Calculate the ΔG for the cell reaction at 298 K for the cell.Zn(s) | Zn2+ || Cd2+ | Cd(s)Given : F = 96500 C mol–1, Ecell = 0.44 V
Question
Calculate the ΔG for the cell reaction at 298 K for the cell.
Zn(s) | Zn2+ || Cd2+ | Cd(s)
Given :
F = 96500 C mol–1, Ecell = 0.44 V
Solution
Sure, here are the steps to calculate the ΔG for the cell reaction at 298 K for the cell.
Step 1: Write down the given values. Ecell = 0.44 V F = 96500 C mol–1
Step 2: Use the formula for Gibbs free energy change (ΔG) in a redox reaction. ΔG = -nFEcell
In this case, the reaction is Zn(s) + Cd2+ → Zn2+ + Cd(s). The number of electrons transferred (n) in this reaction is 2 (from Zn to Cd2+).
Step 3: Substitute the given values into the formula. ΔG = -2 * 96500 C mol–1 * 0.44 V
Step 4: Calculate the value. ΔG = -84960 J/mol
So, the Gibbs free energy change for the cell reaction at 298 K is -84960 J/mol.
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