Fill This Form To Receive Instant Help

Help in Homework
trustpilot ratings
google ratings


Homework answers / question archive / Chapter 14: Oxidation-Reduction Reactions 1)Which of the following statements regarding oxidation-reduction reactions is correct?             A)      Oxidation-reduction reactions involve sharing electrons

Chapter 14: Oxidation-Reduction Reactions 1)Which of the following statements regarding oxidation-reduction reactions is correct?             A)      Oxidation-reduction reactions involve sharing electrons

Chemistry

Chapter 14: Oxidation-Reduction Reactions

1)Which of the following statements regarding oxidation-reduction reactions is correct?

            A)      Oxidation-reduction reactions involve sharing electrons.

            B)      Oxidation can occur without reduction.

            C)      You can tell that a substance is oxidized if it loses electrons.

            D)      You can tell that a substance is reduced if its oxidation number increases.

            E)      None of these statements is correct.

        2.  All of these statements concerning oxidation are correct except that

            A)      oxygen is necessary for oxidation to take place.

            B)      the oxidizing agent receives electrons from another species.

            C)      oxidation must accompany reduction.

            D)      the oxidizing agent increases the oxidation number of another element.

            E)      the oxidation of a metal produces positive ions.

 

        3.  Which one of the following reactions is an example of an oxidation-reduction reaction?

            A)      BaO(s) + CO2(g) ® BaCO3(s)

            B)      H2(g) + F2(g) ® 2HF(g)

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

            D)      HCl(aq) + NaOH(aq) ® NaCl(aq) + H2O(l)

            E)      Ba2+(aq) + SO42–(aq) ® BaSO4(s)

 

        4.  Which of the following reactions is not an oxidation-reduction reaction?

            A)      C(s) + CO2(g) ® CO2(g)

            B)      CO(g) + Cl2(g) ® COCl2(g)

            C)      2H2O2(l) ® 2H2O(l) + O2(g)

            D)      CaCO3(s) + 2HCl(aq) ® CaCl2(aq) + CO2(g) + H2O(l)

            E)      2HI(g) ® H2(g) + I2(g)

        5.  When a strip of zinc metal is placed in a blue aqueous solution of copper(II) sulfate, the surface of the zinc becomes coated with a reddish solid, and the zinc begins to dissolve to form aqueous zinc sulfate.  Which of the following statements regarding this reaction is correct?

            A)      The copper(II) is being oxidized.

            B)      The zinc is being reduced.

            C)      The sulfate ion is being reduced.

            D)      The solution will lose its blue color as the reaction progresses.

            E)      The reaction described is nonspontaneous.

 

        6.  When a piece of copper wire is placed in a colorless solution of silver nitrate, the surface of the wire becomes coated with a shiny silvery material, and the copper begins to form aqueous copper(II) nitrate, which is blue.  Which of the following statements regarding this reaction is correct?

            A)      The copper(II) is being oxidized.

            B)      The silver ion is being oxidized.

            C)      The nitrate ion is being reduced.

            D)      The solution will become more blue as the reaction progresses.

            E)      The reaction described is nonspontaneous.

        7.  Consider the following reaction:

            Mg(s) + ZnSO4(aq) ® MgSO4(aq) + Zn(s)

            Which of the following statements regarding this reaction is correct?

            A)      Magnesium is neither oxidized nor reduced.

            B)      The sulfate ion is reduced.

            C)      Zinc is the reducing agent.

            D)      Magnesium is the oxidizing agent.

            E)      Zinc gains two electrons.

 

        8.  Consider the following reaction:

            Mn(s) + CuSO4(aq) ® MnSO4(aq) + Cu(s)

            Which of the following statements regarding this reaction is correct?

            A)      Manganese is neither oxidized nor reduced.

            B)      The sulfate ion is oxidized.

            C)      Copper is the reducing agent.

            D)      Manganese is the oxidizing agent.

            E)      Each copper gains two electrons.

 

        9.  Consider the following reaction:

            Mg(s) + NiSO4(aq) ® MgSO4(aq) + Ni(s)

            Which of the following statements regarding this reaction is correct?

            A)      Each magnesium atom gains two electrons.

            B)      The sulfate ion is reduced.

            C)      Nickel ion is the oxidizing agent.

            D)      Magnesium is reduced.

            E)      Each nickel ion loses two electrons.

 

      10.  In which of the following choices is the oxidation number incorrect?

            A)      Fe2+(aq); oxidation number = 2+          D)      Cu2+(aq); oxidation number = 2+

            B)      Cl-(aq); oxidation number = 1–            E)      C(s); oxidation number = 0

            C)      H2(s); oxidation number = 1+                        

      11.  In which of the following choices is the oxidation number incorrect?

            A)      Fe3+(aq); oxidation number = 3+          D)      Cu+(aq); oxidation number = 1+

            B)      I-(aq); oxidation number = 1–              E)      Ni(s); oxidation number = 0

            C)      Cl2(s); oxidation number = 1–                        

      12.  In which of the following choices is the oxidation number incorrect?

            A)      Al3+(aq); oxidation number = 3+          D)      Na+(aq); oxidation number = 1+

            B)      F-(aq); oxidation number = 1–              E)      Cu(s); oxidation number = 2+

            C)      Br2(s); oxidation number = 0                         

      13.  In which of the following choices is the oxidation number incorrect?

            A)      Cr3+(aq); oxidation number = 3+          D)      K+(aq); oxidation number = 1+

            B)      Cl-(aq); oxidation number = 1–            E)      Ag(s); oxidation number = 1+

            C)      F2(g); oxidation number = 0                           

 

      14.  In which compound does bromine have an oxidation number of 3+?

            A)  Br2O    B)  BrO3    C)  Br2O3    D)  BrO2    E)  Br2O5

 

      15.  In which compound does phosphorus have an oxidation number of 3+?

            A)  AlPO4    B)  PF5    C)  H3PO4    D)  H3PO3    E)  PH3

 

      16.  In which substance does chlorine have an oxidation number of 4+?

            A)  KClO4    B)  Cl2    C)  ClO2    D)  Cl2O7    E)  NaCl

 

      17.  In which substance does chlorine have an oxidation number of 7+?

            A)  KClO4    B)  Cl2    C)  ClO2    D)  NaClO    E)  NaCl

 

      18.  In which compound does phosphorus have an oxidation number of 3–?

            A)  AlPO4    B)  PF5    C)  H3PO4    D)  H3PO3    E)  PH3

 

      19.  The ion shown has a charge of 2–.  What are the oxidation numbers of the atoms in the ion?

           

 

            A)      S = 0, O = 2–                                         D)      S = 6+, O = 2–

            B)      S = 2–, O = 0                                         E)      S = 4+, O = 1–

            C)      S = 8+, O = 2–                                               

 

      20.  What are the oxidation numbers of the atoms in the MnO4- ion?

            A)      Mn = 0, O = 1–                                     D)      Mn = 8+, O = 2–

            B)      Mn = 3+, O = 1–                                   E)      Mn = 1–, O = 0

            C)      Mn = 7+, O = 2–                                            

 

      21.  What are the oxidation numbers of the atoms in the Cr2O72- ion?

            A)      Cr = 1–, O = 0                                       D)      Cr = 7+, O = 2–

            B)      Cr = 0, O = 2–                                       E)      Cr = 3+, O = 1–

            C)      Cr = 6+, O = 2–                                             

 

      22.  What are the oxidation numbers of the atoms in the AsO43- ion?

            A)      As = 0, O = 1–                                      D)      As = 3+, O = 2–

            B)      As = 1+, O = 1–                                    E)      As = 5+, O = 2–

            C)      As = 3–, O = 0                                               

 

      23.  What is the oxidation number of sulfur in S2O32–?

            A)  +6    B)  –2    C)  +4    D)  +2    E)  +3

      24.  What is the oxidation number of chlorine in sodium perchlorate, NaClO4?

            A)  +8    B)  –7    C)  +16    D)  +7    E)  –8

 

      25.  What is the oxidation number of boron in sodium tetraborate, Na2B4O7?

            A)  +12    B)  –3    C)  +14    D)  +3    E)  +4

 

      26.  In which of the following does chlorine have an oxidation number of +3?

            A)  HCl    B)  HOCl    C)  HClO2    D)  HClO3    E)  HClO4

 

      27.  Which of the following sulfur species cannot be further reduced?

            A)  H2SO3    B)  SO42–    C)  S2O32–    D)  SO32–    E)  S2–

 

      28.  Consider the reaction:

            Ba(NO3)2(aq) + Na2SO4(aq) ® BaSO4(s) + 2NaNO3(aq)

            Which of the following statements is correct?

            A)      Barium is oxidized.

            B)      Sodium is reduced.

            C)      Nitrate ion is the reducing agent.

            D)      Sulfate ion is the oxidizing agent.

            E)      This reaction is not an oxidation-reduction reaction.

 

      29.  Consider the reaction:

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

            Which of the following statements is correct?

            A)      Calcium is reduced.                               D)      Oxygen is the reducing agent.

            B)      Hydrogen is oxidized.                           E)      Calcium is oxidized.

            C)      Oxygen is oxidized.                                       

 

      30.  The change, Br2 + H2O ® HOBr + HBr, is

            A)      oxidation only.                                      D)      neither oxidation nor reduction.

            B)      reduction only.                                      E)      an acid-base reaction.

            C)      both oxidation and reduction.                       

 

      31.  Consider the reaction:

            2HgO(s) ® 2Hg(l) + O2(g)

            Which of the following statements is correct?

            A)      Mercury is reduced.                              D)      Oxide ion is the reducing agent.

            B)      Oxygen is oxidized.                              E)      All of these statements are correct.

            C)      Mercury(II) ion is the oxidizing agent.          

 

      32.  Consider the reaction:

            N2(g) + 3H2(g) ® 2NH3(g)

            Which of the following statements is correct?

            A)      Nitrogen is oxidized.

            B)      Hydrogen is reduced.

            C)      Nitrogen is the reducing agent.

            D)      The reaction is not an oxidation-reduction reaction.

            E)      Hydrogen is the reducing agent.

 

      33.  Consider the reaction:

            CH4(g) + 2O2(g) ® CO2(g) +  2H2O(g)

            Which of the following statements is correct?

            A)      Carbon is oxidized.

            B)      Oxygen is the reducing agent.

            C)      Oxygen is oxidized.

            D)      Carbon is the oxidizing agent.

            E)      The reaction is not an oxidation-reduction reaction.

 

      34.  Consider the following oxidation-reduction reaction:

            2Fe3+(aq) + 2Hg(l) + 2Cl(aq) ® 2Fe2+(aq) + Hg2Cl2(s)

            Which one of the following pairs correctly indicates the oxidizing agent and the reducing agent in this reaction?

                Oxidizing agent   Reducing agent

            A)      Hg(l)             Fe3+(aq)                            D)      Fe3+(aq)             Hg(l)

            B)      Hg(l)             Cl(aq)                             E)      Cl(aq)             Fe3+(aq)

            C)      Fe3+(aq)             Cl(aq)                                 

 

      35.  Consider the following reaction:

            2Fe3+(aq) + 2Hg(l) + 2Cl(aq) ® 2Fe2+(aq) + Hg2Cl2(s)

            In this reaction,

            A)      Fe3+(aq) is the reducing agent.              D)      Hg(l) is reduced.

            B)      Fe3+(aq) loses electrons.                        E)      Hg(l) is the oxidizing agent.

            C)      Hg(l) loses electrons.                                      

      36.  Consider the reaction:

            H2O(l) + 3SO32-(aq) + 2MnO4-(aq) ® 3SO42-(aq) + 2MnO2(s) + 2OH-(aq)

            Which species is oxidized?

            A)  H2O    B)  SO32-    C)  MnO4-    D)  SO42-    E)  MnO2

 

      37.  Examine the following reaction:

            5FeCl2(aq) + KMnO4(aq) + 8HCl(aq) ® 5FeCl3(aq) + MnCl2(aq) + KCl(aq) + 4H2O(l)

            Which element has undergone oxidation?

            A)  Fe    B)  H    C)  Cl    D)  O    E)  Mn

 

      38.  Examine the following reaction:

            5FeCl2(aq) + KMnO4(aq) + 8HCl(aq) ® 5FeCl3(aq) + MnCl2(aq) + KCl(aq) + 4H2O(l)

            Which element has undergone reduction?

            A)  Fe    B)  H    C)  Cl    D)  O    E)  Mn

 

      39.  Consider the reaction:

            H2O(l) + 3SO32-(aq) + 2MnO4-(aq) ® 3SO42-(aq) + 2MnO2(s) + 2OH-(aq)

            Which species is reduced?

            A)  H2O    B)  SO32-    C)  MnO4-    D)  SO42-    E)  MnO2

 

      40.  Consider the reaction:

            H2O(l) + 3SO32-(aq) + 2MnO4-(aq) ® 3SO42-(aq) + 2MnO2(s) + 2OH-(aq)

            Which species is the reducing agent?

            A)  H2O    B)  SO32-    C)  MnO4-    D)  SO42-    E)  MnO2

 

      41.  Consider the reaction:

            Cu(s) + 4HNO3(aq) ® Cu(NO3)2(aq) + 2NO2(g) + 2OH-(aq)

            Which species is oxidized?

            A)  OH-    B)  NO2    C)  Cu(NO3)2    D)  HNO3    E)  Cu

 

      42.  Consider the reaction:

            Cu(s) + 4HNO3(aq) ® Cu(NO3)2(aq) + 2NO2(g) + 2OH-(aq)

            Which species is the reducing agent?

            A)  OH-    B)  NO2    C)  Cu(NO3)2    D)  HNO3    E)  Cu

      43.  Consider the reaction:

            Cu(s) + 4HNO3(aq) ® Cu(NO3)2(aq) + 2NO2(g) + 2OH-(aq)

            Which species is the oxidizing agent?

            A)  OH-    B)  NO2    C)  Cu(NO3)2    D)  HNO3    E)  Cu

      44.  For the following reaction, what is the oxidizing agent?

            2Cl2(g) + C(s) + 2H2O(l) ® CO2(g) + 4HCl(aq)

            A)  Cl2    B)  C    C)  H2O    D)  CO2    E)  HCl

 

      45.  Consider the reaction:

            Zn(s) + H2SO4(aq) ® ZnSO4(aq) + H2(g)

             Which species is oxidized, and how many electrons are transferred per atom of zinc that reacts?

            A)      Zn, 2 electrons                                       D)      Zn2+, 4 electrons

            B)      H+, 2 electrons                                       E)      H2, 2 electrons

            C)      SO42-, 4 electrons                                           

 

      46.  Consider the reaction:

            Zn(s) + H2SO4(aq) ® ZnSO4(aq) + H2(g)

            Which species is reduced, and how many electrons are transferred per atom of zinc that reacts?

            A)      Zn, 2 electrons                                       D)      Zn2+, 4 electrons

            B)      H+, 2 electrons                                       E)      H2, 2 electrons

            C)      SO42-, 4 electrons                                           

 

      47.  Consider the reaction:

            Zn(s) + H2SO4(aq) ® ZnSO4(aq) + H2(g)

            Which species is the reducing agent, and how many electrons are transferred per atom of zinc that reacts?

            A)      Zn, 2 electrons                                       D)      Zn2+, 4 electrons

            B)      H+, 2 electrons                                       E)      H2, 2 electrons

            C)      SO42-, 4 electrons                                           

 

      48.  Consider the reaction:

            Sn2+(aq) + 2Fe3+(aq) ® Sn4+(aq) + 2Fe2+(aq)

            Which species is reduced, and how many electrons are transferred per Sn2+ ion that reacts?

            A)      Sn2+, 2 electrons                                    D)      Fe2+, 4 electrons

            B)      Fe3+, 2 electrons                                    E)      Fe2+, 2 electrons

            C)      Sn4+, 4 electrons                                             

 

      49.  Consider the reaction:

            Sn2+(aq) + 2Fe3+(aq) ® Sn4+(aq) + 2Fe2+(aq)

            Which species is oxidized, and how many electrons are transferred per Sn2+ ion that reacts?

            A)      Sn2+, 2 electrons                                    D)      Fe2+, 4 electrons

            B)      Fe3+, 2 electrons                                    E)      Fe2+, 2 electrons

            C)      Sn4+, 4 electrons                                             

 

      50.  Consider the reaction:

            Sn2+(aq) + 2Fe3+(aq) ® Sn4+(aq) + 2Fe2+(aq)

            Which species is the oxidizing agent, and how many electrons are transferred per Sn2+ ion that reacts?

            A)      Sn2+, 2 electrons                                    D)      Fe2+, 4 electrons

            B)      Fe3+, 2 electrons                                    E)      Fe2+, 2 electrons

            C)      Sn4+, 4 electrons                                             

 

      51.  In a voltaic cell, the electron flow is always from

            A)      the salt bridge to the cathode.

            B)      the salt bridge to the anode.

            C)      the oxidizing agent through the salt bridge to the reducing agent.

            D)      the reducing agent through the salt bridge to the oxidizing agent.

            E)      the anode to the cathode.

      52.  Consider a voltaic cell that corresponds to the following reaction:

            Fe(s) + Ni2+(aq) ® Fe2+(aq) + Ni(s)

            Which of the following statements is correct?

            A)      Iron is the oxidizing agent.

            B)      The Ni2+ solution must be in the half-cell with the iron electrode.

            C)      No salt bridge is necessary, since the charge is 2+ on both sides of the equation.

            D)      The nickel electrode is the cathode.

            E)      Four electrons will be transferred per atom of iron that reacts.

 

      53.  Consider a voltaic cell that corresponds to the following reaction:

            Mg(s) + Sn2+(aq) ® Mg2+(aq) + Sn(s)

            Which of the following statements is correct?

            A)      Magnesium is the oxidizing agent.

            B)      The Sn2+ solution must be in the half-cell with the magnesium electrode.

            C)      No salt bridge is necessary, since the charge is 2+ on both sides of the equation.

            D)      The tin electrode is the cathode.

            E)      Four electrons will be transferred per atom of magnesium that reacts.

 

      54.  Consider a voltaic cell that corresponds to the following reaction:

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

            Which of the following statements is correct?

            A)      Zinc is the oxidizing agent.

            B)      The Cu2+ solution must be in the half-cell with the zinc electrode.

            C)      No salt bridge is necessary, since the charge is 2+ on both sides of the equation.

            D)      The zinc electrode is the cathode.

            E)      Two electrons will be transferred in this reaction per atom of zinc that reacts.

      55.  Consider a voltaic cell that corresponds to the following reaction:

            Cu(s) + 2Ag+(aq) ® Cu2+(aq) + Ag(s)

            Which of the following statements is correct?

            A)      Copper is the reducing agent.

            B)      The Cu2+ solution must be in the half-cell with the silver electrode.

            C)      No salt bridge is necessary, since the charge is 2+ on both sides of the equation.

            D)      The copper electrode is the cathode.

            E)      Four electrons will be transferred in this reaction per atom of copper that reacts.

 

      56.  Given the following reaction in a voltaic cell:

            Cu(s) + 2Ag+(aq) ® 2Ag(s) + Cu2+(aq)

            Which of the following statements is correct?

            A)      Cu(s) is the anode.

            B)      Oxidation occurs at the silver electrode.

            C)      There is no cathode for this cell.

            D)      Ag(s) is the anode.

            E)      One mole of electrons is transferred in the reaction as written.

 

      57.  In a fuel cell that uses gaseous hydrogen and oxygen as reactants, which one of the following reactions is occurring at the anode?

            A)      2H2O ® 2H2 + O2                                D)      O2 + 4e ® 2O2–

            B)      H2 ® 2H+ + 2e                                    E)      2O2– ® O2 + 4e

            C)      2H+ + 2e ® H2                                             

 

      58.  Consider a voltaic cell that corresponds to the following reaction:

            Cu(s) + 2Ag+(aq) ® Cu2+(aq) + Ag(s)

            If this reaction takes place in the electrochemical cell shown in the figure, which of the following statements is incorrect?

           

 

            A)      I is the copper electrode, which is the anode.

            B)      II is the Ag+ solution.

            C)      III is the salt bridge.

            D)      V contains the substance that is being reduced.

            E)      V is the silver electrode, which is the cathode.

          

 

      59.  Consider a voltaic cell that corresponds to the following reaction:

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

            If this reaction takes place in the electrochemical cell shown in the figure, which of the following statements is incorrect?

           

 

            A)      I is the zinc electrode, which is the anode.

            B)      II is the Cu2+ solution.

            C)      III is the salt bridge.

            D)      IV contains the substance that is being reduced.

            E)      V is the copper electrode, which is the cathode.

          

 

      60.  Consider a voltaic cell that corresponds to the following reaction:

            Mg(s) + Sn2+(aq) ® Mg2+(aq) + Sn(s)

            If this reaction takes place in the electrochemical cell shown in the figure, which of the following statements is incorrect?

           

 

            A)      I is the magnesium electrode, which is the anode.

            B)      II is the Mg2+ solution.

            C)      III is the salt bridge.

            D)      IV contains the substance that is being oxidized.

            E)      V is the tin electrode, which is the cathode.

 

 

      61.  The figure shows a molecular-level representation of the following voltaic cell:

            Fe(s) + Ni2+(aq) ® Fe2+(aq) + Ni(s)

            When drawing the “after” representation one would note that:

           

 

            A)      the nickel electrode will be smaller.

            B)      the iron electrode will be larger.

            C)      the number of Ni2+ ions in solution will decrease.

            D)      deposits will form in the salt bridge.

            E)      the number of Fe2+ ions in solution will remain constant.

 

 

      62.  The figure shows a molecular-level representation of the following voltaic cell:

            Mg(s) + Sn2+(aq) ® Mg2+(aq) + Sn(s)

            When drawing the “after” representation one would note that:

           

 

            A)      the tin electrode will be smaller.

            B)      the magnesium electrode will be larger.

            C)      the number of Mg2+ ions in solution will remain constant.

            D)      deposits will form in the salt bridge.

            E)      the number of Sn2+ ions in solution will decrease.

 

 

      63.  Given the following reaction in a voltaic cell:

            Zn(s) + Ni2+(aq) ® Ni(s) + Zn2+(aq)

            In this cell, Zn(s) is called the

            A)  anode.    B)  oxidizing agent.    C)  salt bridge.    D)  electrolyte.    E)  cathode.

 

      64.  The reaction that occurs in an alkaline battery is as follows:

            Zn(s) + MnO2(s) + H2O(l) ® ZnO(s) + Mn(OH)2(s)

            The substance that is oxidized in this battery is:

            A)  Zn    B)  ZnO    C)  MnO2    D)  H2O    E)  Mn(OH)2

 

      65.  The reaction that occurs in an alkaline battery is as follows:

            Zn(s) + MnO2(s) + H2O(l) ® ZnO(s) + Mn(OH)2(s)

            The substance that is reduced in this battery is:

            A)  Zn    B)  ZnO    C)  MnO2    D)  H2O    E)  Mn(OH)2

 

      66.  The reaction that occurs in an alkaline battery is as follows:

            Zn(s) + MnO2(s) + H2O(l) ® ZnO(s) + Mn(OH)2(s)

            The substance that is the reducing agent in this battery is:

            A)  Zn    B)  ZnO    C)  MnO2    D)  H2O    E)  Mn(OH)2

 

      67.  A mercury button battery that is used in watches and calculators is powered by the following reaction:

            Zn(s) + HgO(s) ® ZnO(s) + Hg(s)

            The substance that is oxidized in this battery is:

            A)  HgO    B)  Hg    C)  ZnO    D)  Zn

 

      68.  A lead-acid battery that is used in cars and trucks is powered by the reaction:

            PbO2(s) + Pb(s) + 2H2SO4(aq) ® 2PbSO4(s) + H2O(l)

            The substance that is the reducing agent in this battery is:

            A)  PbSO4    B)  H2O    C)  PbO2    D)  Pb    E)  H2SO4

 

      69.  A lead-acid battery that is used in cars and trucks is powered by the reaction:

            PbO2(s) + Pb(s) + 2H2SO4(aq) ® 2PbSO4(s) + H2O(l)

            The substance that is the oxidizing agent in this battery is:

            A)  PbSO4    B)  H2O    C)  PbO2    D)  Pb    E)  H2SO4

      70.  A lead-acid battery that is used in cars and trucks is powered by the reaction:

            PbO2(s) + Pb(s) + 2H2SO4(aq) ® 2PbSO4(s) + H2O(l)

            The substance that is reduced in this battery is:

            A)  PbSO4    B)  H2O    C)  PbO2    D)  Pb    E)  H2SO4

 

      71.  The following reaction occurs in a lead storage battery:

            PbO2(s) + Pb(s) + H2SO4(aq)

 2PbSO4(s) + 2H2O(l)

 

            What happens to the sulfuric acid in a lead storage battery when the battery is being discharged?

            A)      Sulfate ions are consumed and their concentration decreases.

            B)      Protons are released so the pH drops.

            C)      The solution gets increasingly more viscous due to an increase in sulfuric acid concentration.

            D)      Its concentration increases.

            E)      All of these are correct.

 

      72.  The following reaction occurs in a lead storage battery:

            PbO2(s) + Pb(s) + H2SO4(aq)

 2PbSO4(s) + 2H2O(l)

 

            Which statement is true?

            A)      The concentration of H2SO4 increases as the battery discharges.

            B)      Pb is formed at the anode during charging.

            C)      PbO2 is formed at the anode during charging.

            D)      The mass of Pb decreases during charging.

            E)      The mass of PbSO4 remains constant during charging and discharging.

 

      73.  Consider the skeletal equation:

            Sn2+(aq) + Fe3+(aq) ® Sn4+(aq) + Fe2+(aq)

            When balanced, the equation will be:

            A)      Sn2+(aq) + Fe3+(aq) ® Sn4+(aq) + Fe2+(aq)

            B)      2Sn2+(aq) + Fe3+(aq) ® Sn4+(aq) + Fe2+(aq)

            C)      2Sn2+(aq) + Fe3+(aq) ® 2Sn4+(aq) + Fe2+(aq)

            D)      Sn2+(aq) + 2Fe3+(aq) ® Sn4+(aq) + 2Fe2+(aq)

            E)      4Sn2+(aq) + Fe3+(aq) ® 2Sn4+(aq) + Fe2+(aq)

 

      74.  A voltaic cell is prepared in which copper metal is oxidized to Cu(II), and silver ion is reduced to silver metal.  Which of the following represents the correctly balanced equation for this reaction?

            A)      Cu(s) + Ag+(aq) ® Cu2+(aq) + Ag(s)

            B)      2Cu(s) + Ag+(aq) ® 2Cu2+(aq) + Ag(s)

            C)      Cu(s) + 2Ag+(aq) ® Cu2+(aq) + 2Ag(s)

            D)      3Cu(s) + 2Ag+(aq) ® 3Cu2+(aq) + 2Ag(s)

            E)      2Cu(s) + 3Ag+(aq) ® 2Cu2+(aq) + 3Ag(s)

 

      75.  A voltaic cell is prepared in which copper metal is oxidized to Cu(II), and silver ion is reduced to silver metal.  Which of the following represents the equation for the reaction that occurs at the anode?

            A)      Cu(s) – 2e ® Cu2+(aq)                         D)      Ag+(aq) + e ®  Ag(s)

            B)      Cu(s) ® Cu2+(aq) + 2e                        E)      Ag(s) ® Ag+(aq) + e

            C)      2Cu(s) ® 2Cu2+(aq) + e                               

          

 

      76.  A voltaic cell is prepared in which aluminum metal is oxidized to Al3+, and nickel(II) is reduced to nickel metal.  Which of the following represents the correctly balanced equation for this reaction?

            A)      Al(s) + Ni2+(aq) ® Al3+(aq) + Ni(s)

            B)      Al(s) + 2Ni2+(aq) ® Al3+(aq) + 2Ni(s)

            C)      2Al(s) + 3Ni2+(aq) ® 2Al3+(aq) + 3Ni(s)

            D)      Al3+(aq) + 2Ni(s) ® Al(s) + 2Ni2+(aq)

            E)      2Al3+(aq) + 3Ni(s) ® 2Al(s) + 3Ni2+(aq)

 

      77.  If the following equation is properly balanced with the smallest whole-number coefficients, what is the coefficient of Bi3+?

            Mn2+(aq) + BiO3(aq) ® MnO4(aq) + Bi3+(aq)

            A)  1    B)  2    C)  3    D)  4    E)  5

 

 

      78.  The following reaction occurs in acid solution.  When the equation is properly balanced with the smallest whole-number coefficients, what is the coefficient of MnO4?

            MnO4(aq) + I(aq) ® Mn2+(aq) + I2(aq)

            A)  1    B)  2    C)  3    D)  4    E)  5

          

 

      79.  A voltaic cell is prepared in which aluminum metal is oxidized to Al3+, and nickel(II) is reduced to nickel metal.  Which of the following represents the equation for the reaction that occurs at the anode?

            A)      Al(s) ® Al3+(aq) + 3e                          D)      Al3+(aq) + 3e ® Al(s)

            B)      Ni2+(aq) + 2e ® Ni(s)                          E)      2Al3+(aq) + 3e ® 2Al(s)

            C)      Ni(s) ® Ni2+(aq) + 2e                                   

 

      80.  Consider the half-reaction Cr3+(aq) ® Cr2O72-(aq).  When the equation is balanced in acid solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

            A)  3, 3    B)  6, 6    C)  7, 6    D)  5, 4    E)  3, 6

 

      81.  Consider the half-reaction NH4+(aq) ® NO3-(aq).  When the equation is balanced in acid solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

            A)  3, 3    B)  2, 6    C)  7, 6    D)  4, 4    E)  3, 8

 

 

      82.  Consider the half-reaction NO3-(aq) ® NO(aq).  When the equation is balanced in acid solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

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

 

      83.  Consider the half-reaction ClO- (aq) ® Cl-(aq).  When the equation is balanced in basic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

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

 

      84.  Consider the half-reaction O2(aq) ® OH-(aq).  When the equation is balanced in basic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

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

 

      85.  Consider the reaction:

            H3AsO3(aq) + BiO3-(aq) ® H3AsO4(aq) + Bi(s)

            When this equation is balanced in acidic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

            A)  2, 6    B)  2, 1    C)  1, 10    D)  1, 2    E)  2, 3

 

      86.  Consider the reaction:

            CrO42-(aq) + HSO3-(aq) ® Cr3+(aq) + SO42-(aq)

            When this equation is balanced in acidic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

            A)  3, 3    B)  2, 1    C)  2, 4    D)  5, 6    E)  2, 3

 

      87.  Consider the reaction:

            Zn(s) + NO3-(aq) ® NH3(aq) + Zn(OH)42-(aq)

            When this equation is balanced in basic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

            A)  3, 3    B)  2, 1    C)  6, 8    D)  5, 6    E)  2, 3

 

      88.  Consider the reaction:

            Al(s) + H2O(l) ® Al(OH)4-(aq) + H2(g)

            When this equation is balanced in basic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

            A)  3, 3    B)  2, 1    C)  6, 8    D)  6, 6    E)  2, 3

 

      89.  Given the following information about the activity series, predict whether the given reaction will occur or not.  If it does occur, write a balanced equation.

            Cu < H2 < Sn < Fe < Zn < Mg

            Mg(s) + HCl(aq) ®

            A)      No reaction will occur.

            B)      Mg(s) + HCl(aq) ® MgH(aq) + Cl(aq)

            C)      Mg(s) + HCl(aq) ® MgCl(aq)  + H(aq)

            D)      Mg(s) + 2HCl(aq) ® MgCl2(aq)  + H2(g)

            E)      Mg(s) + 2HCl(aq) ® MgH2(aq)  + Cl2(g)

 

      90.  Given the following information about the activity series, predict whether the given reaction will occur or not.  If it does occur, write a balanced equation.

            Cu < H2 < Sn < Fe < Zn < Mg

            Mg(s) + ZnCl2(aq) ®

            A)      No reaction will occur.

            B)      Mg(s) + ZnCl2(aq) ® MgCl(aq) + ZnCl(aq)

            C)      Mg(s) + ZnCl2(aq) ® MgCl2(aq) + Zn(s)

            D)      Mg(s) + ZnCl2(aq) ® MgZn(s) + Cl2(g)

            E)      Mg(s) + ZnCl2(aq) ® MgCl2(aq) + Zn(aq)

 

      91.  Given the following information about the activity series, predict whether the given reaction will occur or not.  If it does occur, write a balanced equation.

            Cu < H2 < Sn < Fe < Zn < Mg

            Fe(s) + SnCl2(aq) ®

            A)      No reaction will occur.

            B)      Fe(s) + SnCl2(aq) ® FeCl(aq) + SnCl(aq)

            C)      Fe(s) + SnCl2(aq) ® FeCl2(aq) + Sn(s)

            D)      Fe(s) + SnCl2(aq) ® FeZn(s) + Cl2(g)

            E)      Fe(s) + SnCl2(aq) ® FeCl2(aq) + Sn(aq)

      92.  Given the following information about the activity series, predict whether the given reaction will occur or not.  If it does occur, write a balanced equation.

            Cu < H2 < Sn < Fe < Zn < Mg

            Cu(s) + SnCl2(aq) ®

            A)      No reaction will occur.

            B)      Cu(s) + SnCl2(aq) ® CuCl(aq) + SnCl(aq)

            C)      Cu(s) + SnCl2(aq) ® CuCl2(aq) + Sn(s)

            D)      Cu(s) + SnCl2(aq) ® CuZn(s) + Cl2(g)

            E)      Cu(s) + SnCl2(aq) ® CuCl2(aq) + Sn(aq)

 

      93.  In any electrolytic cell, the cathode is the electrode

            A)      that attracts anions.

            B)      at which electrons are collected from electron donors in the solution.

            C)      at which reduction occurs.

            D)      at which oxidation occurs.

            E)      that is made of graphite.

 

      94.  The figure shows the electrolysis of molten NaI.  What reaction occurs at the anode of this cell?

           

 

            A)      NaI(l) ® NaI2(l)                                    D)      2I-(l) + e ® I2(g)

            B)      I-(l) + e ® I2-                                      E)      2I-(l) ® I2(g) + 2e

            C)      Na+(l) + e ® Na(l)                                        

 

 

      95.  The figure shows the electrolysis of molten NaI.  What reaction occurs at the cathode of this cell?

           

 

            A)      NaI(l) ® NaI2(l)                                    D)      2I-(l) + e ® I2(g)

            B)      I-(l) + e ® I2-                                      E)      2I-(l) ® I2(g) + 2e

            C)      Na+(l) + e ® Na(l)                                        

 

      96.  The figure shows the electrolysis of molten AlCl3.  What reaction occurs at the cathode of this cell?

           

 

            A)      AlCl3(l) ® AlCl2(l)                               D)      2Cl-(l) + 2e ® Cl2(g)

            B)      Cl-(l) + e ® Cl2-                                  E)      2Cl-(l) ® Cl2(g) + 2e

            C)      Al3+(l) + 3e ® Al(l)                                      

      97.  The figure shows the electrolysis of molten AlCl3.  What reaction occurs at the anode of this cell?

           

 

            A)      AlCl3(l) ® AlCl2(l)                               D)      2Cl-(l) + 2e ® Cl2(g)

            B)      Cl-(l) + e ® Cl2-                                  E)      2Cl-(l) ® Cl2(g) + 2e

            C)      Al3+(l) + 3e ® Al(l)                                      

 

 

      98.  The products of the electrolysis of molten magnesium chloride are

            A)      H2(g) and O2(g)                                     D)      H2(g) and Cl2(g)

            B)      Mg(l) and OH(aq)                                E)      Mg(l) and O2(g)

            C)      Mg(l) and Cl2(g)                                             

           

 

      99.  Sodium is produced by electrolysis of molten sodium chloride.  What are the products at the anode and cathode, respectively?

            A)      Cl(aq) and Na2O(l)                              D)      Cl2(g) and Na2O(l)

            B)      Cl2(g) and Na(l)                                     E)      O2(g) and Na(l)

            C)      Na(l) and O2(g)                                              

          

 

    100.  The products of the electrolysis of molten calcium chloride are

            A)      H2(g) and O2(g)                                     D)      CaO(s) and HCl(g)

            B)      CaCl(l) and Cl(g)                                  E)      Ca(l) and O2(g)

            C)      Ca(l) and Cl2(g)                                              

           

 

    101.  Given the following information about the activity series, select element(s) that could be used to protect the iron in a steel ship's hull from corrosion.

            Cu < H2 < Sn < Fe < Zn < Mg

            A)  Cu or Sn    B)  Cu, H2, or Sn    C)  Cu only    D)  Mg only    E)  Zn or Mg

 

 

    102.  Given the following information about the activity series, select element(s) that could be used to protect the iron in a steel evaporative (swamp) cooler from corrosion.

            Cu < H2 < Sn < Fe < Zn < Mg

            A)  Cu or Sn    B)  Cu, H2, or Sn    C)  Cu only    D)  Mg only    E)  Zn or Mg

 

 

    103.  An electrolytic cell is an electrochemical cell in which an oxidation-reduction reaction causes electrons to flow through an external circuit.

           

 

    104.  The cathode is the electrode at which oxidation occurs.

           

 

    105.  Reduction is a chemical process in which an atom's oxidation number decreases.

           

 

    106.  A species that causes a decrease in the oxidation number of another substance is called a reducing agent.

           

 

    107.  The chemical reactions that occur in voltaic (galvanic) cells are nonspontaneous, and require an outside electrical current to power the reaction.

           

 

    108.  Batteries are electrochemical cells that are constructed so that a barrier separates the oxidation reaction from the reduction reaction.

           

 

    109.  The potential of a voltaic cell is greatest in cells constructed of strong oxidizing and reducing agents.

           

 

    110.  Equations that are written to represent either an oxidation reaction or a reduction reaction are called half-reactions.

           

 

    111.  The salt bridge in an electrochemical cell provides cations to the half-cell in which oxidation occurs.

           

 

    112.  The balanced half-reaction for the oxidation of nickel to nickel(II) is

             Ni(s) ® Ni2+(aq) + 2e.

           

 

    113.  An electrolytic cell produces electrical energy.

           

 

    114.  A steel utility pole (made primarily of iron) can be protected from oxidation by attaching a piece of copper, or some other relatively inactive metal, to it.

           

 

    115.  List the oxidation number of sulfur in H2S.

 

    116.  List the oxidation number of sulfur in H2SO4.

    117.  List the oxidation number of sulfur in H2SO3.

 

    118.  The copper ore chalcocite, Cu2S, reacts with oxygen in a process called “roasting” to produce copper metal.  The equation for the reaction is:

            Cu2S(s) + O2(g) ® 2Cu(s) + SO2(g)

            Identify the atoms that are oxidized and reduced, and the oxidizing and reducing agents.

 

    119.  Write and balance the equation for the reaction between aluminum metal and Ni(II) ion to produce Al3+ and nickel metal.  Show both of the half-reactions and the number of electrons transferred.

 

    120.  Given the following information about the activity series, Cu < H2 < Sn < Fe < Zn < Mn, predict whether the following reaction will occur or not.  If yes, write a balanced equation.

            Mn(s) + HCl(aq) ®

 

 

    121.  Given the following information about the activity series, Cu < H2 < Sn < Fe < Zn < Mn, predict whether the following reaction will occur or not.  If yes, write a balanced equation.

            Fe(s) + SnCl2(aq) ®

 

    122.  The figure shows the electrolysis of molten AlCl3.  Write the reactions that occur at the anode and the cathode of this cell.

           

 

 

    123.  If two metals are in contact with each other in a moist environment, one of the metals will begin to corrode.  Why is this true?

 

Option 1

Low Cost Option
Download this past answer in few clicks

16.87 USD

PURCHASE SOLUTION

Already member?


Option 2

Custom new solution created by our subject matter experts

GET A QUOTE

rated 5 stars

Purchased 7 times

Completion Status 100%

Sitejabber (5.0)

BBC (5.0)

Trustpilot (4.8)

Google (5.0)

Related Questions