Home/ Questions/Balance the following redox reaction in acidic solution: Cu(s)+NO3−(aq)→Cu2+(aq)+NO2(g) Express your answer as a chemical equation...
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Asked: 2022-04-11T18:45:29+00:00 In:

Balance the following redox reaction in acidic solution: Cu(s)+NO3−(aq)→Cu2+(aq)+NO2(g) Express your answer as a chemical equation…

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Balance the following redox reaction in acidic solution:

Cu(s) + NO3−(aq) → Cu2+(aq) + NO2(g)

Express your answer as a chemical equation including phases.

♦ Relevant knowledge
Redox reaction

Reactions are triggered by the transfer of electrons. The reaction products that are able to transfer electrons are oxidized , and the process is referred to as the process of oxidation. The species that is prone to accept electrons is diminished and the process is called reduction.

Redox reaction is a mixture of two species, so the processes of reduction and oxidation happen simultaneously.

In order to balance these reactions, there are rules to follow.

  • Oxidation and reduction are written in a separate manner.
  • Charge is balanced through addition numbers of electrons.
  • The number of water molecules is balanced by hydrogen Ions.
  • The net or reaction that results is created by adding two half.
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    Based on the redox equation:

    Cu(s) + NO3−(aq) → Cu2+(aq) + NO2(g)

    This redox formula, the oxidation status for Cu changed from 0 to +2 and the N’s oxidation status N changed from +5 to +4.

    Step 1: Write the half equations

    Cu(s) → Cu2+(aq) NO3−(aq) → NO2(g)

    Step 2: Other elements apart from oxygen have been also balanced so let’s equalize the oxygen by adding water

    Cu(s) → Cu2+(aq) NO3−(aq) → NO2(g) + H2O(l)

    Cu(s) → Cu2+(aq) NO3−(aq) → NO2(g) + H2O(l)

    H+(aq)

    Cu(s) → Cu2+(aq) + 2H+(aq) + NO3−(aq) → NO2(g) + H2O(l) 

    Step 3: Balancing the charge through adding electrons

    Cu(s) → Cu2+(aq) + 2e−1e−+ 2H+(aq) + NO3−(aq) → NO2(g) + H2O(l)

    Step 4: Equalizing the electrons of both equations by multiplying equation 2 by the factor 2.

    Cu(s) → Cu2+(aq) + 2e−2e−+ 4H+(aq) + 2NO3−(aq) → 2NO2(g) + 2H2O(l)

    Step 5: Add both equations by cancelling out the same species on the opposite side of equations

    Cu(s) → Cu2+(aq) + 2e−2e− + 4H+(aq)+ 2NO3−(aq) → 2NO2(g) + 2H2O(l)

    Cu(s) + 4H+(aq) + 2NO3−(aq) → Cu2+(aq) + 2NO2(g) + 2H2O(l)  

    Thus, the balanced equation for redox is as follows

    Cu(s) + 4H+(aq) +2NO3−(aq) → Cu2+(aq) + 2NO2(g) + 2H2O(l)

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