In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell poten

In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell potential at 25°C?

In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell potential at 25°C?

Step 1: Identify the concentrations of Ag⁺ in the concentration cell. We have [Ag⁺]1 = 0.1 M and [Ag⁺]2 = 1 M.
Step 2: Write the formula for the cell potential (E) in a concentration cell: E = E° - (0.059/n)log([Ag⁺]1/[Ag⁺]2.
Step 3: Determine the standard cell potential (E°) for the reaction. For a concentration cell, E° = 0 V.
Step 4: Identify the number of electrons transferred (n) in the reaction. For Ag⁺ to Ag, n = 1.
Step 5: Substitute the values into the formula: E = 0 - (0.059/1)log(0.1/1).
Step 6: Calculate the logarithm: log(0.1) = -1.
Step 7: Substitute the logarithm value back into the equation: E = 0 - (0.059)(-1).
Step 8: Calculate the final cell potential: E = 0.059 V.

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