If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction pote

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Question: If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction potential is +0.34 V, what is the cell potential at 25°C using the Nernst equation?

Options:

0.34 V
0.30 V
0.28 V
0.25 V

Correct Answer: 0.30 V

Solution:

E = E° - (RT/nF)ln(Q); E = 0.34 - (0.0257/2)ln(100) = 0.30 V.

If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction pote

Practice Questions

If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction potential is +0.34 V, what is the cell potential at 25°C using the Nernst equation?

0.34 V
0.30 V
0.28 V
0.25 V

Questions & Step-by-Step Solutions

If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction potential is +0.34 V, what is the cell potential at 25°C using the Nernst equation?

Step 1: Identify the given values. The concentration of Cu²⁺ is 0.01 M, the standard reduction potential (E°) is +0.34 V, and the temperature is 25°C.
Step 2: Convert the temperature from Celsius to Kelvin. 25°C is equal to 298 K (25 + 273).
Step 3: Use the Nernst equation: E = E° - (RT/nF)ln(Q).
Step 4: Determine the values for R, T, n, and F. R (universal gas constant) = 0.0257 V·K/C, T = 298 K, n (number of electrons transferred) = 2 for Cu²⁺, and F (Faraday's constant) = 96485 C/mol.
Step 5: Calculate Q, the reaction quotient. Since the concentration of Cu²⁺ is 0.01 M, Q = 1 / [Cu²⁺] = 1 / 0.01 = 100.
Step 6: Substitute the values into the Nernst equation: E = 0.34 - (0.0257/2)ln(100).
Step 7: Calculate (0.0257/2) = 0.01285.
Step 8: Calculate ln(100) which is approximately 4.605.
Step 9: Multiply 0.01285 by 4.605 to get approximately 0.0592.
Step 10: Subtract this value from 0.34: E = 0.34 - 0.0592 = 0.2808 V.
Step 11: Round the final answer to two decimal places: E ≈ 0.30 V.

Nernst Equation – The Nernst equation relates the cell potential to the standard reduction potential and the concentrations of the reactants and products.
Standard Reduction Potential – The standard reduction potential is a measure of the tendency of a chemical species to be reduced, measured under standard conditions.
Cell Potential Calculation – Calculating the cell potential involves substituting values into the Nernst equation and understanding the significance of each term.

If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction pote

What’s inside this PDF?

If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction pote

Practice Questions

Questions & Step-by-Step Solutions

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