Oxidation

[Hye]

The following equations are not balanced.
i   Identify the species that has been reduced and the species that has been oxidised.
ii   Write balanced half equations for the oxidation and reduction reactions.
iii   Combine the half equations to write a balanced equation.

NO3–(aq) + H+(aq) + Cu(s) -> NO(g) + H2O(l) + Cu2+(aq)

For i) the answer is NO3– is reduced to NO and Cu is oxidised to Cu2+

I don't get why NO  with Cu is oxidised to Cu2+ ??

Thanks

[Potter]

The reason of why NO is reduced is due to the reduction potentials. Have a look at the table.
Though, this seems like a very unlikely reaction to occur.

http://en.wikipedia.org/wiki/Table_of_standard_electrode_potentials

ii) NO3 + 4H + 3e --> NO + 2H2O - Reduction
    Cu --> Cu2+ + 2e - Oxidation

iii) Reduction x 2. Oxidation x 3

2NO3- + 8H + 3Cu ---> 2NO + 4H2O + 3Cu2+
  

[Hye]

Thanks
The iron content in a 0.200 g sample of fencing wire was determined by dissolving the wire in dilute sulfuric acid and making up the resulting pale green solution of Fe2+ ions to 25 mL. The solution was titrated with 0.0300 M potassium permanganate (KMnO4) solution, which is purple in colour. A titre of 20.22 mL was obtained. The solution of Mn2+ and Fe3+ ions produced by the reaction was almost colourless.
a   Write an overall equation for the titration reaction.

The wording is quite confusing :|

[Mao]

Preparation of Iron:

Fe --> Fe²⁺ + 2e

Redox reaction:

[coletrain]

OIL RIG