Balance the following redox (oxidation-reduction) reaction under basic conditions. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.)
CrO42−(aq) + S2O32−(aq) → Cr3+(aq) + SO42−(aq)

  1. 👍 0
  2. 👎 0
  3. 👁 751
  1. Here us a site that tells you the details.

    I don't do them that way. Here is how I do the CrO4^-. You can add the states.
    CrO4^2- ==> Cr^3+

    Cr is +6 on left and +3 on right. Add 3e to left.
    CrO4^2- +3e ==> Cr^3+

    Count the charge on the left (-5) and right (+3); add OH^- to the right to balance the charge.
    CrO4^2- + 3e ==> Cr^3+ + 8OH^-

    Now add H2O to balance.
    CrO4^2- + 4H2O + 3e ==> Cr^3+ + 8OH^-

    1. 👍 0
    2. 👎 1

Respond to this Question

First Name

Your Response

Similar Questions

  1. science, chemistry

    Separate this redox reaction into its component half-reactions. O2+2Cu---->2CuO thought it was: Oxidation 2e-+O2---->2O(-2) Reduction Cu---->Cu(2+)-2e- but this is wrong

  2. Chemistry

    Write a balanced equation for the reaction that occurs in each of the following cases. (Use the lowest possible coefficients. Include states-of-matter under SATP conditions in your answer.) I think have the reactions, but I'm

  3. 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)

  4. Chem 1

    Use oxidation states to identify the element that is being oxidized in the following redox reaction: Cu(s)+2 H 2 S O 4 (aq) → CuS O 4 (aq)+S O 2 (g)+2 H 2 O(l)

  1. 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.

  2. Chemistry

    For a particular redox reaction NO2– is oxidized to NO3– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in basic solution. Phases are optional.

  3. Chemistry

    Consider a generic redox reaction then suppose that the coefficients in the redox reaction are doubled. How will the following quantities be affected for a voltaic cell under nonstandard conditions, will they be Doubled, Halved,

  4. Chemistry

    Complete and balance the equation for this reaction in basic solution? Redox reaction Cr is oxidized to CrO42– and Fe3 is reduced to Fe2...? For a particular redox reaction Cr is oxidized to CrO42– and Fe3 is reduced to Fe2 .

  1. 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

  2. Chemistry

    Balance the following redox reaction in basic solution. H2(g)+Fe3+(aq) ---> H2O(l)+Fe2+(aq)

  3. Chemistry

    Which of the following is an oxidation-reduction (redox) reaction? A. 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g) B. 2NaN3(g) → 2Na(g) + 3N2(g) C. 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) D. Fe(s) + Ni(NO3)2(aq) → Fe(NO3)2(aq) + Ni(s)

  4. chem

    A voltaic cell consists of a strip of cadmium metal in a solution of Cd(NO3)2 in one beaker, and in the other beaker a platinum electrode is immersed in a NaCl solution, with Cl2 gas bubbled around the electrode. A salt bridge

You can view more similar questions or ask a new question.