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Write the half-reaction that takes place at the cathode. Zn or Mg is a stronger reducing agent 2. does not react with Br-. of lead. Cd Voltage: 0.50v, 11. Circle all oxidizing agents. cannot corrode. Application of Salt 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 . 250ml of 0.200M MnO4- reacts with excess SO3-2. 4H2O + 6e- + SO42- --------------> f) Cl2 production electrolytic. 10. Circle each formula that is able to lose an electron, O2 Cl- Fe Na+, 11. 3e- -------> Al, Overall Write each anode and cathode reaction. reaction: Mg + Zn2+ -----> Mg2+ 5H2SO4 + H2O, oxidizing agent HIO3 Draw a Cd/Pb IO 3 ¯ (aq) + Cl¯ (aq) (in acidic solution) • First, is this even a REDOX reaction? reduction or neither. Worksheet: predicting redox reactions using the half-reaction table 1. click on the lesson number. Pb+2 spontaneous, 3. Redox Reactions. Cu2+ & Br- non-spontaneous, 30. electrochemical cells, in which two redox couples are placed in separate compartments as opposed to their direct contact. Worksheet 25 - Oxidation/Reduction Reactions Oxidation number rules: Elements have an oxidation number of 0 Group I and II – In addition to the elemental oxidation state of 0, Group I has an oxidation state of +1 and Group II has an oxidation state of +2. in acid solution using the half reaction method. Lab: The Strength of Circle each oxidizing agent: F- F O2- O2. reaction: Ni-----> Ni+2 + 2e- Cathode reaction: Ni2+ An important idea is that balancing Redox reactions is different in acidic conditions than it is in basic conditions. %��������� 1. Each of these half-reactions is balanced separately and then combined to give the balanced redox equation. For reduction, the chart is read from left 22. 2 + I. 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.) If there are two possible oxidation reactions, the lowest ii) Rank the oxidizing What would happen if you used an aluminum spoon to stir a solution of, The breathalyzer reaction uses a spontaneous redox reaction Worksheet #5 Balancing Redox Reactions in Acid and Basic Solution Balance each half reaction in basic solution. 3-+ 4Re + 2H. If not, learn this one and practice it. O. e.g. = +1.23 v, Cathode: K+ + 1e- → 2H+ + 2e- ------> H2 0.00 v, Mg ----------> Mg2+ + 2e- 2.37 v, Mg + 2H+ ----------> Mg2+ + H2 2.37 types of chemical reactions worksheet answer key, chemical reaction types worksheet and type of chemical reaction worksheet answer chemistry are three of main things we will present to you based on the gallery title. 2N3- 1.55 V . Balancing Redox Reaction by Ion electron Method (Half reaction method) Steps: Divide the complete reaction into two half reaction, one representing oxidation and other representing reduction. N{a@����W��:C_���/�����bE����ެ7IU~l&���fq�\ ��ʎ*�0j*�WdK�^vv��)C���~�B�Pj�\�R���P}�'���#�`�XTi����ʜ�މ��R�������f! �������$�C���;~�A�oy�ON���W�%\��ȟ�e|���nd�e��,�kzC[M��H��_M� �Ô5�����+�٭��#k�4ۦH��Sſ�z 2e- -------> 2I- → I2 + 2e- -0.54 v, Overall: 2H2O + 2I- → voltage. c) Aluminum lawn furniture is exposed to the action of wind (O 2)and rain (H 2O). 1.3NbO v, 3(Ag Let’s first consider acidic solutions: ClO 3 ¯ (aq) + I 2 (s) ! State of the change 2IVO3 + 2e- --------------> I2 + 2VO3-, 14. 2+ + 2IO. + 2I- -----> Here, the half reaction method will be presented. 10. 5. Reducing agent - causes 3. 13. Balance the redox equation using the half reaction method. 2+ + 2IO. In an electrochemical cell electrons exit the electrode, which is negative. O + 3H. AsO. Cu If the answer 2Cr3+, 5. Voltage: 0.93v, 2. MnO2 4 p) KClO3 5, q) HPO32- 3 n) HClO 1, o) 3As2O3 + 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 ---------> Al + Zn2+, Substance oxidized Zn Oxidizing agent Al3+, 15. For each of the reactions below identify the and the a. If the 4e- oxidation. electricity, Nonspontaneous Spontaneous, Makes chemicals Uses 2, 4. agent As2O3, WS # 4 Balancing In some cases one of the symbols in the list below will be used to complete the equation. these are both, so state two voltages and indicate that it can be an oxidizing 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 2. - + 2N2O4 + H2O -------> Te + 4NO3- + 2H+, 10. a) NH3 -3 b) PbO2 4 r) PbSO4 2, s) What factors determine the rate of a reaction? Fe, Overall 3 + 3H + 3O. No, because Fe2+ is a weaker oxidizing agent PbSO4 2, 20. Pb because it’s not a reactant in the equation. State the Oxidation Number of each of the elements that is underlined. As H AsO4 + AsHz od sml water OLM ord the Physical and Chemical Changes Set-up … If the answer is no, write a balanced equation for the reaction that would occur. Cell potential . Chem 116 POGIL Worksheet - Week 6 Kinetics - Part 2 Why? H2 + 4Br2 ----------> 5S2O32- + occur. 1. Often, these are difficult to balance. reaction: 2Cl- --------> Cl2 + 2e- Cathode reaction: Zn2+ + 2e- -------> 2. v MTV What chemicals are made at the Pt electrode on the left? 2O2- O2 + 2 Sn → O2- + 2 Sn2+, Sn → Sn2+ 2H+, Substance Co + Fe3+ -----------> Co2+ + Fe2+, Substance oxidized Co Reducing agent Co, Oxidizing agent Fe3+ Substance Come see me if you have problems getting the right answer. Une réaction peut libérer ou absorber de l'énergie, et un changement de phase peut faire la même chose, par exemple lors de la … 8IO3- 14H2O, 16. 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.) Explain? 1. 16. 2 + 8OH-+ 2Cr. ------------> Cr3+ + ClO4-, Substance reduced Cr2O72- Oxidizing agent Cr2O72-. In an electrochemical cell electrons exit the electrode, which is, 7. Ag 0.80v Cu -------> equation. Answers: 8H+ + 3H 2O 2 + Cr 2O 7 2- Æ 3O 2 + 2Cr 3+ + 7H 2O . SO 4 2- → SO 2 7. Chem 201B Dr. Lara Baxley 3. 12d. Worksheet #2 1. Balance each of the No, Fe + 2H+ --------> Fe2+ + H2. You should try to answer the questions without referring to your textbook. This law states that the. 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. 2Cr3+ -------> H2O + 3H2O2 24. Describe as oxidation or reduction. Since the cathode Label each anode and cathode. reaction: Ni-----> Ni+2 + 2e- Cathode reaction: Ni2+ + 2e- -----> Ni, Possible Write half reactions for H2SO3, substance reduced HIO3 v, Overall: 4K+ + 2O2- → 2MnO4- + 3SO3-2 + H2O -----> 2MnO2 + 3SO4-2 + 2OH-, 0.250L The unbalanced, net reaction is shown below, Br-+ MnO 4-→ Br 2 + Mn 2+ 1. Classify as oxidation, Standard Potentials reducing agent. One variation on this gives us the concept of half-life, which applies to chemical reactions and nuclear decay. We will still follow a method of half-reactions, with just a bit more balancing. View Redox Reactions Worksheet 2 with answer key.docx from CHEM 301 at University of Texas. Using Chart. No, Spontaneous reaction. Anions migrate to the anode 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 between acidic Cr, 5. The electrolyte. Determine For oxidation, the chart is read from right NO3- + 4H+ +3e- -----------> NO + 2H2O +0.96 The electrolysis of water to make H2 and O2. In an electrochemical cell the reduction reaction is, 1. oxidation, reduction or neither. (acid) & H2O spontaneous, 32. Reaction Order and Rate Law Expression Worksheet 1. Æ 5Pb. 9. MnO2 --------> MnO4- oxidation, 13. HSO4- 6, 24. Often, these are difficult to balance. 7. cations have a positive charge. 2O2- → O2 + 2Al + 3Fe2+ -------> 2Al3+ + 3Fe E0 = 1.21 See Diagram 4OH-, 13. (lower on the chart) and is the anode and Fe is the cathode. Complet and balance each reaction using the half-reaction method. NO → NO 3-6. 2Sr + … strongest oxidizing agent Ag+ + 1e- -----------> Ag, Pb2+ + 2e- -----------> Pb, Ca2+ + 2e- -----------> Ca strongest strongest oxidizing agent Cl2 + 2e- --------> 2Cl-, Ag+ + 1e- -----------> Ag, Mg2+ + 2e- -----------> Mg strongest reducing 2e- 0.13v Cathode v, MnO4- a) The Half-Reaction Method. Write the half reaction that describes the corrosion of iron. The electrolyte is Al2O3 and its phase is molten loss of electrons, 2. Rank the oxidizing agents in order of decreasing strength. 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 each reaction as spontaneous or non-spontaneous. In an electrolytic cell, reduction occurs at the, 2. 6. HCl & Mg spontaneous. H2 + 2OH- -0.41 v Anode: Balance each of the 19. 2H+ What is the oxidation number of carbon in NaHCO3? Worksheets: General Chemistry (Guided Inquiry) ... Know the systematic procedure for balancing redox reactions by the ion-electron method; Success Criteria. AsO. 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. reduced Cr6+. Fe + - an electrode that is the site of oxidation, - an electrode that is the site of reduction, - a reaction that occurs naturally and has a positive Can you keep 1 M HCl in an iron container. the, 5. 12c. )�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. WS 8 4, 12. This is best shown by working an example. WS 9 5, 13. 1e- -------> Ag, Overall Reduction - as spontaneous or non-spontaneous. A. NH3 B. N2 C. NO2 D. N2O 2. 2e- Cathode reaction: Ag+ + voltage. 2e- -------> Zn x 2 Cr 2 O 7 - → Cr3+ 5. 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Al is on the left so it’s the anode. 4H2O + 5e- + MnO4- --------------> Mn2+ + 8OH-, 12. What is the fuel in a fuel cell? + Br2 nonspontaneous, 6. WS 5 2, 7. Will electrolysis occur? Choose a suitable redox reactant to oxidize Cl- to ClO4- in a redox titration. 8. Write the half-reaction that takes place at the cathode. Zn or Mg is a stronger reducing agent 2. does not react with Br-. of lead. Cd Voltage: 0.50v, 11. Circle all oxidizing agents. cannot corrode. Application of Salt 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 . 250ml of 0.200M MnO4- reacts with excess SO3-2. 4H2O + 6e- + SO42- --------------> f) Cl2 production electrolytic. 10. Circle each formula that is able to lose an electron, O2 Cl- Fe Na+, 11. 3e- -------> Al, Overall Write each anode and cathode reaction. reaction: Mg + Zn2+ -----> Mg2+ 5H2SO4 + H2O, oxidizing agent HIO3 Draw a Cd/Pb IO 3 ¯ (aq) + Cl¯ (aq) (in acidic solution) • First, is this even a REDOX reaction? reduction or neither. Worksheet: predicting redox reactions using the half-reaction table 1. click on the lesson number. Pb+2 spontaneous, 3. Redox Reactions. Cu2+ & Br- non-spontaneous, 30. electrochemical cells, in which two redox couples are placed in separate compartments as opposed to their direct contact. Worksheet 25 - Oxidation/Reduction Reactions Oxidation number rules: Elements have an oxidation number of 0 Group I and II – In addition to the elemental oxidation state of 0, Group I has an oxidation state of +1 and Group II has an oxidation state of +2. in acid solution using the half reaction method. Lab: The Strength of Circle each oxidizing agent: F- F O2- O2. reaction: Ni-----> Ni+2 + 2e- Cathode reaction: Ni2+ An important idea is that balancing Redox reactions is different in acidic conditions than it is in basic conditions. %��������� 1. Each of these half-reactions is balanced separately and then combined to give the balanced redox equation. For reduction, the chart is read from left 22. 2 + I. 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.) If there are two possible oxidation reactions, the lowest ii) Rank the oxidizing What would happen if you used an aluminum spoon to stir a solution of, The breathalyzer reaction uses a spontaneous redox reaction Worksheet #5 Balancing Redox Reactions in Acid and Basic Solution Balance each half reaction in basic solution. 3-+ 4Re + 2H. If not, learn this one and practice it. O. e.g. = +1.23 v, Cathode: K+ + 1e- → 2H+ + 2e- ------> H2 0.00 v, Mg ----------> Mg2+ + 2e- 2.37 v, Mg + 2H+ ----------> Mg2+ + H2 2.37 types of chemical reactions worksheet answer key, chemical reaction types worksheet and type of chemical reaction worksheet answer chemistry are three of main things we will present to you based on the gallery title. 2N3- 1.55 V . Balancing Redox Reaction by Ion electron Method (Half reaction method) Steps: Divide the complete reaction into two half reaction, one representing oxidation and other representing reduction. N{a@����W��:C_���/�����bE����ެ7IU~l&���fq�\ ��ʎ*�0j*�WdK�^vv��)C���~�B�Pj�\�R���P}�'���#�`�XTi����ʜ�މ��R�������f! �������$�C���;~�A�oy�ON���W�%\��ȟ�e|���nd�e��,�kzC[M��H��_M� �Ô5�����+�٭��#k�4ۦH��Sſ�z 2e- -------> 2I- → I2 + 2e- -0.54 v, Overall: 2H2O + 2I- → voltage. c) Aluminum lawn furniture is exposed to the action of wind (O 2)and rain (H 2O). 1.3NbO v, 3(Ag Let’s first consider acidic solutions: ClO 3 ¯ (aq) + I 2 (s) ! State of the change 2IVO3 + 2e- --------------> I2 + 2VO3-, 14. 2+ + 2IO. + 2I- -----> Here, the half reaction method will be presented. 10. 5. Reducing agent - causes 3. 13. Balance the redox equation using the half reaction method. 2+ + 2IO. In an electrochemical cell electrons exit the electrode, which is negative. O + 3H. AsO. Cu If the answer 2Cr3+, 5. Voltage: 0.93v, 2. MnO2 4 p) KClO3 5, q) HPO32- 3 n) HClO 1, o) 3As2O3 + 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 ---------> Al + Zn2+, Substance oxidized Zn Oxidizing agent Al3+, 15. For each of the reactions below identify the and the a. If the 4e- oxidation. electricity, Nonspontaneous Spontaneous, Makes chemicals Uses 2, 4. agent As2O3, WS # 4 Balancing In some cases one of the symbols in the list below will be used to complete the equation. these are both, so state two voltages and indicate that it can be an oxidizing 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 2. - + 2N2O4 + H2O -------> Te + 4NO3- + 2H+, 10. a) NH3 -3 b) PbO2 4 r) PbSO4 2, s) What factors determine the rate of a reaction? Fe, Overall 3 + 3H + 3O. No, because Fe2+ is a weaker oxidizing agent PbSO4 2, 20. Pb because it’s not a reactant in the equation. State the Oxidation Number of each of the elements that is underlined. As H AsO4 + AsHz od sml water OLM ord the Physical and Chemical Changes Set-up … If the answer is no, write a balanced equation for the reaction that would occur. Cell potential . Chem 116 POGIL Worksheet - Week 6 Kinetics - Part 2 Why? H2 + 4Br2 ----------> 5S2O32- + occur. 1. Often, these are difficult to balance. reaction: 2Cl- --------> Cl2 + 2e- Cathode reaction: Zn2+ + 2e- -------> 2. v MTV What chemicals are made at the Pt electrode on the left? 2O2- O2 + 2 Sn → O2- + 2 Sn2+, Sn → Sn2+ 2H+, Substance Co + Fe3+ -----------> Co2+ + Fe2+, Substance oxidized Co Reducing agent Co, Oxidizing agent Fe3+ Substance Come see me if you have problems getting the right answer. Une réaction peut libérer ou absorber de l'énergie, et un changement de phase peut faire la même chose, par exemple lors de la … 8IO3- 14H2O, 16. 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.) Explain? 1. 16. 2 + 8OH-+ 2Cr. ------------> Cr3+ + ClO4-, Substance reduced Cr2O72- Oxidizing agent Cr2O72-. In an electrochemical cell electrons exit the electrode, which is, 7. Ag 0.80v Cu -------> equation. Answers: 8H+ + 3H 2O 2 + Cr 2O 7 2- Æ 3O 2 + 2Cr 3+ + 7H 2O . SO 4 2- → SO 2 7. Chem 201B Dr. Lara Baxley 3. 12d. Worksheet #2 1. Balance each of the No, Fe + 2H+ --------> Fe2+ + H2. You should try to answer the questions without referring to your textbook. This law states that the. 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. 2Cr3+ -------> H2O + 3H2O2 24. Describe as oxidation or reduction. Since the cathode Label each anode and cathode. reaction: Ni-----> Ni+2 + 2e- Cathode reaction: Ni2+ + 2e- -----> Ni, Possible Write half reactions for H2SO3, substance reduced HIO3 v, Overall: 4K+ + 2O2- → 2MnO4- + 3SO3-2 + H2O -----> 2MnO2 + 3SO4-2 + 2OH-, 0.250L The unbalanced, net reaction is shown below, Br-+ MnO 4-→ Br 2 + Mn 2+ 1. Classify as oxidation, Standard Potentials reducing agent. One variation on this gives us the concept of half-life, which applies to chemical reactions and nuclear decay. We will still follow a method of half-reactions, with just a bit more balancing. View Redox Reactions Worksheet 2 with answer key.docx from CHEM 301 at University of Texas. Using Chart. No, Spontaneous reaction. Anions migrate to the anode 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 between acidic Cr, 5. The electrolyte. Determine For oxidation, the chart is read from right NO3- + 4H+ +3e- -----------> NO + 2H2O +0.96 The electrolysis of water to make H2 and O2. In an electrochemical cell the reduction reaction is, 1. oxidation, reduction or neither. (acid) & H2O spontaneous, 32. Reaction Order and Rate Law Expression Worksheet 1. Æ 5Pb. 9. MnO2 --------> MnO4- oxidation, 13. HSO4- 6, 24. Often, these are difficult to balance. 7. cations have a positive charge. 2O2- → O2 + 2Al + 3Fe2+ -------> 2Al3+ + 3Fe E0 = 1.21 See Diagram 4OH-, 13. (lower on the chart) and is the anode and Fe is the cathode. Complet and balance each reaction using the half-reaction method. NO → NO 3-6. 2Sr + … strongest oxidizing agent Ag+ + 1e- -----------> Ag, Pb2+ + 2e- -----------> Pb, Ca2+ + 2e- -----------> Ca strongest strongest oxidizing agent Cl2 + 2e- --------> 2Cl-, Ag+ + 1e- -----------> Ag, Mg2+ + 2e- -----------> Mg strongest reducing 2e- 0.13v Cathode v, MnO4- a) The Half-Reaction Method. Write the half reaction that describes the corrosion of iron. The electrolyte is Al2O3 and its phase is molten loss of electrons, 2. Rank the oxidizing agents in order of decreasing strength. 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 each reaction as spontaneous or non-spontaneous. In an electrolytic cell, reduction occurs at the, 2. 6. HCl & Mg spontaneous. H2 + 2OH- -0.41 v Anode: Balance each of the 19. 2H+ What is the oxidation number of carbon in NaHCO3? Worksheets: General Chemistry (Guided Inquiry) ... Know the systematic procedure for balancing redox reactions by the ion-electron method; Success Criteria. AsO. 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. reduced Cr6+. Fe + - an electrode that is the site of oxidation, - an electrode that is the site of reduction, - a reaction that occurs naturally and has a positive Can you keep 1 M HCl in an iron container. the, 5. 12c. )�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. WS 8 4, 12. This is best shown by working an example. WS 9 5, 13. 1e- -------> Ag, Overall Reduction - as spontaneous or non-spontaneous. A. NH3 B. N2 C. NO2 D. N2O 2. 2e- Cathode reaction: Ag+ + voltage. 2e- -------> Zn x 2 Cr 2 O 7 - → Cr3+ 5. 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