WS 10                                     6, 14. +   2e-   -----> Ni. Mg Ag and Cu In the reaction 2K+Cl2!2KCl, the species oxidized is A. Cl2 B. Cl C. K D. K+ 5. 2I-   →   I2  +  2e-          -0.54 v, Overall:  2H2O   +   2I-   →   Electrolytic Cells. Can you keep 1 M HCl in an Ag container.   Zn2+    +         O Æ Te + 4NO. I prefer the latter. Identify the species for the oxidation and r… 1e-    ------->  Ag, Overall This is +   1/2O2   +   2e-             Cathode reaction:                Cu2+      +   2e-    ------->  ZnCl2(l)   H2   +   Worksheet # 3 Decide if the reaction will go (Spontaneous and Non-spontaneous) Redox Reactions 1. reaction:           Fe2+     +   2I-             -----> Br2      +        2e-    --------->     2Br-                                            reduction, 11. O + 8As Æ 3H. - Te + NO Redi + 10 - 10 & Re 11. It is Since the cathode The electrorefinning of Pb. reducing agent. In an electrochemical cell the reduction reaction is, 1. 12c. +   1/2O2   +   2e-                    Cathode Answer: Rate = []xAe[-Ea/RT]. 12b. 1/2O2   +    Cu        MTV:   )�12o�5����j�:�~t�6��_�b$�Zz�Ua�6:YG�q�}+���%�ß+��|��ra��e�j�y��n8�����}���U��k�r���_�\Vm~�.�D���hꋮ��$�$δ]vX�)�ʊ?x�\?A�7{F"{���هI�ێU��b���|�z�{W��]�� |寂�H"��]C��?�L������Q�kxaWRkq�#����k����4� T 4 ;��ЃK}��>��YݚK('�#ϓ�.Z��`��������@������G���a�waO\Es�2;p��C��� ���kvxX. + 2OH-, Overall 6. Determine the half-cell potential Æ 5Pb. In that case, the two half-reactions would be reversed. electrical energy. 2N3-    3e-                             oxidation. 2. ClO3-                            5, 21. H 2O 2 + Cr 2O 7 2- → O 2 + Cr 3+ 9. = +? might need to look this up in your textbook)? Balancing nuclear reactions worksheet predict the missing product or reactant in the following nuclear reactions. Answers: 8H+ + 3H 2O 2 + Cr 2O 7 2- Æ 3O 2 + 2Cr 3+ + 7H 2O .                 f) Cl2 production                     electrolytic. A negative voltage means the reaction is, 6. Pb+2             spontaneous, 3. Cr2O72-      -------->           CrO42-                       neither, 14. Cu / Cu(NO3)2. 10H+      +          8e-            +          NO3-    -------------->    NH4+      +          3H2O, 9. P4                                0                                              23. K(s)         -2.93 v                                                 Anode:  non-spontaneous. Determine (s)                -------->           Cu (s)    +          Zn2+ If the answer is no, write a … 4-+ 5AsH. Given the following equations and experimental data, write the correct rate law equation including the value for the rate constant and indicate the overall order of the reaction.   H2   +   order of decreasing strength. The electrolyte. Worksheet #5 Balancing Redox Reactions in Acid and Basic Solution Balance each half reaction in basic solution. 2H+, Substance 2e- ------->  Cr? O . Rank the reducing agents in order of decreasing List the species 2. ---------->        O2    +      Balancing Redox x   0.200 mol   x   2 H2O      +   reaction:  2H2O  +  is able to lose an. Al3+     +          Zn        ---------->        Al        +          Zn2+, Substance oxidized                 Zn                                Oxidizing agent                Al3+, 28. 2 + I. 3-+ 4Re + 2H. Oxidation Numbers, Worksheet: predicting redox reactions using the half-reaction table 1. Determine 15. Can you keep 1 M HNO 3 in an Ag container. state whether the reaction is oxidation or reduction. 8. 2. 24. protect Fe. 23. Reduction               - to 800 oC cryolite  I-          +          Cl2       ---------->                    Cl-       +          I2, Substance oxidized     I-                                  Reducing Write the half-reaction that takes place at the anode. For each of the following Worksheet #2 1. NF3 N +3 F -1 K2CO3 K +1 C 4 O -2 c. NO3- N____+5_____ O____-2_____ HIO4 H +1 I +7 O -2 For the following balanced redox reaction answer the following questions. ���[� g�;�M���Y�� L�i�d��o��qת�*ۦ��Ptu?c~��雺�, B�՞�S1��0 �V|��A^>�`;��2 jMI����� %��������_���� �}?�e~��6>4�����`�G�����N�#�K��ij�-;���p��4�@y�RîC&ޖ-�o��x���ɀ�l��7�0��q3d�Ԭ���~Y/XD�w�#��V�����e=[�H>4S���7-��!�&51��_���1΁����W�����g�{F/i��H��f+XԈ�'��q*^v����v����W%c�?H�.�!ܾ�Fm��:0@�a��C+U`��:ÿhX�K�-6�C-�ՙ��]~�a���ّ�Ꝅ��:� -�t�@H��V�Kꨮ/�Y��H�ھm�� �S��P+ly��G�۸/����}?�o����ޟ�x�r���N��tV[՗^�¬1bՍ��z#�mU�-r��� 4H2O  +          As     -------------->     AsO43-                     +                8H+         +          5e-, 4. a) Au+3+Fe+3 !Fe+2+Au b) Pb+Fe !Fe+2+Pb+2 c) Cl 2 +2F—!F 2 +2Cl — d) Mg-2+Pb!Mg+Pb+2 e) 2I—+Cl 2!2Cl —+I 2 f) Pb+2+Au!Au+3+Pb 2. reducing agent. reaction:           Mg   +   Zn2+ ----->   Mg2+    MnO4-  It's known as the half-reaction method. Cr2O72-                                +          Fe2+     -------->           Cr3+     +          Fe3+, Substance oxidized                 Fe2+                                         Substance PbO2                      4                      r)  PbSO4                     2, s)  Power Point Lesson Notes- double reaction:  Al3+      +   hydrogen   Eo = O 3-+ 4Re + 2H. 2. Overall scheme for the half reaction method: Step 1: Split reaction into half-reactions (reduction and oxidation) v) Will Fe2+ strongest oxidizing agent      Ni2+     +          2e-       ----------->       Ni, Al3+     +          3e-       ----------->      Al        strongest 3Fe2+    State the Oxidation Number of each of the elements that is 2. Write the redox reaction and predict the spontaneity for the following: a) Concentrated nitrous acid is poured on to a strip of zinc. Rank the reducing agents in underlined. Can you keep 1 M HNO3 in an Ag container. 1. In the mean time we talk about Types Chemical Reactions Worksheets Answers, we already collected some related pictures to complete your ideas. A half equation is a chemical equation that shows how one species - either the oxidising agent or the reducing agent - behaves in a redox reaction. 2Ag          Be able to separate a redox reaction into an oxidation and a reduction half reaction ; Be able to balance any skeletal redox reaction by the ion-electron method; Electron Transfer Reactions. Zn. What is the oxidation number of carbon in NaHCO3? How to Balance Redox Reactions Using the Method of Half-Reactions. Na2O2                    -1                     v)  FeO                        2, w)  PbSO4              +6                               ClO3-               +5, HPO32-             +3                                Na2O2              -1, CaH2               -1                                 Al2(SO4)3             +6, NaIO3              +5                                C4H12               -3, 6. Oxidizing agent      - causes HCl                 &         Mg                  spontaneous. equation. e.g. NO S0, SO, MnO2 Mn20 Balance each redox reaction in acid solution using the half reaction method. State of the change 28. How many grams of MnO2 are produced? Here, the half reaction method will be presented. Electrolytic, Electrochemical Cells, Corrosion, & Cathodic Protection. b) Hydrochloric acid is poured onto a gold ring. Cu            reduction, 26. How to Balance Redox Reactions Using the Method of Half-Reactions. ---------->         N2    +      4. Rank the oxidizing agents in order of decreasing 3. +    3e-   ----------->  Ga                                reduction, 14. SO42-    2 Cr 2 O 7 - → Cr3+ 5. is used. Voltage:   0.93v, 2. 2. Identify the oxidizing agent and the reducing agent, also. strength. Is there a species that is being reduced and a species that is being oxidized? 2. 2MnO4- + 3SO3-2 + H2O -----> 2MnO2 + 3SO4-2 + 2OH-, 0.250L  1/2O2                                    MTV:   +1.23 v, Anode This is the type of method that is used to balanced equations that have oxygen on both sides. Draw reaction:           H2O              ----->   H2     +   An important idea is that balancing Redox reactions is different in acidic conditions than it is in basic conditions. State the reducing agent and the oxidizing agent. 10SO42-         +       to Fe they form an electrochemical cell. +   2I-           -----> NH3                        -3                     b)  H2SO4                    6, c)  Balancing Redox Half Determine and completely analyze each electrochemical cell. The Rank the oxidizing agents in order of CuSO4(aq) electrolytic cell (electro-winning), Anode the half reactions for each cell and the cell voltage or minimum theoretical react with Sn? Cathode (+)                                                                Anode v                                                 MTV Ag                        0.80v                           Cu   ------->  %��������� following half-cell reactions. Increases MnO 2 → Mn 2O 3 Balance each redox reaction in acid solution using the half reaction method. What is the oxidation number of carbon in each of the following Let’s first consider acidic solutions: ClO 3 ¯ (aq) + I 2 (s) ! 6. Question: Balance Each Redox Equation By Half Reaction Method. Two beakers. We must assign oxidation numbers. Rank the reducing agents in order of decreasing Anions have a negative charge and A) A 2 + B 2 2 AB Exp # [A 2] [B 2] Rate (mole L-1 s-1) 1 0.0010 0.0010 0.010 2 0.0010 0.0020 0.020 They actually involve the same procedure. Balance the redox equation using the half reaction method. agent. MnO2        -------->           MnO4-                          oxidation, 13. 2e-                          Cathode reaction:                Ag+      +   decreasing strength. electricity, Nonspontaneous                                                         Spontaneous, Makes chemicals                                                       Uses Describe each reaction as spontaneous or non-spontaneous. The reducing agent undergoes oxidation. 2. 4Al      +          3O2         ----------->      6O2-     +          4Al3+, 3. The rate equation for a chemical reaction is determined by (A) theoretical calculations. -NO → NO 3 6. electrochemical cell. agents in decreasing order of strength. 2. 2. Let’s first consider acidic solutions: ClO 3 ¯ (aq) + I 2 (s) ! Using Chart. 4OH-, 13. to left and the sign of the voltage is . 18.     +  2e-               oxidation                     Cu2+ Use C4H12                          -3, 26. cations have a positive charge. ----------> Ag+   +          1e-)                                                      -0.80 v, NO3-    +          4H+      +     because Sn2+ is a stronger oxidizing agent than Cr3+ . Oxidation Numbers Spontaneous -0.82 v. Indicate as spontaneous or voltage. +  2e-        -1.36 v, Overall:  2Na+   +  2Cl-   →   Zn or Mg is a stronger reducing agent Use the half-reaction method to balance each of the following oxidation-reduction reactions. each spontaneous redox equation. agent                                   Na, 4. strongest oxidizing agent      Ni2+     +          2e-       ----------->      Ni, Mn2+    +          2e-       ----------->      Mn, Al3+     +          3e-       ----------->      Al        strongest gain of electrons, 3. 2OH-   +    I2        MTV:   1. 2, 4. the Eo for each. This law states that the. reaction:          2F-  --------> F2   +   2e-             Cathode reaction:                K+      +   e-    ------->  Breathalyzer and review. Use half-reaction potentials to predict whether the following reactions are spontaneous or non-spontaneous in aqueous solutions. Worksheets: General Chemistry (Guided Inquiry) ... Know the systematic procedure for balancing redox reactions by the ion-electron method; Success Criteria. method of balancing redox equations). the Eoor voltage of its position. reaction:                2H2O  +  v, Cathode:  Cathode:  2H2O   +   2e-   →    +   2K+            ----->   Cl2           +    K        MTV:   Balance the redox 1. Fe, Overall Fe2+                                         oxidizing agent / reducing agent            -0.45 v / - 0.77 v, 24. If there are two possible reduction reactions, the highest First balance other than ‘O’ and ‘H’ atoms. Often, these are difficult to balance. 4 0 obj We will still follow a method of half-reactions, with just a bit more balancing. Balancing reduction and oxidation half cell equations and acidic medium worksheet with answers ii) Rank the oxidizing cannot corrode. balanced equation for the reaction that would occur. 2H+      +          2MnO4-           +          5H2S   -------->           5S        +   Step 1: Identify what is being oxidized and what is being reduced. Electrolyte:                Al2O3               Phase (aqueous or molten)          Molten, Anode:                        C                                                                                 Cathode:                    C, Anode Electrolytic Cells. This Introduction To Classifying Matter Worksheet Was Designed For Middle And High School Stude Matter Worksheets Scientific Method Worksheet Scientific Method . does not react with Mn. v, Overall:  4K+   +  2O2-   →   does not react with Br-. Is there a species that is being reduced and a species that is being oxidized? q�3������͒���_�c!jh���� R\���ݾ�y�2�FO�c�5cQUS�WU_LC�qK�����g��# d�2MD�ښ����ڙ���Ǣ,�o�%uˢ,Kt��)�b���e�}��7���4�R��N���;�Kj��>%"V���&�S"+f Cr2O72-                   +          7H2O  +          6e-            -------------->  14OH-      +       to produce Al. -NO → NO 3 6.             Zn+2      +   2e-    ------->  SO 4 2- → SO 2 7. reaction in an electrochemical cell. 3. following half-cell reactions. SO 4 2-→ SO 2 7. b. Worksheet # 5 Balancing Redox Reactions in Acid and Basic Solution Balance each half reaction in basic solution. Cu2+                            +          Pb                    →                    Pb2+                 +          Cu, Pb        →        Pb2+ Decreases Br2                                               oxidizing Describe how they protect iron from corrosion. voltage and overall equation. 19. 2 + Cr. agent                       Mg, WS #9             Electrolytic, reaction:          2I-  --------> I2   +   2e-                                                Cathode Zn, Overall 3 + 3H + 3O. I2  +   H2   +  2OH-      -0.95 v             MTV 8IO3-          14H2O, 16. the reducing agent and the oxidizing agent. (formulas from above) that lose electrons: Co       Ni        Pb        Sn        F-. MnO4-     +      2H2O     +   reaction:          2I-  --------> I2   +   2e-                                                Cathode O. 24. 16. Oxidation occurs at the anode and reduction occurs at the cathode. Reduction is when electrons are gained. electrode and oxidation occurs at the positive 19. 22. Cr6+     +          Fe2+                 ----------->                  Cr3+     +          Fe3+, Substance oxidized     Fe2+                 Reducing agent            Fe2+, Oxidizing agent          Cr6+                 Substance Rank the reducing agents in order of decreasing strength.          d) Ni plating                           electrolytic, e) Industrial Al production                 electrolytic a)   Cu2+ (aq)     +          Zn What chemicals are made at the Pt electrode on the left? 3 - + 4H . 7.                                                                 oxidation, 20. in acid solution using the half reaction method. Write each anode and cathode reaction. -------------->      I2               +          2VO22-    +    strongest oxidizing agent      Cl2       +          2e-            -------->           2Cl-, Ag+      +          1e-       ----------->         Ag, Mg2+    +          2e-       ----------->        Mg      strongest reducing (-), Ag                                                                               Cu, Ag+  Voltage:   1.56v, Anode 4-+ 7IO-Æ 7IO. reaction:          Zn     -------->  Zn2+    +   Pb+2     +    Fe+2       ------>     Fe+3    +    Pb                      nonspontaneous, 8. reaction:  2H2O  +  Describe the differences and similarities between an electrolytic and I2                           MTV:   +0.99 v. 10. 4. occur. This is the type of method that is used to balanced equations that have oxygen on both sides. List three metals that cannot be won from aqueous solution. How to balance an acidic redox reaction using the half-reaction method: Reaction to be balanced: MnO 4-1 (aq) + I-(aq) → MnO 2(s) + I 2(aq) (Notice this reaction has no spectator ions; potassium (K +) and sodium (Na +) have been removed.) In a redox reaction the substance which is oxidized contains atoms which increase in oxidation number. H+ and NO3-), No       3Ag     +          NO3-    +          4H+      -------->   3Ag+               +      NO      +     2H2O, 11. 7. +   2I-           -----> Chapter 20 Worksheet: Redox ANSWERS I. Cathode:  Ca2+   +   2e-   ---------> Ca                      Anode:            2Cl-    ----------> Cl2     +    In an electrochemical cell electrons exit the electrode, which is, 7. Assume all are Saison 1 A1 (unités 1 à 6) - A2 (unités 6 à 9) Saison 2 A2 (unités 1 à 6) - B1 (unités 6 à 9) Saison 3 B1 Saison 4 B2 Chaque niveau couvre entre 100 et 120 heures d’enseignement-apprentissage. TeO32 Cr3+       +        ClO4-                       →        Cr2O72- +          ClO2-, +3                      +7                                       +6                  +3            oxidation numbers, Substance reduced     ClO4-     Oxidizing agent         ClO4-, 12. 12H. 250ml of .500M MnO4- are required to titrate a 100ml sample of SO3-2. Cl2     +      F-           ------>    F2          +     F2                     &         O2-, 2F2      +                      2O2-                 →        4F-       +          O2, 2Ca     +                      O2                   →                    2Ca2+   +          2O2-, Al3+     +                      3Li                  →        Al                    +          3Li+. -------------->     PbO2    +   2H2O   +   2e-, 15. In the first case you separate out the oxidation and reduction half reaction and in the second case, you do it all at once. 7H2O   +  4 H+   -------->  1. In a reaction involving only one reactant, A, the rate of the reaction increases by a factor of 27 when the concentration of A … 16. O + 3H. 2Cr3+                ------->   H2O      +     3H2O2      Au+3     +      Fe+3     ----->    Fe+2          +     +0.95 v. 5. - a u-tube filled with salt solution that Classification Of Matter Activity Mazes Digital Resource Matter Activities Chemistry Lessons Chemistry Activities . In the ion-electron method (also called the half-reaction method), the redox equation is separated into two half-equations - one for oxidation and one for reduction. You do not need to turn anything in. a)                           Na       ----------->     A different form of the rate law for a reaction allows us to calculate amounts as a function of time. Application of List three metals that can be won from aqueous solution.        P3-                               reduction, 12. Cr2O72- reducing the orange color as it reacts Anode:                        Ag                   Cathode:                      penny, Anode H2O   +    See Diagram K, Overall mol MnO2     x   86.9g  =  4.34g. Each of these half-reactions is balanced separately and then combined to give the balanced redox equation. Hydrogen –usually +1, except when bonded to Group I or Group II, when it forms hydrides, -1. If the answer is no, write a balanced equation for the reaction that would occur. Ch 0,2 Cr - NO; S. 6. Circle all oxidizing agents. in an Au container. State two metals that can be used to cathodically ©LaBrake!&!Vanden!Bout!2014! Test # 2, Text Worksheets Quiz 1. O + +   4NO, Substance reduced          NO3-                            Reducing Determine the oxidation number of each atom in the following substances . with Pb, however, Ca+2 does not react with 7. Ni+2 reacts with Mn, however, Al+3 Ni+2 reacts with Mn, however, Al+3 agents in decreasing order of strength. Na                          0                      f)  Cl2                          0, g)  and the surface of the Al darkens. reaction:           H2O   +   Cu2+          ----->   2H+      +   Classify as oxidation, ------>     2Ag    +    PbSO4                  6                                  ClO3-               5, HP032-                  3                                  Na2O2              -1, CaH2                    -1                                 Al2(SO4)3             6, NaIO3                  5                                  C4H12              -3, 14. The breathalyzer reaction uses a spontaneous redox reaction Show your work below each reaction and put coefficients in the spaces provided: Half - Reactions Homework! Oxidation, Reduction, Agents, & Reactions. as well as a color change from purple to clear. 2Sr + … = +1.23 v, Cathode:  K+   +   1e-   →    Au                  nonspontaneous (two oxidizing agents), 2. agent                      H+                    Reducing Anions migrate to the anode and (aq), Substance oxidized                            Zn                    Substance reduced                       Cu2+, Oxidizing agent                                  Cu2+                Reducing agent                             Zn, b)   Cl2 (g)         +          2 Na (s) -------->           2 Cr3+                                         oxidizing agent                                       -0.74 v / -0.41v, 27. O. Cu2+                 &         Br-                                non-spontaneous, 30. v, MnO4-     a) NH3             -3                                 b) H2SO4                     +6, c) ZnCO3             +4                                d) Al(OH)3                  +3, e) Na               0                                  f) Cl2                           0. spontaneous. iron corrodes in air and water. 20. Zn  --------->         Al        +          Zn2+, Substance oxidized         Zn                    Oxidizing agent          Al3+, 15. Anode:                        Mg                                                                  Cathode:                    Zn, Anode each oxidation and reduction half reaction for each question above. 2Ag+            ----->   Pb2+    +         IO3-                        -------->           I2                  reduction, SnCl2               &         Ni                    Spontaneous, Ni(NO3)2         &         Fe                    Spontaneous. This example problem illustrates how to use the half-reaction method to balance a redox reaction in a solution. P    +      3e-        ----------> agent, the reducing agent, the substance oxidized and the substance reduced. 1. 6H2O   +    2MnO, 17. reactions and leads you through the use of the endo rule. NO → NO 3-6. 19. 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