Cell Designation : E (measured)
= Sn I Sn^2+ II Cu^2+ I Cu
Temp= 3 Celsius
Temp= 276.15 Kelvin
Delta G= ?????
Show work please!!!!
I have to use the formula below but I don't know how! :(
Delta G = -nFE
n = number of electrons transferred. In this case that is 2. Sn ==> Sn^2+ + 2e and Cu^2+ + 2e ==> Cu
F is the Faraday constant of 95,485 coulombs
E is the cell voltage.
T is kelvin temperature. substitute and go. Don't foget the - sign.
how do i get voltage cell????
Your post said "E measured" so I assume you have that given to you. If it isn't given, add the oxidation half cell to the reduction half cell to obtain Ecell.
To calculate the standard Gibbs free energy change (ΔG) for the given cell reaction, we need to use the Nernst equation:
ΔG = -nFΔEcell
where:
- ΔG is the standard Gibbs free energy change
- n is the total number of electrons transferred in the balanced cell reaction
- F is the Faraday's constant (approximated as 96,485 C/mol)
- ΔEcell is the cell potential, which can be calculated using the standard reduction potentials (E°) of the half-reactions involved in the cell reaction:
1. Identify the half-reactions for each electrode in the cell:
- Sn → Sn^2+ + 2e^- (Reduction half-reaction)
- Cu^2+ + 2e^- → Cu (Oxidation half-reaction)
2. Look up the standard reduction potentials (E°) for each half-reaction in a table or reference source. The E° value for the reduction half-reaction of Sn^2+ can be found to be -0.14 V, and the E° value for the oxidation half-reaction of Cu^2+ can be found to be 0.34 V.
3. Calculate the cell potential (Ecell) using the Nernst equation:
Ecell = E°(reduction) - E°(oxidation)
Ecell = (-0.14 V) - (0.34 V)
Ecell = -0.48 V
4. Subtract the appropriate number of electrons (n) involved in the balanced cell reaction. In this case, since the balanced reaction has one Sn^2+ ion and one Cu^2+ ion, the number of electrons transferred is 2 (2e^-), so n = 2.
5. Calculate the standard Gibbs free energy change (ΔG):
ΔG = -nFΔEcell
ΔG = -(2)(96,485 C/mol)(-0.48 V)
ΔG = 92,579 J/mol
Therefore, the standard Gibbs free energy change (ΔG) for the given cell reaction is 92,579 J/mol.