Question: In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell potential at 25°C?
Options:
0.059 V
0.118 V
0.177 V
0.236 V
Correct Answer: 0.118 V
Solution:
E = E° - (0.059/n)log([Ag⁺]1/[Ag⁺]2); E = 0 - (0.059/1)log(10) = 0.059 V.
In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell poten
Practice Questions
Q1
In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell potential at 25°C?
0.059 V
0.118 V
0.177 V
0.236 V
Questions & Step-by-Step Solutions
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.
Concentration Cell – A type of electrochemical cell where the same species is present in two different concentrations, leading to a potential difference.
Nernst Equation – A formula used to calculate the cell potential based on standard electrode potential and the concentrations of the reactants and products.
Logarithmic Relationships – Understanding how to manipulate logarithmic functions in the context of the Nernst equation.
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