Chemistry

posted by .

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 overall potential should be positive in order for the reactions to occur spontaneously.


4. 2 HgCl2 (aq) + SnCl2 (aq) --> SnCl4 (aq) + Hg2Cl2 (s)
Hg2Cl2 (aq) + SnCl2 (aq) --> 2 Hg (s) + SnCl4 (aq)

5.
2 Hg(l) + 2 e⁻ --> Hg©ü©÷⁺ E₀ = -0.79 V
Sn©ù⁺ + 2 e⁻ --> Sn©÷⁺ E₀ = 0.15 V
Total: -0.64 V


Sn©÷⁺ + 2 e⁻ --> Sn©ù⁺ E₀ = -0.15 V
Hg©ü©÷⁺ + 2 e⁻ --> 2 Hg(l) E₀ = 0.79 V
Total: 0.64 V

  • Chemistry -

    This looks to be part of the answers for a problem by another person; however, without the same name I can't go back and look at the original post.
    #4 looks ok except they are molecular equation; the problem asked for net ionic equations. Also, I don't know where the equations came from; but I don't see anything wrong with what is here. I'm assuming what went before is ok.
    #5. I can't make out the funny symbols.

  • Chemistry -

    Sn2+ (aq) + 2Hg2+ (aq) + 2Cl (aq)--> Sn4+ (aq) + Hg2Cl2 (s)
    Hg2Cl2 (s) + Sn2+ (aq) --> 2Hg (I) + Sn4+ (aq) + 2Cl- (aq)

    5. Sn(2+) --> Sn(4+) + 2e- Eo = -0.15 V
    2e+ + 2Hg(2+) + 2Cl --> Hg2Cl2 Eo = 0.85 V
    Total: 0.75 V

    Hg2Cl2 + 2e- --> 2Hg(2+) + 2Cl- Eo= 0.27 V
    Sn(2+) + 2 e? --> Sn(4+) Eo = -0.15 V
    Total: .12 V

  • Chemistry -

    Those are different from the original post, I am trying to work on it!

  • Chemistry -

    #4.Sn2+ (aq) + 2Hg2+ (aq) + 2Cl (aq)--> Sn4+ (aq) + Hg2Cl2 (s)
    I think 2Hg2+ should be 2HgCl2 for the complete rxn of
    Sn^2+ 2HgCl2 ==> Hg2Cl2(s) + Sn^4+ + 2Cl^-
    What you wrote has Sn being oxidized but Hg doesn't change.; i.e., it's one on the left and one on the right.


    Hg2Cl2 (s) + Sn2+ (aq) --> 2Hg (I) + Sn4+ (aq) + 2Cl- (aq)
    This part looks ok.

  • Chemistry -

    #5. You need to redo the Hg one as a result of my comments above.
    For Sn you want
    Sn ^2+ ==> Sn^4+ + 2e Eo = -0.15. Written this way it is an oxidation potential.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    The Hydrolysis Reactions - Write net-ionic equations for the reaction of each salt with water below. If there is no reaction, write N.R. 1. NH4C2H3O2 2. NH4Cl 3. NaCl 4. Na2CO3 5. NaC2H3O2 6. NaHSO4 7. FeCl3 8. NaH2PO4 9. NaHCO3
  2. 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 …
  3. 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 …
  4. Chemistry

    Questions: 1. In each test tube, a precipitate formed upon DROPWISE addition of the second reagent (steps 5 and 6). What are these precipitates?
  5. Chemistry PLEASE HELP!!

    Questions: 1. In each test tube, a precipitate formed upon DROPWISE addition of the second reagent (steps 5 and 6). What are these precipitates?
  6. 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 …
  7. 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 …
  8. Chemistry

    3. Which oxidation-reduction reactions are best balanced by the half-reaction method?
  9. 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, …
  10. 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) --> …

More Similar Questions