Calculate the potential at 25∘C for a cell that has the following ion concentrations: [Ag+] = 1.0×10−2M , 3.2×10−2M .
Your post isn't very clear. Do you mean this is a concentration cell with one half cell of 1E-2M and the other 3.2E-2.
If so then Ecell = -(0.05916/1)log (dilute/concd)
Sorry!
Consider a galvanic cell that uses the reaction
2Ag+(aq)+Sn(s)→2Ag(s)+Sn2+(aq)
What is Ag? What's the other number for?
To calculate the potential of a cell, you need to use the Nernst equation, which relates the cell potential to the concentrations of the ions involved in the cell reaction. The Nernst equation is given by:
E = E° - (RT / nF) * ln(Q),
where:
- E is the cell potential,
- E° is the standard cell potential at 25°C,
- R is the gas constant (8.314 J/mol·K),
- T is the temperature in Kelvin,
- n is the number of electrons transferred in the cell reaction,
- F is Faraday's constant (96485 C/mol), and
- Q is the reaction quotient, which is the concentration ratio of the products divided by the concentration ratio of the reactants.
Based on the given concentrations, it seems like this is a cell involving the Ag+ ion. However, you haven't specified the other ion involved in the cell reaction, so it's not possible to determine the reaction equation or the value of n.
Please provide the other ion involved in the cell reaction, so we can proceed with calculating the cell potential.