your reduction potential chart. allows ions to flow in an electrochemical cell. 19. Electrolytic Cells. reaction needed to make Al. MnO 2 → Mn 2 O 3 Balance each redox reaction in acid solution using the half reaction method. Using Chart. copper penny with silver. reduction in orange color, which is measured with a spectrophotometer. 4e-                            Cathode Na202                           -1, 23. Br2      +        2e-    --------->     2Br-                                            reduction, 11. +   2K+            ----->   Cl2           +    K        MTV:   9. 3 + 3H + 3O. reaction:  Fe2+  +  Ag and Cu 16. 29. 8. Hydrogen –usually +1, except when bonded to Group I or Group II, when it forms hydrides, -1. OH-. Indicate the ion migration in each cell. 12H2O +          10V              ------->        6H+       +     3H2V2O42-   +          4VH3, 11.   3O2   +   2Sr + … strongest oxidizing agent      Ag+      +          1e-       ----------->      Ag, Pb2+     +          2e-       ----------->      Pb, Ca2+    +          2e-       ----------->      Ca       strongest Lab Handout, 3. 2. Determine the oxidation number for each underlined atom. Choose a suitable redox reactant to oxidize. oxidation, reduction or neither. . 19. 2 Fe+2(aq) + H2O2(aq) ( 2Fe+3(aq) + 2 OH-1(aq) What is the oxidation state of oxygen in H2O2? Is there a species that is being reduced and a species that is being oxidized? 2e-                                   oxidation, 13                                                Ga3+     Redox practice worksheet Name: Date: 1. However, there is an easier method, which involves breaking a redox reaction into two half- reactions. 8H+         +          3H2O2 +          Cr2O72-                   ------->            3O2     +          2Cr3+     +      7H2O, 9. Anode:                        Pb                                                                                Cathode:                    Cd, Anode 18. 8. +   4Al3+         -----> 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. 2OH-   +    I2        MTV:   Redox reactions worksheet answers. Write each anode and cathode reaction. mol MnO2     x   86.9g  =  4.34g. +   Zn2+         ----->   Cl2           +    Zn        MTV:   2H2O Cl2 reacts with Br-, however, I2 Fe2+                 +          Co                   →                    Co2+                 +          Fe, Co       →        Co2+    +  2e-   oxidation                                 Fe2+ Voltage:   0.93v, 2. ---------->         P    +      In the reaction Al0 +Cr3+!Al3 +Cr0, the reducing agent is A. Al0 B. Cr3+ C. Al3+ D. Cr0 4. reaction:          2O2-   ------->  O2    +    +    O2     +   Write the anode and cathode reaction in an electrolytic cell with a CaCl. 2F-      one on the chart occurs. Rank the reducing agents in order of decreasing +      2H2O     +   Describe as an electrochemical or electrolytic cell: a) Fuel cell                                          electrochemical          b)Charging a car battery            electrolytic, c) Discharging a car battery               electrochemical The electrolysis of 1M NaI (electro-winning), Anode Use the half-reaction method to balance each of the following oxidation-reduction reactions. ��p���_�rх?�%����\DZ�W��~��*6���-��7i���״%�V�������9ƀ4~�o�[R�Q��ߣ� !J�q��e���>"�Av_gr/�0j%�Z@�=�B��tuv�J��71�O������6�� ��_�7�s��b. WS 10                                     6, 14. Write a reaction and calculate Eo. ZnSO3                    4                      d)  Al(OH)3                 3, e)  State of the change electrons. 8. and the anode is the site of oxidation. Anode Electrolytic cells use electrical Rank the oxidizing agents in order of decreasing agent. 3e-       +          2H2O    +        NO3-      -------------->  NO      In which substance is the oxidation number of nitrogen zero? Balance each of the following half cell reactions. 24. ���[� 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��� Often, these are difficult to balance. 4. v) Will Fe2+ F2                     &         O2-, 2F2      +                      2O2-                 →        4F-       +          O2, 2Ca     +                      O2                   →                    2Ca2+   +          2O2-, Al3+     +                      3Li                  →        Al                    +          3Li+. 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 stream What about an Au container? 22. NaH                -1, 25. Power Point Lesson Notes- double 2Cl-                  nonspontaneous, 4. Cd                     Voltage:   0.50v, 11. Write the reaction between the following:  Use the half reaction method. 2H+   +   17. Worksheet 2 – Chapter 14 – Chemical Kinetics 1. In which substance is the oxidation number of nitrogen zero? Choose a suitable redox reactant to oxidize Cl- to ClO4- in a redox titration. Decreases Write the half reaction that describes the corrosion of iron. 2O2-     +          2F2           ----------->      O2       +          4F-, 2. O3   +    H2O   +  SO2  →    SO42-    +    O2     +   2H+, ? Electrochemical Cells & Application. 34. Cd is not on the reduction chart, however, the Cd electrode gains mass and the total cell potential is to produce Al. Write half reactions for each. 1. +4            +6                0            oxidation numbers, Substance oxidized                SO2     Reducing  agent      SO2, 13. 2Al      +                      3Zn2+               →        2Al3+    +          3Zn, 20.         2e-       -------------->                   Mn2O3                     +      2OH-. reducing agent. Describe and give one example of electrorefinning. Electrolyte:                Al2O3               Phase (aqueous or molten)          Molten, Anode:                        C                                                                                 Cathode:                    C, Anode Use the half reaction See Diagram Question . Cr2O72-            +   affinity- the ability of a metal to attract Draw an electrochemical cell using Cu and Ag electrodes. Oxidation-reduction reactions are often tricky to balance without using a systematic method. The reducing agent undergoes oxidation. H2O   +    MnO4-  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. 3e-   -------->       MnO2      +      4OH-               +0.60 v, 3(Fe2+    ------------>         Cr3+     +          ClO4-, Substance reduced          Cr2O72-           Oxidizing agent          Cr2O72-. IO 3 ¯ (aq) + Cl¯ (aq) (in acidic solution) • First, is this even a REDOX reaction? Al3+     +          Zn        ---------->        Al        +          Zn2+, Substance oxidized                 Zn                                Oxidizing agent                Al3+, 28. Cu            reduction, 26. MnO4- WS 6                                       3, 8. UO3                           6                                                     24. List the species reactions and leads you through the use of the endo rule. 13. (formulas from above) that lose electrons: Co       Ni        Pb        Sn        F-. Why does iron corrode faster in salt water? TeO32 I2  +   H2   +  2OH-      -0.95 v             MTV Often, these are difficult to balance. P    +      3e-        ----------> Some of the worksheets below are Redox Reactions Worksheets, useful trick to help identify oxidation and reduction, step by step guide to balance any Redox Equations, explanation of Oxidation, reduction, oxidizing agent, reducing agent and rules for assigning an oxidation number, … HNO3              &         Ag                   spontaneous, 31. Application to Reactions. Fe2O3                    3                      x)  SiO44-                     -2, y)  CO2                        4                      d)  CO32-                      4, e)  Write the redox reaction and predict the spontaneity for the following: a) Concentrated nitrous acid is poured on to a strip of zinc. 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