Question

Calculate the standard EMF for an electrochemical cell comprised of nickel and zinc electrodes. Provide complete step-by-step calculations.

Answer 1

Answer:

.0223 volt.

Explanation:

ECell∘=ECathode∘−EAnode∘

=0.80−(−2.37)=3.17 volt

Cell reaction, Mg+2Ag+→2Ag+Mg2+

Ecell=ECell∘−n0.0591log[Ag+]2Mg2+

=3.17−20.0591log[1×10−3]20.2

=3.17−0.1566=3.0134 volt

when Mg2+=0.1 M

Ecell=Ecell∘−20.0591log(1×10−3)2

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Answer 2

Answer:

When exposed to moisture, steel will begin to rust fairly quickly. This creates a significant problem for items like nails that are exposed to the atmosphere. The nails can be protected by being coated with zinc metal, to make a galvanized nail. The zinc is more likely to oxidize than the iron in the steel, so it prevents rust from developing on the nail.

step by step explanation:

[tex]

[tex]3F2(g)+2Au(s)→6F−(aq)+2Au3+(aq)(23.6.5)

[tex]3F2(g)+2Au(s)→6F−(aq)+2Au3+(aq)(23.6.5) 2Li(s)+2H2O(l)→2Li+(aq)2OH−(aq)+H2(g)(23.6.6)(23.6.6)2Li(s)+2H2O(l)→2Li+(aq)2OH−(aq)+H2(g)

[tex]3F2(g)+2Au(s)→6F−(aq)+2Au3+(aq)(23.6.5)

2Li(s)+2H2O(l)→2Li+(aq)2OH−(aq)+H2(g)(23.6.6)(23.6.6)2Li(s)+2H2O(l)→2Li+(aq)2OH−(aq)+H2(g) Using the table above will allow you to predict whether reactions will occur or not. For example, nickel metal is capable of reducing copper (II) ions, but is not capable of reducing zinc ions. This is because nickel (Ni)(Ni) is below Cu2+Cu2+, but is above Zn2+Zn2+ in the table.

[tex]3F2(g)+2Au(s)→6F−(aq)+2Au3+(aq)(23.6.5) 2Li(s)+2H2O(l)→2Li+(aq)2OH−(aq)+H2(g)(23.6.6)(23.6.6)2Li(s)+2H2O(l)→2Li+(aq)2OH−(aq)+H2(g) Using the table above will allow you to predict whether reactions will occur or not. For example, nickel metal is capable of reducing copper (II) ions, but is not capable of reducing zinc ions. This is because nickel (Ni)(Ni) is below Cu2+Cu2+, but is above Zn2+Zn2+ in the table.

Explanation:

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