MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced) i. Write the reduction and oxidation half-reactions (without electrons). (.5 point) ii. Balance the equations for atoms (except O and H). (.5 point) iii. Balance the equations for atoms O and H using

46,081 results
  1. chemistry

    MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced) i. Write the reduction and oxidation half-reactions (without electrons). (.5 point) ii. Balance the equations for atoms (except O and H). (.5 point) iii. Balance the equations for atoms O and H using H2O

  2. chemistry

    2. What is the reduction half-reaction for the following unbalanced redox equation? Cr2O72– + NH4+ Cr2O3 + N2 A.) Cr2O3 -> Cr2O7^2– *B.) Cr2O72– -> Cr2O3 C.) NH4+ -> N2 D.) N2 -> NH4+ 3. Which oxidation-reduction reactions are best balanced by the

  3. chemistry

    Consider the following half-reactions: MnO4- + 8H+ + 5e- --> Mn2+ + 4H2O NO3- + 4H+ + 3e- --> NO + 2H2O Predict whether NO3- ions will oxidize Mn2+ to MnO4- under standard-state conditions.

  4. Balance each of the following redox reactions occu

    Balance each of the following redox reactions occurring in acidic solution a) SO32- (s) +MNO4- ---> SO42- +Mn2+ b) S2O32-+ Cl2 ---> SO42-+Cl-

  5. Chemistry

    Identify the oxidation-reduction reactions among the following: 1. Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) 2. 2Na(s) + Cl2(aq) → 2NaCl(s) 3. 2Mg(s) + O2(g) → 2MgO 1 and 2 only 2 and 3 only 1 and 3 only All of 1, 2, and 3 None of 1, 2, and 3

  6. chem

    Balance the following oxidation-reduction reaction in acid solution: SO32- + MnO4- --> SO42- + Mn2+ + H2O

  7. chemistry

    A voltaic cell is contructed in which a copper wire is placed in a 1.0 M Cu(NO3)2 solution and a strip of gold i placed in a 1.0 M AuNO3 solution. The measured potential of the cell is found to be 1.36V and the copper electrode is negative. The Ered for

  8. Gen Chem

    What is n, the number of moles of electrons transferred, in the following reaction? 2 MnO4-(aq) + 16 H+(aq) + 10 Cl-(aq) ===> 2 Mn2+(aq) + 5 Cl2(g) + 8 H2O(l).

  9. chemistry

    "Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of the following aqueous solution: CuBr2(aq)" Possible oxidation reactions: 1. 2Br- -> Br2 + 2e- = -1.09 2. 2H2O -> O2 + 4H+ + 4e- = -1.23 Possible reduction

  10. Chemistry - Please check

    d) 2Al(s) + Fe2O3(s)  2Fe(l) + Al2O3(s) Oxidation 2Al(s)  2Al+ + 2e- Reduction Fe23+ + 3e-  2Fe(l) Oxidation numbers for chlorine HCl = -1 MnO2(s)= +4 KMnO4(s)= +7 Oxidation numbers for manganese Mn(s)= ? MnCl2(s)= +7 Mn2+(aq)= ? MnO4- =? And then

  11. Chemistry

    3. Which oxidation-reduction reactions are best balanced by the half-reaction method? A.) covalent reactions *B.)acid-base reactions C.) ionic reactions D.) intermolecular reactions Thank you.

  12. Chemistry

    Dr.Bobb222 please help balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (a)

  13. chemistry- electrochemical cell

    What makes this an oxidation-reaction? 3Ag2S+2Al(s) -> Al2S3+6 Ag(s)? Write the half-reactions showing the oxidation and reduction reactions. Identify which is the oxidation reaction and which is the reduction reason. What is oxidized in the reaction? What

  14. Chemistry HELP PLEASE!!

    write the oxidation and reduction half-reactions that occur at the anode and cathode, respectively, when MgCl2 liquid is electrolyzed using inert electrodes. HELP PLEASE!!!

  15. Chemistry

    MnO4– + SO32– + H2O → MnO2 + SO42– + OH– If the reaction occurs in an acidic solution where water and H+ ions are added to the half-reactions to balance the overall reaction, how many electrons are transferred in the balanced reduction

  16. chemistry

    Use the following pair of reduction half-reactions to design a galvanic cell. Then write in the proper coefficient for each of the species involved in the overall reaction. Water molecules and protons are not shown in the half-reactions, but may be needed

  17. Chemistry

    Using the standard reduction potentials, calculate the equilibrium constant for each of the following reactions at 298 K. 10Br- + 2MnO4- + 16H+ -> 2Mn2+ + 8H20 + 5Br2 Work: 2Br- -> Br2 + 2e- (This would be multiplied by 5 to balance out with the upper

  18. chemistry

    Mg + Au+ -> Mg2+ + Au what is the oxidation and reduction half reactions

  19. chemistry

    Balance following oxidation reduction reactions using oxidation states method? a) Cl2(g) + Al(s) --> Al3+(aq) + Cl- b.) O2(g) + H2O(l) + Pb(s) --> Pb(OH)2(s) c) H+(aq) + MnO4-(aq) + Fe2+(aq) --> Mn2+(aq) + Fe3+(aq) + H2O(l)

  20. balanced equation

    ? MnO4– + ?H+ + ?C2O42– --> ?Mn2+ + ?H2O + ?CO2 what's the balanced equation? correct coefficients? is it 1MnO4- + 2H+ + 1C2O42- --> 1Mn2+ + 1H20 + 2CO2 ? c2042..? are you missing parenthesis somewhere? oh i see, no i believe this is correct: MnO4- +

  21. Chemistry

    For the following electrochemical cell: Fe(s) / Fe2+(aq) // MnO4–(aq) Mn2+(aq) / Pt(s) Which letter corresponds to the correct balanced chemical equation in an acidic solution? A. 5Fe(s) + 16H+(aq) + 2MnO4–(aq)--> 2Mn2+(aq) + 8H2O(l) + 5Fe2+(aq) B.

  22. Chemistry

    Balance the following equations for a half reaction that occurs in a acidic solution A) ClO3- --> Cl2 B)H2BO3- -->BH4- C) MnO4- + HNO2 -->NO3- +Mn2+

  23. CHEMISTRY

    I haven't learned half reactions for oxidation and reduction so please teach me by leading me from step to step.... I don't get this.. Sn2+ +2Fe3+---> Sn4+ +2Fe2+ The answer key says Oxidation: Sn2+--->Sn4+ +2e- Reduction: 2Fe3+ + 2e----->2Fe2+ **where did

  24. chemistry- redox

    Complete and balance the following equations using the method of half-reaction. both reactions happen in acidic solutions: a. Cu(s) + NO3-(aq)--> Cu2+(aq) + NO2(aq) b. Mn2+(aQ) + NaBiO3(s)--> Bi3+(aq) + MnO4-(aq) I'm having trouble getting the half-rxn

  25. Chemistry

    Electron Transfer Theory Write an label the oxidation and reduction half-reaction equations. a) Ni(s) + Cu(NO3)2(aq) -> Cu(s)+ Ni(No3)2(aq) oxidation - Ni(s) -> Ni2+(aq) + 2e- reduction - Cu2+(aq) + 2e- -> Cu(s) b) Pb(s) + Cu(NO3)2(aq) -> Cu(s) +

  26. Chem (electron transfer)

    KMnO4 + HCl → MnCl2 + Cl2 + H2O + KCl If the reaction occurs in an acidic solution where water and H+ ions are added to the half-reactions to balance the overall reaction, how many electrons are transferred in the balanced reduction half-reaction? The

  27. Chemistry

    Identify the oxidation-reduction reactions among the following: 1. Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) 2. 2Na(s) + Cl2(aq) → 2NaCl(s) 3. 2Mg(s) + O2(g) → 2MgO Identify the oxidation-reduction reactions among the following: 1 and 2 only 2 and 3 only 1

  28. Chemistry

    What is the reduction half-reaction for the reaction between iron(II) sulfate and potassium permanganate in a sulfuric acid solution? 5Fe2+(aq) + MnO4–(aq) + 8H+(aq) --> 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) a. MnO4– + 3e– --> Mn2+(aq) + 4H2O b. MnO4–(aq)

  29. Chemistry (electron transfer)

    MnO4^– + SO3^2– + H2O → MnO2 + SO4^2– + OH^– If the reaction occurs in an acidic solution where water and H+ ions are added to the half-reactions to balance the overall reaction, how many electrons are transferred in the balanced reduction

  30. ap chemistry

    Write the half reactions and the balanced equation for the galvanic cell Hg(ℓ)|Hg2+2(aq)||MnO4(aq),Mn2+(aq),H+(aq)|Pt(s). What is the smallest possible integer coefficient of H2O(ℓ) in the combined balanced equation?

  31. Chemistry

    For the following electrochemical cell: Fe(s) / Fe2+(aq) // MnO4–(aq) Mn2+(aq) / Pt(s) Which letter corresponds to the correct balanced chemical equation in an acidic solution? A. 5Fe(s) + 16H+(aq) + 2MnO4–(aq)--> 2Mn2+(aq) + 8H2O(l) + 5Fe2+(aq) B.

  32. Chemistry

    Design an electrochemical cell using Pb(s) and Mn(s) and their solutions to answer the following questions. I just want to see if my answers are correct. I drew the cell already. Thanks 1. Give the line notation for this electrochemical cell. Mn(s) ∣

  33. Chemistry

    CONSIDER THE FOLLLOWING UNBALANCED REDOX EQUATION: IO3^-(AQ) + Al(S)-->I2(S) + A;^3+(AQ) A. WHAT IS THE OXDATION NUMBER OF IODINE IN THE IODATE ION? I GOT IO3^6(AQ)? B. WHICH SPECIES IS THE REDUCING AGENT I GOT AL^3+(AQ) C. USING THE OXIDATION AND

  34. chemistry-balanced redox equations

    Use the following steps to balance the redox reaction below: Mg + Au+ Mg2+ + Au a. Write the oxidation and reduction half-reactions. Make sure each half-reaction is balanced for number of atoms and charge b. Multiply each half-reaction by the correct

  35. Chemistry

    4, Assign oxidation states for the two elements in the compound OF2. Explain the rules that you use. 5. For each of the following oxidation-reduction reactions of metals and nonmetals, identify the element that is oxidized and the element that is being

  36. AP Chemistry

    2 Al + 3 Cu(NO3)2 --> 2 Al(NO3)3 + 3 Cu 1. Write balanced equations for the oxidation and reduction half-reactions. Identify each half-reaction as oxidation or reduction. 2. In the balanced overall reaction, determine which is the oxidation and reduction

  37. Chemistry -Please Help

    2. What is the reduction half-reaction for the following unbalanced redox equation? Cr2O7^2– + NH4^+ Cr2O3 + N2 A.) Cr2O3 -> Cr2O7^2– B.) Cr2O7^2– -> Cr2O3 C.) NH4^+ -> N2 D.) N2 -> NH4^+ I think it is B...? 3. Which oxidation-reduction reactions are

  38. Chemistry

    For the following electrochemical cell: Fe(s) | Fe2+(aq) || MnO4–(aq), Mn2+(aq) | Pt(s) Which letter corresponds to the correct balanced chemical equation in an acidic solution? A. 2Mn2+(aq) + 8H2O(l) + 5Fe2+(aq)-> 5Fe(s) + 16H+(aq) + 2MnO4–(aq) B.

  39. biochemistry

    The phenomenon of coupling always involves ? oxidation and reduction reactions decarboxylation reactions reactions that produce energy and related reactions that require energy esterification and oxidation reactions None of the above

  40. chemistry

    MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced) i. Write the reduction and oxidation half-reactions (without electrons). (.5 point) ii. Balance the equations for atoms (except O and H). (.5 point) iii. Balance the equations for atoms O and H using H2O

  41. Chemistry

    write unbalanced oxidation and reduction reactions for the following processes: Mn³⁺(aq) → MnO₂(s) + Mn²⁺(aq)

  42. Electrochem

    I have a table of standard potentials in water that gives a number of reactions and their e*reduction. Say I'm looking for the reaction Al(s) --> Al+3 + 3e-, but the book gives me the reaction Al+3 + 3e- --> Al(s) and a E*red value of -1.68. If this were

  43. Chemistry

    separate this redox reaction into its component half-reactions. O2 + 4Cu-->2CuO Oxidation half-reaction: ? Reduction half-reaction: ? I believe that the Oxidation is copper and that reduction is oxygen. So I tried to write it as 4Cu^+ --> 4Cu + 4e^- O2^2-

  44. chemistry

    1)The reaction of methane and oxygen yields carbon dioxide gas and water. The unbalanced reaction is as follows: CH4(g) + O2(g)CO2(g) + H2O(g) A. If 0.718 grams of methane are reacted, how many grams of water vapor are produced? B. If 1.621 grams CO2 are

  45. General Chemistry

    Balance the following redox reaction in acidic and basic solutions: Fe(OH)2(s) + O2(g) --> Fe(OH)3(s) These are the steps my instructor gave us to balance redox reactions: 1. Divide into 1/2 rxns (reduction & oxidation) 2. Balance atoms other than H & O 3.

  46. Chemistry

    For the following electrochemical cell: Fe(s)/Fe2+(aq)//MnO4–(aq), Mn2+(aq)/ Pt(s) Which letter corresponds to the correct balanced chemical equation in an acidic solution? A. 2Mn2+(aq) + 8H2O(l) + 5Fe2+ ==> (aq)5Fe(s) + 16H+(aq) + 2MnO4–(aq) B. 5Fe(s)

  47. Chem -plz check work

    so i've worked on this some more, now I am asking if someone will plz check my work 2 half cells in a galvanic cell consist of one iron Fe(s) electorde in a solution of iron (II) sulphate FeSO4(aq)and a silver Ag(s) electrode in a silver nitrate solution,

  48. AP Chemistry

    Sodium can be extracted by heating naturally occurring salt until it is molten. An electrochemical process is then used to extract the sodium. Cl2 is produced at the anode, and Na is collected at the cathode. 1. Write the half-reactions that occur at the

  49. Chemistry

    Balancing Complete Redox Reactions I need help on the half reduction part for both reduction and oxidation of Cl2(g) --> cl^1- (aq) + OCl^1- (aq). I got both of the half reactions started. Cl2 --> Cl^- (Reduction) .... Cl^1- (aq) + OCl^1- (aq) (Oxidation)

  50. CHEM 1A

    Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) Br ‾(aq) + MnO4‾(aq) →

  51. chem 1A

    Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) Mn2+(aq) + NaBiO3(s) →

  52. Chemistry

    What is the reduction half-reaction for the reaction between iron(II) sulfate and potassium permanganate in a sulfuric acid solution? 5Fe2+(aq) + MnO4–(aq) + 8H+(aq) --> 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) a. MnO4– + 3e– -->Mn2+(aq) + 4H2O b. MnO4–(aq)

  53. analytical chemistry

    Write balanced net-ionic equations to describe: a. The oxidation of Mn2+ to MnO4- by ammonium peroxydisulfate [(NH4)2S2O8] b. The air-oxidation of HAsO32- to HAsO42- c. The oxidation of Ce3+ to Ce4+ by sodium bismuthate (NaBiO3) Write balanced net-ionic

  54. science 20-1

    state whether oxidation or reduction will occur, determine the number of electrons gained or lost, and write a balanced half-reaction. a. Sn4+(aq) →Sn2+(aq) oxidation, 2 electrons lost b. Na+(aq) →Na(s) reduction, no electrons lost c. S(s) →S2-(aq)

  55. Chemistry

    CHCl3 + MnO4- = Cl2 + CO2 + Mn+2 Balance the above with half reactions in acidic medium. For the above reaction, can you please show the half reactions...which is getting oxidised...both C and Cl's oxidation # are changing showing both getting

  56. Chemistry

    Using the change in oxidation number method, balance the redox reaction shown below. (NO2^2)+ (MnO4^-)---> (NO3^-)+ Mn^2+ Divide into half reactions. I will show you how to do MnO4^- and you do the other one. MnO4^- ==> Mn^+2 Step 2. Determine the

  57. Chemistry

    Which of the following is true about oxidation reactions? A. Oxidation reactions are the principal source of energy on Earth. B. All oxidation reactions are accompanied by reduction reactions. C. The burning of wood in a fireplace and the metabolization of

  58. chemistry

    Use the following steps to balance the redox reaction below: Mg + Au+ Mg2+ + Au -Write the oxidation and reduction half-reactions. Make sure each half-reaction is balanced for number of atoms and charge. -Multiply each half-reaction by the correct number,

  59. Chemistry

    Electron Transfer Theory Write an label the oxidation and reduction half-reaction equations. a) Ni(s) + Cu(NO3)2(aq) -> Cu(s)+ Ni(No3)2(aq) oxidation - Ni(s) -> Ni2+(aq) + 2e- reduction - Cu2+(aq) + 2e- -> Cu(s) b) Pb(s) + Cu(NO3)2(aq) -> Cu(s) +

  60. Soil Chemistry

    In saturated soils, oxygen is quickly depleted and microbes must utilize the next most favorable electron acceptor, in this case sulfate (SO42-). Under these conditions, Mn (and Fe) are oxidized to Mn2+ (and Fe2+). Select the correct oxidation and

  61. chemistry grade 12

    Question: Balance the following reactions by the oxidation number method. a) I2 + HNO3 --> HIO3 + NO2 + H2O b) MnO4- + H+ + Cl- --> Mn2+ + Cl2 + H2O I know how to give each atom oxidation number but after i don't know how to apply the method.

  62. chemistry grade 12

    Thanks DrBob222 for previous answers. Question: Balance the following reactions by the oxidation number method. a) I2 + HNO3 --> HIO3 + NO2 + H2O b) MnO4- + H+ + Cl- --> Mn2+ + Cl2 + H2O

  63. Chemistry

    Can someone help me balance this equation? MnO4(¨C) + H(+) + C2O4(2¨C)--> Mn(2+) + H2O + CO2 Sure but tell us what you don't understand about it. You need to learn how to do them yourself. Tell me what you don't understand, in detail, and I can help you

  64. chemistry(check my asnwer)

    Why doesn't potassium ion K+ from KMnO4 appear in the following two unbalanced equations: MnO4– + C2O42– Mn2+ + CO2 MnO4– + Fe2+ Mn2+ + Fe3+ ? A. KMnO4 is not added to either reaction. B. The presence of K+ would result in a net positive charge in

  65. chemistry

    Why doesn't potassium ion K+ from KMnO4 appear in the following two unbalanced equations: MnO4– + C2O42– Mn2+ + CO2 MnO4– + Fe2+ Mn2+ + Fe3+ ? A. The presence of K+ would result in a net positive charge in the products. B. The equations cannot be

  66. chemistry

    Why doesn't potassium ion K+ from KMnO4 appear in the following two unbalanced equations: MnO4– + C2O42– Mn2+ + CO2 MnO4– + Fe2+ Mn2+ + Fe3+ ? A. KMnO4 is not added to either reaction. B. The presence of K+ would result in a net positive charge in

  67. Chemistry

    Why doesn't potassium ion K+ from KMnO4 appear in the following two unbalanced equations: MnO4– + C2O42– Mn2+ + CO2 MnO4– + Fe2+ Mn2+ + Fe3+ ? A. KMnO4 is not added to either reaction. B. K+ is a spectator ion and redox reactions are written as net

  68. Chemistry

    Write half-reactions for the oxidation and reduction processes for the following: Sn2+ + IO3- -> Sn4+ + I- (acidic solution) MN2+ + H2O2 -> MnO2 + H2O (basic solution)

  69. Chemistry

    I'm confused with this question as I don't understand how to write the reactions. Here is the question if you could please help me with this question or just even give me an example on how to do it. I would really appreciate it. Thank you. Write the

  70. Science (Chemistry)

    The question: Balance each of the following skeletal equations by using oxidation and reduction half reactions. All the reactions take place in acidic solution. Identify the oxidizing agent and reducing agent in each reaction. a) Cl[sub]2[/sub] (g) +

  71. Chemistry

    I am having trouble with the balancing the oxidation-reduction equations that are in a basic solution. This is the first one that I'm doing that's in a basic solution, and I can't get it! I get everything right except I get 2H2O instead of one on the left.

  72. Chemistry

    Using half reactions, write the equation for MnO4- reacting with H2O2 in acid solution to give Mn2+ and O2

  73. Chem

    Write a balanced equation for the following reduction-oxidation reaction. SO3–2 + MnO4–SO42– + Mn2+ __SO32–(aq) + ___MnO4–(aq) + ___H+(aq)--> ___SO42–(aq) + ___Mn2+(aq) + ___H2O(l) I have no idea how to do this type of problem, care to explain?

  74. chemistry

    write the oxidation and reduction half reactions for mg+au^+---->mg^2^++au

  75. chem1A

    Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) (b) Cr2O72-(aq) + Cl ‾(aq)

  76. Chemistry

    I'm supposed to balance a redox reaction that occurs in an acidic solution. I already balanced it(h**p://img148.imageshack.us/img148/4304/redoxht8.jpg), but how do I tell if a half-reaction is oxidation or reduction? I know an oxidation reaction loses

  77. Chemistry

    Why doesn't potassium ion K+ from KMnO4 appear in the following two unbalanced equations: MnO4– + C2O42– Mn2+ + CO2 MnO4– + Fe2+ Mn2+ + Fe3+ ? The potassium ion is a spectator ion. You have written ionic equations (but omitted the arrows to separate

  78. Electroplating in Chem

    Today I began an electroplating lab between a copper strip and a coin in electrolyte solution with a battery. I am struggling to figure out the copper half-reactions that occured, and whether they are reduction or oxidation. I only need two, and one is

  79. Chem

    For the following electrochemical cell: Fe(s) Fe2+(aq) MnO4–(aq) Mn2+(aq) Pt(s) Which letter corresponds to the correct balanced chemical equation in an acidic solution? A. Fe(s) + 8H+(aq) + MnO4–(aq)Mn2+(aq) + 4H2O(l) + Fe2+(aq) B. 5Fe(s) + 16H+(aq) +

  80. Chem

    For the following electrochemical cell: Fe(s) Fe2+(aq) MnO4–(aq) Mn2+(aq) Pt(s) Which letter corresponds to the correct balanced chemical equation in an acidic solution? A. Fe(s) + 8H+(aq) + MnO4–(aq)Mn2+(aq) + 4H2O(l) + Fe2+(aq) B. 5Fe(s) + 16H+(aq) +

  81. chemistry

    In many residential water systems, the aqueous Fe3+ concentration is high enough to stain sinks and turn drinking water light brown. The iron content is analyzed by first reducing the Fe3+ to Fe2+ and then titrating with MnO4- in acidic solution. Fe2+(aq)

  82. Chemistry

    1. Tube # 3: (a) It started out as purple, and turned into green. (b) No precipitate was noticably formed. Tube #4: (a) This tube was purple, and turned into white. (b) A brown precipitate was formed after adding 1 mL of NaHSO3. Tube #5: (a) This tube was

  83. Chemistry question

    This is a hard one. I'll do my best to try and translate =) A sour liquid mixture (many H+) contains Fe2+ ions and is being titrated with 0,0202M MnO4-. At the end of the titration, the amount of MnO4- that had been used up was 20cm3. How much was the mass

  84. chemistry

    what is the oxidation half reaction, reduction half reaction, and the complete balanced reaction of the following? (a) Al(s) + MnO4‾(aq) → MnO2(s) + Al(OH)4‾(aq) (b) Cl2(g) → Cl ‾(aq) + ClO ‾(aq) (c) NO2‾(aq) + Al(s) → NH3(g) + AlO2‾(aq)

  85. Chemistry

    Balancing Complete Redox Reactions I need help on the half reduction part for both reduction and oxidation of Cl2(g) --> cl^1- (aq) + OCl^1- (aq). I got both of the half reactions started. Cl2 --> Cl^- (Reduction) .... Cl^1- (aq) + OCl^1- (aq) (Oxidation).

  86. chemistry

    Using the half-reaction method, balance the redox reaction below. Show your work; partial credit will be given. I- + Br2 → IO3- + Br- Write the reduction and oxidation half-reactions. Balance them for atoms. Balance each of the half-reactions for charge.

  87. chemistry Dr BOB

    In many residential water systems, the aqueous Fe3+ concentration is high enough to stain sinks and turn drinking water light brown. The iron content is analyzed by first reducing the Fe3+ to Fe2+ and then titrating with MnO4- in acidic solution. Fe2+(aq)

  88. Chemistry

    I need chemistry help. I think 1. c, 2.b, & 3.a (please tell me why or why not and help me set up the problems if possible) 1.) The following half reaction has been balanced except for the electrons. How many and where should the electrons be included? 14

  89. Chemistry

    2. What is the reduction half-reaction for the following unbalanced redox equation? Cr2O72– + NH4+ Cr2O3 + N2 A.) Cr2O3 -> Cr2O7^2– *B.) Cr2O72– -> Cr2O3 C.) NH4+ -> N2 D.) N2 -> NH4+ 3. Which oxidation-reduction reactions are best balanced by the

  90. Chemistry: check answers

    Please check. Thank you. 2. What is the reduction half-reaction for the following unbalanced redox equation? Cr2O72– + NH4+ Cr2O3 + N2 A.) Cr2O3 -> Cr2O72– B.) Cr2O72– -> Cr2O3 C.) NH4+ -> N2 D.) N2 -> NH4+ 3. Which oxidation-reduction reactions are

  91. Chemistry

    Dr. Bob222 I still didn't understand which is the reduction half reaction and its products and oxidation half reaction...and why is it O3 to IO3-...0 to -6 and then Please help...entrance exam soon Write the oxidation and reduction half reactions(showing

  92. Chemistry Dr. BOB

    In many residential water systems, the aqueous Fe3+ concentration is high enough to stain sinks and turn drinking water light brown. The iron content is analyzed by first reducing the Fe3+ to Fe2+ and then titrating with MnO4- in acidic solution. Fe2+(aq)

  93. Chemistry

    Can you please help me write the oxidation and reduction half reactions represented in each of these redox equations, and help me write the half reactions in net ionic form if they occur in aqueous solution. 1) PbO(s) + NH3(g) --> N2(g) + H2O(l) + Pb(s) 2)

  94. chemistry

    Balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. (a) H2O2(l) + Pb(s) → H2O(l) + Pb2+(aq) (b) O2(g) + Mn(s) → H2O(l) + Mn2+(aq)

  95. Science

    sodium can be extracted by heating naturally occuring salt until it is molten. an electrochemical process is then used to extract the sodium. cl2 is produces at the anode and Na is collected at the cathode. write the half-reactions that occur at the anode

  96. AP Chemistry

    Sodium can be extracted by heating naturally occurring salt until it is molten. An electrochemical process is then used to extract the sodium. Cl2 is produced at the anode, and Na is collected at the cathode. Write the half-reactions that occur at the

  97. Chemistry

    1. Sodium can be extracted by heating naturally occurring salt until it is molten. An electrochemical process is then used to extract the sodium. Cl2 is produced at the anode, and Na is collected at the cathode. A standard reduction potential graph for the

  98. Chemistry

    Please help...entrance exam soon Write the oxidation and reduction half reactions(showing e- lost or gained) for the foll O3 + I- -> IO3- + O2 (acidic)

  99. chemistry

    Why are half-reactions used in redox reactions? A. They make it easier to keep track of spectator ions in the reaction. B. They make it easier to see the oxidation and reduction parts of the reaction separately. C. They make it possible to neglect the

  100. Chemistry

    Write the oxidation and reduction half-reactions for a silver-chromium voltaic cell. (Use the lowest possible coefficients. Include states-of-matter at 1 atm and 25°C in your answer.)

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