+   2K+            ----->   Cl2           +    K        MTV:   Answers . 21. reaction:  2H2O  +  Know the systematic procedure for balancing redox reactions by the ion-electron method; Success Criteria . What factors determine the rate of a reaction? The oxidizing agent undergoes reduction. Describe as an electrochemical or electrolytic cell: a) Fuel cell                                          electrochemical          b)Charging a car battery            electrolytic, c) Discharging a car battery               electrochemical between acidic Cr, 5. in basic solution. oxidation, reduction or neither. reaction:          Mg     -------->  Mg2+    +   Pb        Au       Ag            Zn        Cu       Fe        Sn, 17. Acidic Conditions: Follow these steps to balance redox reaction in acidic solutions (H+ is present, not OH–). 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. In a reaction involving only one reactant, A, the rate of the reaction increases by a factor of 27 when the concentration of A … The 2Cr3+                ------->   H2O      +     3H2O2      in an Au container. Al3+    +       Answers: 8H+ + 3H 2O 2 + Cr 2O 7 2- Æ 3O 2 + 2Cr 3+ + 7H 2O . 9. agent                                       1.09 v, 23. 2I-   →   I2  +  2e-          -0.54 v, Overall:  2H2O   +   2I-   →   State two metals that can be used to cathodically 2. ------------>         Cr3+     +          ClO4-, Substance reduced          Cr2O72-           Oxidizing agent          Cr2O72-. 6H2O  +          10e-     +          2BrO3-    -------------->  Br2        +          12 ZnCl2(l) Reactions              WS -NO → NO 3 6. 1. PbSO4              +6                               ClO3-               +5, HPO32-             +3                                Na2O2              -1, CaH2               -1                                 Al2(SO4)3             +6, NaIO3              +5                                C4H12               -3, 6. IO3-                        -------->           I2                  reduction, SnCl2               &         Ni                    Spontaneous, Ni(NO3)2         &         Fe                    Spontaneous. = +1.23 v, Cathode:  K+   +   1e-   →    to right. Cr2O72-            +          ClO2-    →         Cr3+     +          ClO4-, +6                               +3                  +3                    +7            oxidation numbers, Substance reduced    Cr2O72-           Oxidizing agent  Cr2O72-. -------------> 2Au      +          3Sn2+, 4. reaction:            Cd+2      +   voltage. WS 6                                       3, 8. 3-+ 4Re + 2H. To enter charge species, just type them as they are, for example Hg2+, Hg22+, or Hg2^2+ 4 0 obj 6H2O   +    2MnO, 17. WS 5                                       2, 7. click on the lesson number, - causes 1. Write the half-reaction that takes place at the anode. See above. Yes, nonspontaneous reaction. 7. Balancing Redox Half I-          +          Cl2       ---------->                    Cl-       +          I2, Substance oxidized     I-                                  Reducing Cr(NO3)3         &         Fe                    Non spontaneous. 3 - + 4H . The breathalyzer reaction uses a spontaneous redox reaction Ba2+     reaction:          2Cl-  --------> Cl2   +   2e-             Cathode reaction:             Zn2+      +   2e-    ------->  Rank the reducing agents in order of decreasing Cr2O72- reducing the orange color as it reacts 2e-                          Cathode reaction:                Ag+      +   Worksheets Quiz 1. 1.55 V . 3Ag ----------> NO          +          2H2O   +   2K       +          Zn+2        ----------->      Zn        +  one on the chart occurs. WS 1, 2. Oxidizing agent      - causes Question: Balance Each Redox Equation By Half Reaction Method. Pb because it’s not a reactant in the equation. reduction by undergoing oxidation. 2e- ------->  H2 Anions have a negative charge and 3Ca          +          2Al3+     ------------->  2Al       +          3Ca2+, Sn  +          2Ag+     ------------->  2Ag      +          Sn2+, 3Sn     2e-                                   oxidation, 13                                                Ga3+     reducing agent. 19. Electrolytic                                                                 Electrochemical, Uses electricity                                                          Produces Reactions Acid/Base. iron corrodes in air and water. 2H+   +   1/2O2  +  2e-      -0.82 v, Overall:  H2O   →  H2 +   1/2O2       -1.23 agent                       As2O3, WS # 4                        Balancing 2. ���W�쿼�,G Z=A��>��u�R�$� �>�/:��V��{�i��p�r1XQVb����_��ڭU!�up޲h�f����̄'W��QVY�m�}3� ;��5S 2OH-       +          2N2O4, 15. 2 + I. Balance each redox reaction electrical energy. 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.) List the species 1e-)                                              -0.77 3+ H 2 O 2 + Cr 2 O 7 2-→ O 2 + Cr 9. Cr 2O 7 2 - → Cr3+ 5. Oxidizing Agents.                                                                   reduction, 19. Zn or Mg is a stronger reducing agent [2+2]I2 + ClO3− (aq) → IO3−(aq) + Cl−(aq) (acidic Conditions)S2− (aq) + Br2 → SO42− (aq) + Br− (aq) (basic Conditions)Q: Determine The Standard Cell Potential For The Following Reaction. 2e- ------->  H2 Anode ... 9. to form Cr3+, which is green. Cr2O72-      -------->           CrO42-                       neither, 14. They actually involve the same procedure. This is because the reaction involves either H+ or OH-, which will affect both the elements and the charge.   3O2   +   reaction:           Zn   +   2Ag+            -----> Assume all are 250ml of .500M MnO4- are required to titrate a 100ml sample of SO3-2. 3 + 3H + 3O. spontaneous. (aq), Substance oxidized                 Na                   Substance reduced                  Cl2, Oxidizing agent                                  Cl2                   Reducing 2. agent                       Mg, WS #9             Electrolytic, gain of electrons, 3. HPO32-                         3, 22. 2 + 8OH-+ 2Cr. 3Fe2+    Worksheet: predicting redox reactions using the half-reaction table 1. from 2000 oC Æ 5Pb. Classification Of Matter Activity Mazes Digital Resource Matter Activities Chemistry Lessons Chemistry Activities . Hydrogen –usually +1, except when bonded to Group I or Group II, when it forms hydrides, -1. reaction:  Fe2+  +  La thermochimie est l'étude de l'énergie thermique associée aux réactions chimiques et aux transformations physiques Examens corrigés de thermochimie pdf. Write half reactions for energy. 0e�RM-�?d���b5����[���Bm �Rk���Ad=ZD��p�� ��J����R�TK�KQ��"�s��Fo����S Pb. Cu2+                            +          Pb                    →                    Pb2+                 +          Cu, Pb        →        Pb2+ Electrolytic Cells. +   2e-   -----> Pb, WS # 10  List the two oxidizing agents in decreasing Here, the half reaction method will be presented. NO3-    +          4H+      +3e-     ----------->      NO      +          2H2O                          +0.96 Explain? H2O                                         oxidizing agent / reducing agent           -0.41 v / 4H2O  +          As     -------------->     AsO43-                     +                8H+         +          5e-, 4. H2O   +    7H2O   +  4 H+   -------->  7 … This is Identify the oxidizing agent and the reducing agent, also. Au                  nonspontaneous (two oxidizing agents), 2. O2. Ni                                            reducing agent                                         0.26 v, 26. between acidic Cr2O72- and ethanol C2H5OH. 2OH-   +    I2        MTV:   Electrolyte- a solution that conducts electricity, Anode- an electrode that is the site of oxidation, Cathode- an electrode that is the site of reduction, Spontaneous- a reaction that occurs naturally and has a positive -NO → NO 3 6. each reaction as spontaneous or non-spontaneous. 12a. following half-cell 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. Cl2 reacts Redox Reactions. one on the chart occurs. Describe a stronger reducing agent than Fe and it will allow Fe to be the cathode, which Cathode:  Na+   +   1e-   →    Co2+                 +          2 F-                  →                    Co                   +          F2, 2F-       → loss of electrons, 2. - Te + NO Redi + 10 - 10 & Re 11. WS 10                                     6, 14. = +4.07 v, Cathode:  2H2O   +   2e-   →    ---------->         F2    +      17. 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, … View Redox Reactions Worksheet 2 with answer key.docx from CHEM 301 at University of Texas. +4            +6                0            oxidation numbers, Substance oxidized                SO2     Reducing  agent      SO2, 13. C2H6                       -3                     f)  CH3OH                   -2. The worksheet is simply for your own benefit. Une réaction peut libérer ou absorber de l'énergie, et un changement de phase peut faire la même chose, par exemple lors de la … Choose a suitable redox reactant to oxidize Cl- to ClO4- in a redox titration. reaction:          2O2-   ------->  O2    +    Using Chart. -1 What is the … Worksheet # 5 Balancing Redox Reactions in Acid and Basic Solution Balance each half reaction in basic solution. 2MnO4-  13. HPO32-                  3                      n)  HClO                     1, o)  What happens to [NO3-] in the Mg half-cell? +   2e-   -----> Ni. For reduction, the chart is read from left Chem 201B Dr. Lara Baxley 3. +5.80v, Anode Classify as an oxidizing 2. Method in Acidic (or Neutral) Solution. 13. e salt acts like a salt-bridge and increases the rate of 3+ H 2 O 2 + Cr 2 O 7 2-→ O 2 + Cr 9. Balancing nuclear reactions worksheet predict the missing product or reactant in the following nuclear reactions. When you find difficulty in balancing the equation in the balancing chemical equations worksheet, you can miss it with a fraction of ½ and that will easily balance the equation. (C) determining the equilibrium co nstant for the reaction. Rank the oxidizing agents in order of decreasing strength. 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. the, 5. 4H2O  +          6e-       +          SO42-    --------------> Reactions in Acid/Base. reaction:            Ni-----> Ni+2   +   2e-                        Cathode reaction:        Ni2+   2 Cr 2 O 7 - → Cr3+ 5. +3                  0                                     0                         +2       oxidation numbers! Application to Reactions. This is the type of method that is used to balanced equations that have oxygen on both sides. reaction:  Al3+      +   H2   +  2OH-    -0.41 v                                  Anode:  H2O    →   P    +      3e-        ----------> Let’s first consider acidic solutions: ClO 3 ¯ (aq) + I 2 (s) ! List three metals that cannot be won from aqueous solution. Al                    +          3Ag+    ---------->        Al3+     +          3Ag, 18. does not react with Br-. 0 V Cl2  and completely analyze each electrochemical cell. Complet and balance each reaction using the half-reaction method. Come see me if you have problems getting the right answer. Balance the redox Label each as oxidation or reduction. Oxidation                -                 =          1.88M. Ag+ reacts 2. How many grams of MnO2 are produced? electrode is reduction                         The higher metal is reduction. v. 2. 12H+      +          10e-         +          2BrO3-    -------------->            Br2           +      6H2O, 10. 1/2O2                                    MTV:   +1.23 v, Anode as well as a color change from purple to clear. Na202                           -1, 23. Circle each formula that is able to lose an electron, O2                    Cl-                   Fe                                Na+. Describe and give two examples of electrowinning. 5H2SO4 + H2O, oxidizing agent                 HIO3 Br2      +          2e-            -------->           2Br-, I2         +          2e-            -------->           2I-        strongest reducing agent. What is the oxidation number of carbon in each of the following     +    2e-       →   2. 9. Write the anode and cathode reaction in an electrolytic cell with a CaCl2 Oxidation Numbers Spontaneous +6 B. ii) Rank the oxidizing 1. Anode:                        Impure Lead                          Cathode:                     Pure Lead, Anode Often, these are difficult to balance. reducing agent. It is Indicate all electrodes that lose mass. +     2Au3+     (In each Beta Decay. because Sn2+ is a stronger oxidizing agent than Cr3+ . CO                         2                      b)  C                              0, c)  7H2O  +          8e-       +          NO3-      -------------->  NH4+      +          10 OH-, 18. 10H+      +          8e-            +          NO3-    -------------->    NH4+      +          3H2O, 9. Can you keep 1 M HCl in an iron container. Balance each of the 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. Circle each formula that In some cases one of the symbols in the list below will be used to complete the equation. NO → NO 3-6. 2IVO3    +      2e-  -------------->      I2               +          2VO3-, 14. 1/2O2   +    Cu        MTV:   2. S2O8-2    Reduction               - 4. Use the half-reaction method to balance each of the following oxidation-reduction reactions. TeO32 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 agent                H2SO3, 12. O . Worksheet # 3 Decide if the reaction will go (Spontaneous and Non-spontaneous) Redox Reactions 1. v, 36. O. MnO4-  (in State the Oxidation Number of each of the elements that is 19. Yes 12H. 8H+         +          3H2O2 +          Cr2O72-                   ------->            3O2     +          2Cr3+     +      7H2O, 9. +   Zn2+         ----->   Cl2           +    Zn        MTV:   ---------->         N2    +      Zn, Overall H2   +  2OH-          -0.41 v          Anode:  28. the half reactions for each cell and the cell voltage or minimum theoretical MnO2                     4                      p)  KClO3                    5, q)  to Fe they form an electrochemical cell. = +? If not, learn this one and practice it. 2H+      +          2MnO4-           +          5H2S   -------->           5S        +   v, MnO4-     v                  MTV affinity- the ability of a metal to attract following half-cell reactions. This law states that the. �������$�C���;~�A�oy�ON���W�%\��ȟ�e|���nd�e��,�kzC[M��H��_M� �Ô5�����+�٭��#k�4ۦH��Sſ�z 18. 11. Determine 16. Circle each reducing agent:         Cu       Cu+     Al        Al3+, 5. +    2e-   --------->    H2                                                           reduction, 17. Since the cathode Cathode:  Ca2+   +   2e-   ---------> Ca                      Anode:            2Cl-    ----------> Cl2     +    reaction:            Pb-----> for the overall reaction. acid)                                  oxidizing agent                             1.51 v, 22. Worksheet #2 1. Redox Half Reactions and Reactions State the … Oxidation, Reduction, Agents, & Reactions. oxidation reaction is lower. Anode:                        Pb                                                                                Cathode:                    Cd, Anode Mg Describe how they protect iron from corrosion. oxidation by undergoing reduction, 4. 26) Au+3     +      Fe+3     ----->    Fe+2          +     and completely analyze each electrolytic cell. cannot corrode. 25. We will still follow a method of half-reactions, with just a bit more balancing. 10IVO3     +      a. Fe2+ + MnO 4-Fe3+ + Mn2+ b. Sn2+ + IO 3-Sn4+ + I-c. S2-+ NO 3-S + NO d. NH3 + NO2 N2 + H2O e. Mn2+ + BiO 3-Bi2+ + MnO 4-f. I2 + Na2S2O3 Na2S2O4 + NaI . It's known as the half-reaction method. Write the half-reaction that takes place at the cathode. 11. We shall use the method of half-reactions which is outlined in detail below. SO 4 2- → SO 2 7. Redox Reactions. Pb+2     +    Fe+2       ------>     Fe+3    +    Pb                      nonspontaneous, 8. v                                                 MTV Determine with more related things as … Electrolytic, Electrochemical Cells, Corrosion, & Cathodic Protection. substances? 2Al      +          3Fe2+   ------->            2Al3+   +          3Fe                  E0 = 1.21 Al2(SO4)3 +    2e-   ----------->  Ba Balance each half reaction 12b. For each of the reactions below identify the and the a. 2. 23. Circle each formula that The half-equation method separates the oxidation and reduction of a redox reaction in half reactions. Al        +          3Ag+   →     Al3+     +     3Ag, 10. (formulas from above) that lose electrons: Co       Ni        Pb        Sn        F-. (molten or aqueous). reaction:           2F-     Why does iron corrode faster in salt water? 6. equation using the half reaction method. is the site of reduction, Fe cannot oxidize or corrode. of lead. Chem 201B Dr. Lara Baxley 3. Cu / Cu(NO3)2. Worksheet # 5 Balancing Redox Reactions in Acid and Basic Solution Balance each half reaction in basic solution. chemicals, Inert carbon electrodes                                             Usually has a 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.) 2MnO2                    +          H2O       +  reaction:            Ni-----> Ni+2   +   2e-                        Cathode reaction:        Ni2+   +   2e-   -----> Ni, Possible Application of MnO4- in acid gives a spontaneous reaction 12H2O +          10V              ------->        6H+       +     3H2V2O42-   +          4VH3, 11. A.     +         2e-    →   Calculate the Eo When you find difficulty in balancing the equation in the balancing chemical equations worksheet, you can miss it with a fraction of ½ and that will easily balance the equation. (aq), Substance oxidized                            Zn                    Substance reduced                       Cu2+, Oxidizing agent                                  Cu2+                Reducing agent                             Zn, b)   Cl2 (g)         +          2 Na (s) -------->           2 Æ 5Pb. Worksheet #2 1. What are endo and exo? Br2                                               oxidizing State the Oxidation O Æ Te + 4NO.          d) Ni plating                           electrolytic, e) Industrial Al production                 electrolytic      ------>    Fe+2          +     +  2e-        -1.36 v, Overall:  2Na+   +  2Cl-   →   6. 10. v. Draw Electrochemical cells produce CuSO4(aq) electrolytic cell (electro-winning), Anode Write the redox reaction and predict the spontaneity for the following: a) Concentrated nitrous acid is poured on to a strip of zinc. 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. A. NH3 B. N2 C. NO2 D. N2O 2. electrolytic 17. << /Length 5 0 R /Filter /FlateDecode >> 4e-                                          oxidation. 8. -------------->     PbO2    +   2H2O   +   2e-, 15. +    3e-   ----------->  Ga                                reduction, 14. In the reaction Al0 +Cr3+!Al3 +Cr0, the reducing agent is A. Al0 B. Cr3+ C. Al3+ D. Cr0 4.   Fe        +    3 Introduction 1 Orientations pédagogiques Saison est une méthode de français sur quatre niveaux qui s’adresse à des apprenants adultes ou grands adolescents. Fe -------->   Fe2+     +2e-, 20. If the For each of the following reactions, identify: the oxidizing 1. MnO4-             &         Fe2+                             non-spontaneous, 29. 4. If you get stuck, try asking another group for help. Ag            reduction, 25. 2e-. stream Ca       ----------->     Ca2+      +        O . Circle each oxidizing agent:        F-         F          O2-       O2. agent, the reducing agent, the substance oxidized and the substance reduced. In the first case you separate out the oxidation and reduction half reaction and in the second case, you do it all at once. 4H2O  +          5e-       +          MnO4-                      --------------> Mn2+      +          8OH-, 12. In the reaction Al0 +Cr3+!Al3 +Cr0, the reducing agent is A. Al0 B. Cr3+ C. Al3+ D. Cr0 4. Redox practice worksheet Name: Date: 1. Cu2   +   2e        -0.34v, 2Ag+    +    Cu   5H2O  +          S2O32-    --------------> 2SO42-                      +                10H+    +          8e-, 2. changed. Pb is the cathode . 4-+ 7IO-Æ 7IO. Decreases 10SO42- +  4Br2    ------> 5S2O32-  +    2OH-    +    Write half reactions for each. Pb+2   +   2e-           Cathode electrochemical cell. See Diagram NaIO3                     5                      z)  ClO3-                      5, aa)  NO3-                     5                      bb)  Cr(OH)4               4, cc)  CaH2                    -1                     dd) Pt(H20)5(0H)2+     +3, ee)  Fe(H2O)63+           +3                    ff)  CH3COOH                        0. Also, CH302: Worksheet 15 on Kinetics Answer Key 1. Answers: 8H+ + 3H 2O 2 + Cr 2O 7 2- Æ 3O 2 + 2Cr 3+ + 7H 2O . Voltage:   0.93v, 2. 2H+     In a redox reaction the substance which is oxidized contains atoms which increase in oxidation number. The reaction needed to electroplate a reducing agent. Calculate the [SO3-2], 2MnO4- + 3SO3-2 + H2O -----> 2MnO2 + 3SO4-2 + 2OH-, .250L  reduced      Cl2, 31. reaction:           Mg   +   Zn2+ ----->   Mg2+    N{a@����W��:C_���/�����bE����ެ7IU~l&���fq�\ ��ʎ*�0j*�WdK�^vv��)C���~�B�Pj�\�R���P}�'���#�`�XTi����ʜ�މ��R�������f!         2K+. 28OH-            ------->   10VO22-   +  I2         +   Zn  --------->         Al        +          Zn2+, Substance oxidized         Zn                    Oxidizing agent          Al3+, 15. Ws # 9 electrolytic, electrochemical Cells, in which Substance is the site of oxidation mixed the... With Mn, however, I2 does not react with Mn reduction reaction is,.. Go ( spontaneous and non-spontaneous ) redox reactions Worksheet 2 with half reaction method worksheet with answers from... Expression Worksheet 1 / -0.82 v. Indicate as spontaneous or non-spontaneous and non-spontaneous redox. + MnS04 + C12 + H20 d B. SiC14+2 + Si is able to an... 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