Calculate the standard free-energy change for the following reaction at 25 c. standard reduction potentials can be found here. 2au^3+ (aq) + 3zn (s) < --> 2au (s) + 3zn^2+(aq) can someone me with this?

The standard free energy change for the reaction will be -1308.54 kJ.

Explanation:

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:

At Cathode:  × 2   

At Anode:    × 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.