<u>Answer:</u> The standard free energy change for the reaction will be -1308.54 kJ.
<u>Explanation:</u>
We are given a net redox reaction:
Here, gold is getting reduced and zinc is getting oxidized. So, the half cell reactions for the above net reaction are:
<u>At Cathode:</u> × 2
<u>At Anode:</u> × 3
To calculate the , we use the equation:
= Standard oxidation potential of the oxidation half reaction + Standard reduction potential of the reduction half reaction
Putting values in above equation:
The total electrons change for the redox reaction are 6.
To calculate he standard free energy change, we use the equation:
where,
n = Number of electron change = 6
F = Faraday's constant = 96500 F
Putting values in above equation, we get:
Hence, the standard free energy change for the reaction will be -1308.54 kJ.