1. Questions

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 number, in order to balance charges for the two half-reactions.

c. Add the equations and simplify to get a balanced equation.

  1. 👍 3
  2. 👎 2
  3. 👁 540
princess

  1. You need to learn how to do these yourself. What exactly do you not understand so we can get you started on th right foot.

    1. 👍 0
    2. 👎 11
    DrBob222

  2. Mg to Mg2+ loses 2 electrons
    Au+ to Au gains one electron. So 2Au for each Mg

    Mg yields Mg+ +2e
    Au+ + e yields Au

    so multiply the second equation by 2

    1. 👍 1
    2. 👎 1
    👨‍🏫
    bobpursley

  4. hey ibis

    1. 👍 0
    2. 👎 2
    Anonymous

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Classify each of the following as a redox reaction or a non-redox reaction. Zn+CuCl2 -> ZnCl2+Cu HCl+NaOH -> H2O+NaCl 2CO+O2 -> 2CO2 SO3+H2O -> H2SO4

  2. Chemistry

    In a particular redox reaction, MnO2 is oxidized to MnO4– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in acidic solution. Phases are optional. MnO2 + Cu^2+ ---> MnO4^- + Cu^+

  3. chemistry

    Balance the redox reaction of eq. Cu2S + SO4(-2) gives CuO + SO2 (Acidic )

  4. chemistry

    Balance the following redox reaction. MnO4 (aq) + Fe (s) --> Mn2+ (aq) +Fe2+ (aq)

  1. 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

  2. Chemistry

    Calculate E, E^o and (delta)G^o for the following cell reaction: Mg(s) + Sn2+(aq) (yields) Mg2+(aq) + Sn(s) [Mg2+] = 0.045 M, [Sn2+] = 0.035 M

  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

    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.

  1. CHEM AP

    Complete and balance the following equation. MnO4^‾ (aq) + CH3OH(aq) ¨ Mn^2+(aq) + HCO2H(aq) (acidic solution) I KNOW ITS a redox, so i followed the steps and got: 4MnO4^- (aq) + 5CH3OH (aq) + 11H2O (l) + 12H^+ (aq) ¨

  2. chemisrty

    Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO3 and HI are mixed. 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g) 2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq)→ H2SO3(s) +

  3. Chemistry

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

  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 .

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