Write molecular, complete ionic, and net ionic equations for the reactions that occur, if any, when solutions of the following s
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<u>Answer:</u>
<u>For A:</u> The standard cell potential of the reaction is 4.4 V
<u>For B:</u> The standard Gibbs free energy of the reaction is
<u>For C:</u> The reaction is spontaneous as written.
<u>Explanation:</u>
- <u>For A:</u>
The given chemical reaction follows:
The given half reaction follows:
<u>Oxidation half reaction:</u> ( × 2)
<u>Reduction half reaction:</u>
The substance having highest positive potential will always get reduced and will undergo reduction reaction.
Here, chlorine will undergo reduction reaction will get reduced.
Substance getting oxidized always act as anode and the one getting reduced always act as cathode.
To calculate the of the reaction, we use the equation:
Hence, the standard cell potential of the reaction is 4.4 V
- <u>For B:</u>
Relationship between standard Gibbs free energy and standard electrode potential follows:
where,
n = number of electrons transferred =
F = Faradays constant =
= standard cell potential = 4.4 V
Putting values in above equation, we get:
Hence, the standard Gibbs free energy of the reaction is
- <u>For C:</u>
For a reaction to be spontaneous, the standard Gibbs free energy change of the reaction must be negative.
From above, the standard Gibbs free energy change of the reaction is coming out to be negative.
Hence, the reaction is spontaneous as written.