                          

 

      62.  Write and balance the equation for the combination reaction that occurs when aluminum metal reacts with oxygen gas.

            A)      Al(s) + O2(g) ® AlO(s)                        D)      2Al(s) + 2O2(g) ® Al2O3(s)

            B)      Al(s) + O2(g) ® AlO2(s)                       E)      4Al(s) + 3O2(g) ® 2Al2O3(s)

            C)      2Al(s) + 2O2(g) ® 2AlO2(s)                          

 

      63.  When zinc metal is placed into a copper(II) nitrate solution, a single-displacement reaction occurs.  Write a balanced equation to describe this reaction.

            A)      Zn(s) + Cu(NO3)2(aq) ® ZnNO3(aq) + CuNO3(aq)

            B)      Zn(s) + Cu2NO3(aq) ® ZnNO3(aq) + Cu(aq)

            C)      Zn(s) + Cu(NO3)2(aq) ® Zn(NO3)2(aq) + Cu(s)

            D)      2Zn(s) + Cu(NO3)2(aq) ® 2Zn(NO3)2(aq) + Cu(s)

            E)      Zn(s) + Cu2NO3(aq) ® ZnNO3(aq) + 2Cu(aq)

 

      64.  When copper metal is placed into a silver nitrate solution, a single-displacement reaction occurs, forming a copper(II) compound.  Write a balanced equation to describe this reaction.

            A)      Cu(s) + Ag(NO3)2(aq) ® CuNO3(aq) + AgNO3(aq)

            B)      Cu(s) + AgNO3(aq) ® CuNO3(aq) + Ag(aq)

            C)      Cu(s) + Ag(NO3)2(aq) ® Cu(NO3)2(aq) + Ag(s)

            D)      2Cu(s) + Ag(NO3)2(aq) ® 2Cu(NO3)2(aq) + Ag(s)

            E)      Cu(s) + 2AgNO3(aq) ® Cu(NO3)2(aq) + 2Ag(s)

 

      65.  When calcium metal is placed in water, a single-displacement reaction occurs.  Write a balanced equation to describe this reaction.

            A)      Ca(s) + H2O(l) ® CaO(aq) + H2(g)

            B)      Ca(s) + H2O(l) ® CaO(s) + H2(g)

            C)      Ca(s) + H2O(l) ® Ca(OH)2(aq) + H2(g)

            D)      Ca(s) + 2H2O(l) ® Ca(OH)2(aq) + H2(g)

            E)      2Ca(s) + 2H2O(l) ® 2Ca(OH)2(aq) + H2(g)

 

      66.  Predict which of the following reactions will occur? 

            (i)   Ni(s)  +  FeCl2(aq®  NiCl2(aq)  +  Fe(s)

            (ii)  2Al(s)  +  3NiCl2(aq®  2AlCl3(aq)  +  3Ni(s)

            (ii)  Fe(s)  +  CuCl2(aq®  FeCl2(aq)  +  Cu(s)

            A)  i only    B)  ii only    C)  iii only    D)  ii and iii    E)  All three will occur.

 

      67.  Which of the metals (Fe, Zn, Mg) will react in an aqueous solution of Al(NO3)3 to produce aluminum metal?

            A)  Fe    B)  Zn    C)  Mg    D)  All of these    E)  None of these

 

      68.  When potassium metal is placed in water, will a reaction occur?  If so, what is the balanced equation for the reaction?

            A)      No reaction will occur.

            B)      Yes.  2K(s) + 2H2O(l) ® 2K(OH)2(aq) + H2(g)

            C)      Yes.  2K(s) + 2H2O(l) ® 2KOH(aq) + H2(g)

            D)      Yes.  2K(s) + 2H2O(l) ® 2KH2O(aq)

            E)      Yes.  2K(s) + 2H2O(l) ® 2KOH(aq) + 2H2(g)

 

      69.  When iron metal is placed into a solution of hydrochloric acid, will a reaction occur?  If so, what is the balanced equation for the reaction?

            A)      No reaction will occur.

            B)      Yes.  2Fe(s) + 2HCl(aq) ® 2FeCl(aq) + H2(g)

            C)      Yes.  Fe(s) + 2HCl(aq) ® FeCl2(aq) + H2(g)

            D)      Yes.  Fe(s) + 3HCl(aq) ® FeCl3(aq) + H2(g)

 

      70.  When copper metal is placed in a solution of zinc nitrate, will a reaction occur?  If so, what is the balanced equation for the reaction?

            A)      Yes.  Cu(s) + Zn(NO3)2(aq) ® CuNO3(aq) + ZnNO3(aq)

            B)      Yes.  Cu(s) + Zn2NO3(aq) ® CuNO3(aq) + Zn(aq)

            C)      Yes.  Cu(s) + Zn(NO3)2(aq) ® Cu(NO3)2(aq) + Zn(s)

            D)      No reaction will occur.

            E)      Yes.  Cu(s) + Zn2NO3(aq) ® CuNO3(aq) + 2Zn(aq)

 

      71.  When copper metal is placed in a solution of platinum(II) chloride, will a reaction occur?  If so, what is the balanced equation for the reaction?

            A)      Yes.  Cu(s) + PtCl2(aq) ® CuCl(aq) + PtCl(aq)

            B)      Yes.  Cu(s) + Pt2Cl(aq) ® CuCl(aq) + Pt(aq)

            C)      Yes.  Cu(s) + PtCl2(aq) ® CuCl2(aq) + Pt(s)

            D)      No reaction will occur.

            E)      Cu(s) + Pt2Cl(aq) ® CuCl(aq) + 2Pt(aq)

 

      72.  When aqueous solutions of sodium chloride and silver nitrate are mixed, a double-displacement reaction occurs.  What is the balanced equation for the reaction?

            A)      NaCl(aq) + AgNO3(aq) ® Na(s) + AgNO3Cl(aq)

            B)      NaCl(aq) + AgNO3(aq) ® NaNO3(aq) + AgCl(aq)

            C)      NaCl(aq) + AgNO3(aq) ® NaNO3(aq) + AgCl(s)

            D)      NaCl(aq) + AgNO3(aq) ® NaNO3(aq) + ClAg(s)

            E)      NaCl(aq) + AgNO3(aq) ® NaNO3(aq) + 3AgCl(s)

 

      73.  When aqueous solutions of potassium chloride and lead(II) nitrate are mixed, a double-displacement reaction occurs.  What is the balanced equation for the reaction?

            A)      KCl(aq) + Pb(NO3)2(aq) ® K(s) + PbNO3Cl(aq)

            B)      KCl(aq) + Pb2NO3(aq) ® KNO3(aq) + PbCl(aq)

            C)      KCl(aq) + Pb2NO3(aq) ® KNO3(aq) + 2PbCl(s)

            D)      2KCl(aq) + Pb(NO3)2(aq) ® KNO3(aq) + ClPb(s)

            E)      2KCl(aq) + Pb(NO3)2(aq) ® 2KNO3(aq) + PbCl2(s)

      74.  If solutions of potassium carbonate and calcium nitrate are mixed, will a double-displacement reaction occur?  If so, what is the balanced equation for the reaction?

            A)      No reaction will occur.

            B)      Yes.  K2CO3(aq) + Ca(NO3)2(aq) ® KNO3(aq) + CaK(s)

            C)      Yes.  K2CO3(aq) + Ca(NO3)2(aq) ® KNO3(aq) + CaCO3(s)

            D)      Yes.  K2CO3(aq) + Ca(NO3)2(aq) ® 2KNO3(aq) + CaCO3(s)

            E)      Yes.  K2CO3(aq) + Ca(NO3)2(aq) ® K2(NO3)2(aq) + CaCO3(s)

      75.  If solutions of potassium chromate and calcium nitrate are mixed, will a double-displacement reaction occur?  If so, what is the balanced equation for the reaction?

            A)      No reaction will occur.

            B)      Yes.  K2CrO4(aq) + Ca(NO3)2(aq) ® KNO3(aq) + CaK(s)

            C)      Yes.  K2CrO4(aq) + Ca(NO3)2(aq) ® KNO3(aq) + CaCrO4(s)

            D)      Yes.  K2CrO4(aq) + Ca(NO3)2(aq) ® 2KNO3(aq) + CaCrO4(s)

            E)      Yes.  K2CrO4(aq) + Ca(NO3)2(aq) ® K2(NO3)2(aq) + CaCrO4(s)

 

      76.  Which of the following ionic compounds would be expected to be insoluble in water?

            A)  NaCl    B)  KOH    C)  AgI    D)  Li2SO4    E)  Ca(CH3CO2)2

      77.  Which of the following ionic compounds would be expected to be insoluble in water?

            A)  KCl    B)  PbI2    C)  NH4NO3    D)  CuSO4    E)  NaCH3CO2

 

      78.  Which of the following ionic compounds would be expected to be insoluble in water?

            A)  CaS    B)  Ca(NO3)2    C)  Na2SO4    D)  KI    E)  NaOH

 

      79.  Consider the reaction CaCO3(s) + 2HCl(aq) ® CaCl2(aq) + CO2(g) + H2O(l).  The driving force that causes the reaction to go to completion is:

            A)      formation of a precipitate.                     D)      none of  these.

            B)      formation of an insoluble gas.               E)      formation of an element.

            C)      formation of a soluble salt.                            

 

      80.  Consider the reaction Ca(OH)2(aq) + 2HCl(aq) ® CaCl2(aq) + 2H2O(l).  The driving force that causes the reaction to go to completion is:

            A)      formation of a precipitate.                     D)      formation of water.

            B)      formation of an insoluble gas.               E)      formation of an element.

            C)      formation of a soluble salt.                            

 

      81.  When aqueous solutions of K2CO3 and CaCl2 are mixed, what is the correct formula for the precipitate that forms?

            A)  KCl(s)    B)  K2Cl2(s)    C)  CaCO3(s)    D)  K2Ca(s)    E)  ClCO3(s)

 

      82.  When aqueous solutions of NaOH and MgCl2 are mixed, a precipitate forms.  What is the correct formula for the precipitate?

            A)  NaCl(s)    B)  NaCl2(s)    C)  MgCl2(s)    D)  MgOH(s)    E)  Mg(OH)2(s)

 

      83.  Complete and balance the equation for the reaction that occurs when HCl(aq) and Mg(OH)2(aq) are mixed.  This reaction occurs in your stomach if you take Milk of Magnesia®.

            A)      HCl(aq) + Mg(OH)2(aq) ® MgCl2(aq) + H2O(l)

            B)      2HCl(aq) + Mg(OH)2(aq) ® MgCl2(aq) + H2O(l)

            C)      2HCl(aq) + Mg(OH)2(aq) ® MgCl2(aq) + 2H2O(l)

            D)      HCl(aq) + Mg(OH)2(aq) ® MgCl(aq) + H2O(l)

            E)      2HCl(aq) + Mg(OH)2(aq) ® MgCl2(aq) + H2(g)

 

      84.  Complete and balance the equation for the reaction that occurs when H2SO4(aq) and NaOH(aq) are mixed.

            A)      H2SO4(aq) + NaOH(aq) ® NaSO4(aq) + H2(g)

            B)      H2SO4(aq) + NaOH(aq) ® NaSO4(aq) + H2O(l)

            C)      H2SO4(aq) + 2NaOH(aq) ® Na2SO4(aq) + H2O(l)

            D)      H2SO4(aq) + 2NaOH(aq) ® Na2SO4(aq) + 2H2O(l)

            E)      2H2SO4(aq) + 2NaOH(aq) ® Na2SO4(aq) + 2H2O(l)

 

      85.  Complete and balance the equation for the reaction that occurs when HBr(aq) and KOH(aq) are mixed.

            A)      HBr(aq) + KOH(aq) ® KBr(aq) + H2O(l)

            B)      2HBr(aq) + KOH(aq) ® Br2(l) + H2O(l)

            C)      2HBr(aq) + KOH(aq) ® KBr(aq) + H2O(l)

            D)      HBr(aq) + KOH(aq) ® BrOH(aq) + KH(aq)

            E)      HBr(aq) + KOH(aq) ® KBrO(aq) + H2(g)

 

      86.  When powdered sulfur burns in air, a purple flame is produced, as well as a toxic, foul-smelling gas.  Write a balanced equation for the reaction between sulfur and oxygen gas.

            A)      S8(s) + O2(g) ®  SO2(g)                        C)      S8(s) + 8O2(g) ®  8SO2(g)

            B)      S8(s) + 4O2(g) ®  8SO2(g)                    D)      2S8(s) + 8O2(g) ®  8SO2(g)

      87.  When acetylene gas, C2H2, burns in air, a combustion reaction occurs.  Write a balanced equation to represent this reaction, which occurs when welding torches are used.

            A)      C2H2(g) + O2(g) ®  C2H2O2(g)

            B)      C2H2(g) + O2(g) ®  C2O2(g) + H2(g)

            C)      C2H2(g) + O2(g) ®  CO2(g) + H2O(g)

            D)      C2H2(g) + O2(g) ®  2CO2(g) + H2O(g)

            E)      2C2H2(g) + 5O2(g) ®  4CO2(g) + 2H2O(g)

 

      88.  Sterno, or “canned heat,” contains methanol, CH3OH, and is used for heating containers of food.  Write a balanced equation to represent the combustion reaction that occurs when methanol burns in air.

            A)      CH3OH(l) + O2(g) ®  CH4O3(g)

            B)      2CH3OH(l) + O2(g) ®  C2O2(g) + H2(g)

            C)      CH3OH(l) + O2(g) ®  CO2(g) + H2O(g)

            D)      2CH3OH(l) + 3O2(g) ®  2CO2(g) + 4H2O(g)

            E)      2CH3OH(l) + 6O2(g) ®  2CO2(g) + 4H2O(g)

 

      89.  Would an aqueous solution of CH3OH contain ions?  If so, indicate the formulas of the ions in the solution.

            A)      No, this substance would not form ions in solution.

            B)      Yes.  CH3+(aq) + OH?(aq)

            C)      Yes.  CH3?(aq) + OH+(aq)

            D)      Yes.  CH4+(aq) + O?(aq)

            E)      Yes.  CH42+(aq) + O2?(aq)

 

      90.  Would an aqueous solution of K2SO4 contain ions?  If so, indicate the formulas of the ions in the solution.

            A)      No, this substance would not form ions in solution.

            B)      Yes.  K2+(aq) + SO4?(aq)

            C)      Yes.  K22+(aq) + SO42?(aq)

            D)      Yes.  2K+(aq) + SO42?(aq)

            E)      Yes.  2K+(aq) + S2?(aq) + 4O2?(aq)

 

      91.  Would an aqueous solution of KOH contain ions?  If so, indicate the formulas of the ions in the solution.

            A)      No, this substance would not form ions in solution.

            B)      Yes.  K+(aq) + O2?(aq) + H+(aq)

            C)      Yes.  K+(aq) + OH?(aq)

            D)      Yes.  K?(aq) + OH+(aq)

            E)      Yes.  K+(aq) + H2O(l)

 

      92.  When writing a net ionic equation, how would Mg(NO3)2(aq) be represented?

            A)      Mg2+(aq)  +  2NO3(aq)                        D)      Mg(aq)  +  N2(aq)  + 3O2(aq)

            B)      Mg2+(aq)  +  NO3(aq)                          E)      Mg2+(aq)  +  2N3–(aq) + 6O2–(aq)

            C)      Mg2+(aq)  +  (NO3)2(aq)                               

 

      93.  Write and balance a net ionic equation for the reaction between hydrochloric acid and potassium hydroxide.

            A)      HCl(aq) + KOH(aq® KCl(aq) + H2O(l)

            B)      H+(aq) + O2?(aq) ® OH?(aq)

            C)      H+(aq) + OH?(aq) ® H2O(l)

            D)      Cl?(aq) + OH+(aq) ® OHCl(aq)

            E)      K+(aq) + Cl?(aq) ® KCl(aq)

 

      94.  Write and balance a net ionic equation for the reaction between iron(II) chloride and potassium hydroxide to form iron(II) hydroxide and potassium chloride.

            A)      Fe2Cl(aq) + OH?(aq) ® FeOH(s) + Cl?(aq)

            B)      Fe2+(aq) + OH?(aq) ® FeOH(s)

            C)      Fe2+(aq) + 2OH?(aq) ® Fe(OH)2(s)

            D)      2Cl?(aq) + 2K+(aq) ® 2KCl(s)

            E)      2Cl?(aq) + 2K+(aq) ® 2K(s) + Cl2(g)

 

      95.  Write and balance a net ionic equation for the reaction between copper(II) chloride and zinc metal to form copper metal and zinc chloride.

            A)      Cu2Cl(aq) + Zn(s) ® 2Cu(s) + Zn+(aq) + Cl?(aq)

            B)      Cu2+(aq) + Zn(s) ® Cu(s) +  Zn2+(aq)

            C)      2Cu+(aq) + Zn(s) ® 2Cu(s) +  Zn2+(aq)

            D)      Cu2+(aq) + 2Cl?(aq) + Zn(s) ® Cu(s) +  Zn2+(aq) + 2Cl?(aq)

            E)      CuCl+(aq) + Zn(s) ® Cu(s) +  Zn2+(aq) + Cl?(aq)

 

      96.  Identify the spectator ion(s) in the following reaction:

            Zn(s)  + Cu(NO3)2(aq) ® Cu(s)  + Zn(NO3)2(aq)

            A)      Zn2+(aq) and Cu2+(aq)                           D)      NO3(aq) only

            B)      Zn2+(aq) and NO3(aq)                          E)      There are no spectator ions.

            C)      Cu2+(aq) and NO3(aq)                                  

 

      97.  Identify the spectator ions in the following reaction:  

            Zn(s)  +  2HNO3(aq®  Zn(NO3)2(aq)  +  H2(g)

            A)      Zn2+(aq) and NO3(aq)                          D)      Zn2+(aq) only

            B)      H+(aq) and NO3(aq)                            E)      There are no spectator ions.

            C)      NO3(aq) only                                                

 

      98.  Identify the spectator ions in the following reaction:  

            H2SO4(aq)  +  2KOH(aq®  K2SO4(aq)  +  2H2O(l)

            A)      H+(aq) and OH(aq)

            B)      K+(aq) and SO42–(aq)

            C)      K+(aq), NO3(aq) , H+(aq), and OH(aq)

            D)      SO42–(aq) only

            E)      There are no spectator ions.

 

      99.  When balancing a chemical equation, it is acceptable to change the subscripts on the formulas of the skeletal equation.

 

    100.  When one compound is converted into two elements during a chemical reaction, a decomposition reaction has occurred.

 

    101.  When two compounds react to form two new compounds as products no reaction has occurred.

 

    102.  The molecular-level diagram shows a combination reaction occurring.

 

    103.  When aqueous solutions of barium chloride and sodium sulfate are mixed, no reaction will occur.

 

    104.  The molecular-level diagram shows a substance which is a nonelectrolyte.

 

    105.  When writing a net ionic equation, Cu(s) is the same as Cu2+(aq), so if these species appear on opposite sides of the equation, they would be cancelled.

 

    106.  The activity series is used to predict if a proposed double-displacement reaction will occur.

 

    107.  The compound PbCl2 would be expected to be water-soluble.

 

    108.  The net ionic equation for the acid-base neutralization reaction between HCl(aq) and NaOH(aq) is:  H+(aq) + OH?(aq) ® H2O(l).

 

    109.  Examine the photograph.  Note any evidence of the occurrence of a chemical reaction.

          

 

    110.  Examine the molecular-level diagram.  Is a chemical reaction occurring?  Explain your answer.

           

 

    111.  Examine the molecular-level diagram.  Is a chemical reaction occurring?  Explain your answer.

 

    112.  Write a complete, balanced equation for the reaction that occurs when solutions of potassium hydrogen carbonate and hydroiodic acid react to form potassium iodide, water, and carbon dioxide.  (One of the products, potassium iodide, is a dietary supplement used to prevent iodine deficiency.)

 

    113.  What is the class of the reaction in question 92?

 

    114.  Write a complete, balanced equation for the reaction that occurs when aluminum metal reacts with oxygen gas to form aluminum oxide.

 

    115.  What is the class of the reaction in question 94?

 

    116.  Balance the skeletal equation given for the reaction of octane, C8H18, a component of gasoline with oxygen gas:  C8H18(l) + O2(g) ®  CO2(g) + H2O(l)

 

    117.  What is the class of the reaction in question 96?

 

    118.  Balance the skeletal equation given for the reaction of magnesium metal with hydrochloric acid:  Mg(s) + HCl(aq) ®  MgCl2(aq) + H2(g)

 

    119.  What is the class of the reaction in question 98?

 

    120.  A reaction occurs when a piece of silvery metal is placed in a solution of HCl(aq).  Is the metal zinc or silver?  How would you know?

 

    121.  Indicate whether KOH(aq) is an electrolyte or a non electrolyte.

 

    122.  Indicate whether HBr(aq) is an electrolyte or a non electrolyte.

 

    123.  Indicate whether CH3OH(aq) is an electrolyte or a non electrolyte.

 

    124.  Indicate whether CaCl2(aq) is an electrolyte or a non electrolyte.

 

    125.  Would an aqueous solution of (NH4)2CO3 contain ions?  If so, write the formulas for the ions in the solution.

 

    126.  Would an aqueous solution of MgBr2 contain ions?  If so, write the formulas for the ions in the solution.

 

    127.  Would an aqueous solution of C2H5OH contain ions?  If so, write the formulas for the ions in the solution.

 

    128.  Predict whether a reaction will occur when aqueous solutions of silver nitrate and potassium bromide are mixed.  If so, write balanced molecular and net ionic equations for the reaction.

 

    129.  Predict whether a reaction will occur when a piece of copper metal is placed into an aqueous solution of silver nitrate.  If so, write balanced molecular and net ionic equations for the reaction.

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