What is the standard reaction free energy if the standard cell emf is 1.23?
Faraday’s constant is 96485 C/mol.
Answer in units of kJ/mol
dG = -nEoF.
To calculate the standard reaction free energy (ΔG°) using the standard cell emf (E°) and Faraday's constant (F), you can use the equation:
ΔG° = -nFE°
Where:
ΔG° is the standard reaction free energy
n is the number of electrons transferred during the reaction (determined from the balanced equation of the reaction)
F is Faraday's constant
E° is the standard cell emf
In this case, we are given E° as 1.23 and F as 96485 C/mol.
To proceed, you need to determine the number of electrons transferred (n) based on the balanced equation for the reaction. Once you have n, plug in the values into the formula to find the value of ΔG°.
Please provide the balanced equation for the reaction, so we can determine the value of n and further calculate ΔG°.