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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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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.

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Redox Reactions in Everyday Life

Think about an example of a redox reaction and an acid-base reaction in our everyday lives. Give your examples and discuss why you think it's important for all of us to understand this chemistry and why it's not just important to chemistry and why it's not just important to chemists.
(Please don't use the iron and rust example.)

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