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(Use the information in the table below. Show the half reactions and the potentials for each half reaction.) Determine whether the following redox reaction is spontaneous as written. 2Al(s) + 3Zn2+(aq) → 2Al3+(aq) + 3Zn(s) Reduction Potentials at 25°C Electrode

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  1. chemistry

    Determine whether the following redox reactions are spontaneous as written? (Use the information in the table below. Show the half reactions and the potentials for each half reaction.) a. 2Ag(s) + Mg2+(aq) → 2Ag+ (aq) + Mg(s) [5 points] b. 2Al(s) +
  2. Chemistry

    (Use the information in the table below. Show the half reactions and the potentials for each half reaction.) Determine whether the following redox reaction is spontaneous as written. 2Al(s) + 3Zn2+(aq) → 2Al3+(aq) + 3Zn(s) Reduction Potentials at 25°C
  3. Chemistry

    Choose the two half-reactions from a table of standard reduction potentials that most closely approximate the reaction that occur within the battery. What is the standard voltage generated by a cell operating with these half-reactions? 2Li(s) + Ag2CrO4(s)
  4. Chemistry

    Choose the two half-reactions from a table of standard reduction potentials that most closely approximate the reaction that occur within the battery (Pacemaker). What is the standard voltage generated by a cell operating with these half-reactions? (i got
  5. Chemistry- Please help!!

    Using standard reduction potentials, calculate the standard E¡Æcell, emf, for each of the following reactions. State if each reaction is spontaneous or nonspontaneous. (Use the below reactions AS WRITTEN, DO NOT REARRANGE ANY REACTIONS.) You must show
  6. Chemistry

    Using standard reduction potentials, calculate the standard E¡Æcell, emf, for each of the following reactions. State if each reaction is spontaneous or nonspontaneous. (Use the below reactions AS WRITTEN, DO NOT REARRANGE ANY REACTIONS.) You must show
  7. Chemistry

    Using standard reduction potentials, show that one can prepare an ammine complex from CoCl2 and hydrogen peroxide in the presence of ammoinia but not in its absence. (need to write two redux reactions, calculate standard potentials for the reactions, and
  8. Chemistry-Plz see this DrBob

    I am sorry I do not know what happens the symbolism, so I just deleted the symbols. Is it works for you that deleted the symbols? Using standard reduction potentials, calculate the standard Ecell, emf, for each of the following reactions. State if each
  9. chem

    Q: Calculate ℰ° values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible
  10. 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
  11. Chemistry need help

    using standard potentials given in the appendices calculate the standard cell potentials and the equilibrium constants for the following reactions. Zn(s)+( Fe^2+(aq)) ---> (Zn^2+(aq))+ Fe(s) If anyone can show work, then I can do the rest of my homework by
  12. 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.
  13. chemistry

    Write the equation for the reaction, if any, that occurs when each of the following experiments is performed under standard conditions. a) crystals of iodine are added to an aqueous solution of potassium bromide. b) liquid bromine is added to an aqueous
  14. Chemistry

    Write the half cell reactions of the following? 1) Cu/Cu^2+(0.1M)//Ag^+(0.1M)/Ag 2) Zn/Zn^2+ (0.1M)//Cu^2+(0.1M)/Cu 3) Zn/Zn^2+(0.1M)//Ag^+(0.1M)/Ag 4) Zn/Zn(NH3)4^2+*0.5M)//Ag^+(0.1M)/Ag 5) Zn^2+(aq)+4NH3(aq) ...show more Also, around what range of
  15. Electrochemistry

    In lab, we did an experiment with electrochemical cells with solutions of ZnSO4, CuSO4, Al2(SO4)3 and MgSO4 and their respective metal electrodes. There are a couple of post-lab questions that I'm not sure about: (1) Summarize Part A with a data table
  16. 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
  17. chemistry

    Based on the half-reactions and their respective standard reduction potentials below, what is the standard cell potential for the reaction that is expected to occur? Fe3+(aq) + e- → Fe2+(aq) 0.77 V Sn4+(aq) + 2 e- → Sn2+(aq) 0.15 V Pb2+(aq) + 2 e- →
  18. Chemistry

    4. Use the information above to write net ionic equations for the two reactions that you have observed. 5. For each reaction, write the two half-reactions that make it up and calculate the overall reaction potential by adding the two half-reactions. Each
  19. 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.
  20. Chemistry

    Balancing Complete Redxo Reactions. I am not sure how I am suppose to start anything. Even the Half Reactions. BrO3^1- + Br^1- + H^1+ --> Br2 + H20. I need to know all the steps on how to do half reactions & I think I should be good.
  21. chem

    Based on the half-reactions and their respective standard reduction potentials below, what is the standard cell potential for the reaction that is expected to occur? Fe3+(aq) + e- → Fe2+(aq) 0.77 V Sn4+(aq) + 2 e- → Sn2+(aq) 0.15 V Pb2+(aq) + 2 e- →
  22. Chemistry

    On the semi - reactions below is correct to say: Li + + 1℮- => Li. Eº = -3,04V. Au 3+ + 3℮- => Au. Eº = + 1,50V. Pb 2+ + 2℮- => Pb . Eº = - 0,13V. Ag + + 1℮- => Ag. Eº = + 0,80V. a) In the semi reaction Ag, the potential fold if the number of
  23. Chemistry

    Given the following half-reactions and associated standard reduction potentials: AuBr−4(aq)+3e−→Au(s)+4Br−(aq) E∘red=−0.858V Eu3+(aq)+e−→Eu2+(aq) E∘red=−0.43V IO−(aq)+H2O(l)+2e−→I−(aq)+2OH−(aq) E∘red=+0.49V
  24. chemistry

    Calculate the standard reduction potential for the reaction: , given the half-reactions below and their corresponding standard reduction potentials:
  25. chemistry... HELP

    Equilibrium constant question!!!? Standard reduction potentials Reduction half-reaction E(V) Ag+(aq) + e- ---> Ag (s) 0.80 Cu ^2+ (aq) + 2e- ---> Cu (s) 0.34 Sn^4+(aq) + 4e- ---> Sn (s) 0.15 2 H+(aq) + 2e- ---> H2 (g) 0 Ni^2+(aq) + 2e- ---> Ni (s) -0.26
  26. Chemistry

    Given the following half-reactions and their standard reduction potentials, Ni2+ + 2e− Ni E° = -0.25 V 2H+ + 2e− H2 E° = 0.00 V Ag+ + e− Ag E° = 0.80 V a spontaneous reaction will occur between: a. Ni2+ and H2 b. H+ and Ag c. Ag+ and Ni d. Ni2+
  27. Electrochemistry

    I have an electrochem based question. I'm trying to solve for E* based on a chart in my book. I know the equation for solving this is E*= E*ox + E*red. The chart in my book gives a list of reactions and a E*red value. My teacher told us that the greater,
  28. Chemistry, electrochem

    (1) Half-reactions are written as ______ reactions with charge and mass balanced. (2) Among the ions, Cd^2+, Pb^2+ & Ca^2+, ________ has the greatest ability to reduce to its neutral metal. (3) Among the neutral metals; Pb, Ca & Cd, ________ has the least
  29. 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
  30. 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
  31. AP Chemistry

    What are the two half-reactions for the basic oxidized-reduction reaction Fe(OH)2+ H2O2 --> Fe(OH)3? If I can find out the two half-reactions, I'll be able to balance the equation myself. Thanks!
  32. Chemistry

    How many electrons are transferred when C3H7OH burns in oxygen to form carbon dioxide and water? I have no idea where to start. Do I need to do half reactions? Can I even do half reactions for this?
  33. chemistry

    How do you calculate the theoretical cell voltage? 1) Zn|Zn^+2 (1M)| Cu|Cu^+2 (1M) okay so by looking at example this example Calculate the emf (voltage) for the following reaction: Zn(s) + Fe2+ → Zn2+ + Fe(s) Write the 2 half reactions: Zn(s) → Zn2+ +
  34. 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
  35. chemistry

    balance the charge in the two half reactions by multiplying the half reactions by the correct multiplication factors
  36. 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
  37. Chemistry

    What would the two half reactions be for 2Na+1MgBr2 arrow 2NaBr + Mg? I don't know how to determine this, other than that you separate the elements for the two half reactions. My other question is that when you're translating words and you have an element
  38. Chemistry

    What are the half reactions for NH4ClO4 + Al = Al2O3 + AlCl3 + NO? I can balance it once i have the half reactions
  39. Chemistry

    What are the half reactions for NH4ClO4 + Al = Al2O3 + AlCl3 + NO? I can balance it once i have the half reactions
  40. 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,
  41. 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
  42. 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).
  43. Math

    Given table, X ; (1+x)^(1/x) -0.5. ; 4 -0.1 ; 2.8680 -0.01 ; 2.7320 -0.001; 2.7196 0.001 ; 2.7169 0.01 ; 2.7048 0.1 ; 2.5937 0 5 ; 2.25 From the table, show that lim x->infinity (1+x)^(1/x)=e. Plz someone show me the step how to show it based on the table.
  44. Math

    Given table, X (1+x)^(1/x) -0.5. 4 -0.1 2.8680 -0.01 2.7320 -0.001 2.7196 0.001 2.7169 0.01 2.7048 0.1 2.5937 0 5 2.25 From the table, show that lim x->infinity (1+x)^(1/x)=e. Plz someone show me the step how to show it based on the table. Hope u can read
  45. Science

    having wayyy tooo much trouble with this simple assignment. Is there a lab that proves that the light reactions must occur prior to the dark reactions in photosynthesis? So far, I thought of the experiment in which one plant is placed in direct sunlight
  46. Biology III

    I'm having wayyy tooo much trouble with this simple assignment. Is there a lab that proves that the light reactions must occur prior to the dark reactions in photosynthesis? So far, I thought of the experiment in which one plant is placed in direct
  47. CHEMISTRY

    The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on
  48. CHEMISTRY

    The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on
  49. CHEMISTRY

    The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on
  50. Chemistry

    From the Standard Potential Table in your general chemistry textbook: Half-reactions are written as _________ reactions with charge and mass balanced. Among the ions, Cd2+Pb2+ & Ca2+ ,__________ has the greatest ability to reduce to its neutral metal. (Use
  51. 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)
  52. 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
  53. PLEASE HELP CHEM!

    2 HgCl2 (aq) + SnCl2 (aq) --> SnCl4 (aq) + Hg2Cl2 (s) Hg2Cl2 (aq) + SnCl2 (aq) --> 2Hg (s) + SnCl4 (aq) For each reaction, write the two half-reactions that make it up and calculate the overall reaction potential by adding the two half-reactions. Each
  54. chemistry

    Using the given data, and the table of Standard Reduction Potentials, find the standard reduction potential for this half reaction: 8H^+ + BaCrO4(s) + 3e- -> Ba^2+ + Cr^3+ + 4H2O(l) given: Ksp (BaCrO4)=2.1E-10 DeltaGf* (kJ/mol): CrO4^2- (-727.75), Cr2O7^2-
  55. Chemistry

    The following equations are intepretations of the evidence from the reactions of four metals with various cation solutions. Make a table of half-reactions and arrange the four metallic ions and the hydrogen ions in order of their decreasing tendency to
  56. Science

    Generation and conduction of postsynaptic potentials and Integration of postsynaptic potentials and generation of action potentials How can these two relate to football players? Your thoughts?
  57. chemistry

    The standard reduction potentials of lithium metal and chlorine gas are as follows: (for Li, reduction potential is -3.04, for Cl it is 1.36) In a galvanic cell, the two half-reactions combine to 2Li{+](s) + Cl{-}2(g) --> 2Li{+}Cl{-}(aq) cell potential=4.4
  58. chemistry

    In a methane fuel cell, the chemical energy of the methane is converted into electrical energy instead of heat that would flow during the combustion of methane. Using the half-reactions and reduction potentials given below a) Write a net equation for the
  59. chemistry

    In a methane fuel cell, the chemical energy of the methane is converted into electrical energy instead of heat that would flow during the combustion of methane. Using the half-reactions and reduction potentials given below a) Write a net equation for the
  60. Chemistry

    Would you store a solution of zinc nitrate in an aluminum container? Use half-reactions to explain your answer. Al ==> Al^+3 + 3e Zn ==> Zn^+2 + 2e Look up the above half reactions and you will see that the Al will go into solution and the Zn+2 will come
  61. chemistry

    "Ag(s) reacts with none of the 4 (solutions of Ag^+2, Pb^+2, Cu^+2, Zn^+2}. So Ag(s) goes at the bottom of the table for now although there may be some metals below silver when you finish with the entire table. Cu(s) reacts with (Ag^+ solution) so Cu goes
  62. Chemistry

    In certain first order reactions the concentration of the reactant decreases from 0.15 M to 0.11 M in 36 minutes . calculate the time of half reactions
  63. Chemistry

    I need to balance this equation by redox reactions with half reactions method NH4ClO4 + Al --> Al2O3 + AlCl3 + NO
  64. Chemistry

    Help please!!! Complete the two reduction half reactions for the cell shown at the right, and show the line notation for the cell by dragging labels to the correct position. (The electrode on the left is the anode, and the one on the right is the cathode.)
  65. Chemistry

    Uranium-238 has half life of 4.51 * 10^9 years Uranium-234 has half life of 2.48 * 10^5 years Thorium-230 has half life of 8.0 * 10^4 years Radium-226 has half life of 1.62 * 10^3 years Lead-210 has half life of 20.4 years. The rate constant for the decay
  66. chemistry

    I posted this question last night but did not get an answer- I am posting again because I have an exam I am studying for and do not understand this concept! Thanks! Using the given data, and the table of Standard Reduction Potentials, find the standard
  67. 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
  68. chemistry

    Why are half-reactions written to describe redox reactions?
  69. Chemistry

    Answer these questions about NaCl also known as table salt: 1. What is the name of the compound? 2.Are there any other names that it is known by? If yes, then please list them. 3.What is the chemical formula of the compound? Is it an ionic or covalent
  70. chemistry

    (AAAAA)The standard reduction potentials of lithium metal and chlorine gas are as follows: (for Li, reduction potential is -3.04, for Cl it is 1.36) In a galvanic cell, the two half-reactions combine to 2Li{+](s) + Cl{-}2(g) --> 2Li{+}Cl{-}(aq) Calculate
  71. Chemistry

    Okay, so i've got 8 reactions i am supposed to balance "according to the half-reaction method". Only problem is, i was gone for the lesson, and my borrowed notes look like an entirely different language! So if you could please show me the steps and explain
  72. 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
  73. chemistry

    3. For the reaction between Cu and Sn the potentials are given below; Cu2+(aq) +2e- -----------> Cu(s) Eºcathode = 0.34 (half-cell potential) Sn(s) -----------> Sn2+(aq) + 2 e- Eºanode = - 0.14 (half-cell potential)
  74. college

    HIO3 + FeI2 + HCl --> FeCl3 + ICl (in acidic solution) Show and label the two balanced half-reactions (oxidation and reduction). Add H2Os, H+s or OH-s as needed.
  75. AP CHEM

    HIO3 + FeI2 + HCl --> FeCl3 + ICl (in acidic solution) Show and label the two balanced half-reactions (oxidation and reduction). Add H2Os, H+s or OH-s as needed.
  76. Chemistry

    Please write down the redox reactions (using the half-reaction method!) a)Cl2 from OCl- and Cl- in acidic solution b)Br2 from BrO3- and Br- in acidic solution -You don't have to do both, but could you help me step up the half reactions especially for OCl-
  77. Chemistry

    Explain with values and reactions from standard reduction potentials tables why neither gold (I) nor gold (III) not to mention the base metal itself, tarnishes (that is can be oxidized by exposure to air)
  78. math

    The distance remaining for a half marathon race over several minutes is shown in table. Use the information to determine the constant rate change in the minutes per mile. Table: Time (min) Distance Remaining (mi) 40 8 56 6 72 4 88 2
  79. Chemistry

    Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+(aq) solution
  80. Chemistry

    1) Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+(aq) solution
  81. Chemistry ASAP

    Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+ (aq) solution
  82. chemistry

    Lab: Creating a Redox Table Purpose: The purpose of this lab exercise is to construct a table of relative strengths of oxidizing and reducing agents. By completing this exercise, you will see how more extensive tables of relative strengths of oxidizing and
  83. Chemistry

    This question is really making me upset i just can't get the answer right. i've tried so many times. If someone could help it would be muchly appeciated! Experiments were performed with four metals and solutions of their ions: A-A, B-B2+, C-C2+, D-D2+. the
  84. physics

    1. A 450 gram piece of iron is heated from 22 °C to 87 °C. Use this information to complete the following table. Show your work below the table – be sure to include units! Note: The specific heat of iron (Fe) is 0.449 J g^−1 °C^−1 Find the T
  85. chemistry

    The normal boiling point of ethanol is 78.5C. Using the following information: delta H formation (C2H5OH (g))= -234.38 kJ/mol determine the enthalpy of vaporization of ethanol. I know it should be around 39.3 according to a table in my textbook, however, I
  86. chemistry 2

    A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb2+ half-cell. Measurement shows that thesilver electrode is positive. -Write balanced half-reactions and the overall spontaneous reaction.
  87. Chemistry

    Use the Table of Thermodynamic Data to decide which of the following reactions have K>1 at 298 K: (i) HCl(g) + NH3(g)-->NH4Cl(s) (ii) 2 Al2O3(s) + 3 Si(s)-->3 SiO2(s) + 4 Al(s) (iii) Fe(s) + H2S(g)-->FeS(s) + H2(g). Which of the products of these reactions
  88. chemistry

    the reaction of aluminum metal (Al) with oxygen (O2) forms Al2O3. What is a balanced equation for this redox reaction. What are two half reactions to show how many electrons are gained or lost by each species?
  89. intermediate technology

    You have just written a ten-page report for your supervisor. The report outlines the total sales made by your team made in the past year, sales by region, and sales by quarter. While it is important to write out the detail of each category of sales in
  90. chemistry

    if you're given a chart of half cell potentials (reduction potentials), how can you figure out which metals produce the highest voltage? For ex. Cadmium (Cd) with copper (Cu) Silver (Ag) with zinc (Zn) Lead (Pb) with zinc (Zn) would you say that pb and zn
  91. Chem

    1N2(g) reacts with H2(g) to form NH3(g), gaseous ammonia. Show balanced thermochemical equations based on both one mole and two moles of NH3(g). Determine Ho ( for both reactions using Table 6.2 (Hof). Use the summation equations. Show your
  92. AP Biology

    I'm working on a lab to show that light reactions must occur prior to dark reactions in photosynthesis. so far, i thought of the experiment involving two plants, one exposed to sunlight, the other is kept in a box. both receive the same amount of water
  93. Gen Chem

    The signs of DG, DH, and DS at 25°C are shown in the table below for three reactions. Reaction DG DH DS I - + + II - - + III - - - Which reaction or reactions should go in the REVERSE direction at high temperature?
  94. intermediate technology

    Consider the following scenario: You have just written a ten-page report for your supervisor. The report outlines the total sales made by your team made in the past year, sales by region, and sales by quarter. While it is important to write out the detail
  95. 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
  96. Math porportion

    I think I'm thinking right but not sure. Earning $4.23 for each half hour rate that i work. How much money do i earn during a given amount of time? Reprent situation using graph,table,and rule. So for table 4.23 / half hr 8.48 / 1hr 12.69/ 1hr 1/2 Am I
  97. chemistry

    3. For the reaction between Cu and Sn the potentials are given below; Cu2+(aq) +2e- -----------> Cu(s) Eºcathode = 0.34 (half-cell potential) Sn(s) -----------> Sn2+(aq) + 2 e- Eºanode = - 0.14 (half-cell potential) Calculate the E.M.F (Voltage) of the
  98. chemistry

    Zn(s)+2H+(aq)->Zn2+(aq)+H2(g) Br2(aq)+2I-(aq)->2Br-(aq)+I2(aq) Name one compound containing H+ ions and another containing I- ions, which would be suitable for these reactions. Ezplain why zinc is said to be oxidised in its reaction. Complete the half
  99. Chemistry

    Zn(s)+2H+(aq)->Zn2+(aq)+H2(g) Br2(aq)+2I-(aq)->2Br-(aq)+I2(aq) Name one compound containing H+ ions and another containing I- ions, which would be suitable for these reactions. Ezplain why zinc is said to be oxidised in its reaction. Complete the half
  100. Chemistry

    Use the method of half reactions to balance the oxidation half reaction in acid solution as well as provide the oxidized and reduced reactants. Cr2O7 {2-} (aq) + F{-} (aq) = Cr {3+} (aq) + F2(aq) Charges are in { }

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