2Al(s) + 3Pb2 ==> Al2Pb3
So the question says using that equation, what is the standard free energy. Faraday’s J constant is 96485 V · mol . Answer in units of kJ/mol.
I'm... very lost
delta G = -nEoF
n = 6
Calculate Eo for the equation shown using Eo values in tables in your text or on the web.
F is given. Substitute and solve. That will give you delta G.
Post your work if you get stuck.
I was able to figure it out! Thank you :)
To calculate the standard free energy change (∆G°) using the given equation, we need to know the standard reduction potentials (∆G°) for each species involved. However, the equation you provided is incorrect. It seems like there might be a typo or missing information in it.
Please double-check the equation provided and make sure it is balanced and accurate. Once you provide the correct equation, I'll be more than happy to help you calculate the standard free energy change (∆G°).
To calculate the standard free energy change (ΔG°) for the given reaction, you would need to know the standard electrode potentials (E°) of the half-reactions involved.
In this case, the reaction involves the oxidation of aluminum (Al) and the reduction of lead(II) ions (Pb2+). The half-reactions for these processes are as follows:
Al(s) → Al3+(aq) + 3e- E°1 (oxidation)
Pb2+(aq) + 2e- → Pb(s) E°2 (reduction)
To determine the overall ΔG°, you can use the equation:
ΔG° = -nFΔE°
Where:
ΔG° = standard free energy change
n = number of electrons transferred in the balanced equation
F = Faraday's constant = 96485 C/mol (or J/V·mol, as provided)
ΔE° = difference in standard electrode potentials between the oxidation and reduction half-reactions
For the given reaction:
2Al(s) + 3Pb2+ → Al2Pb3
The balanced equation tells us that 3 electrons are transferred. Therefore, n = 3.
To calculate ΔE°, you subtract the reduction potential from the oxidation potential:
ΔE° = E°2 - E°1
You will need to look up the standard electrode potentials for the half-reactions for Al and Pb2+ in a table or reference source. The values typically have units of volts.
Once you have the values for E°1 and E°2, you can substitute them into the equation to calculate ΔE°. Then, substitute the values for n, F, and ΔE° into the equation for ΔG° and convert the answer to kJ/mol if needed.
I do not have access to a database for electrode potentials, so you will have to look up the values and perform the calculations yourself.