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    Understanding Redox Equations

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    Balance the redox equations and give the half-cell reactions and identify the oxidizing agent, species oxidized, reducing agent, and species reduced.

    In an acidic solution: CrO4^2-(aq)+ Cl-(aq)--> Cr^3+(aq) +HClO2(aq)

    In an acidic solution: Fe^2+(aq) + MnO4-(aq) --> Fe^3+(aq)+ Mn^2+(aq)

    In acidic solution: NH4+(aq) + NO3-(aq)--> N2O(g)

    In basic solution: N2H4(aq) + Cu(OH)2(s) ---> N2(g) + Cu(s)

    In basic solution: Ca(OH)2(aq)+ C(s) + ClO2(g)--> CaCO3(s) +ClO2-(aq)

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    Solution Preview

    For these questions, you have to use the EOHC technique....

    E -everything besides Oxygens and hydrogens
    O -Oxygens by adding waters
    H -Hydrogens by adding protons H+
    C -charge by adding electrons e-

    First thing to do is to split into half reactions (sometimes not so easy)
    TIP: Figure out which elements are changing oxidation state first, and try to ignore elements that are not changing in oxidation state.

    For the first question:

    Cr04^-2 --> Cr^3+ is the one half reaction to balance

    Cl^- --> HClO2 is the second half reaction to balance

    Balancing the first....
    CrO4^-2 --> Cr^3+
    Everything else is simply the Cr......already balanced
    Add 4 waters to the RHS (right hand side)

    CrO4^-2 --> Cr^3+ + 4H2O
    Add 8 protons to ...

    Solution Summary

    The solution is comprised of a detailed explanation of how to balance redox reactions, and identify oxidizing agents, reducing agents.