Questions: Non-Standard Cells Cu^2+(aq) + Zn(s) ⇌ Cu(s) + Zn^2+(aq) What happens to the cell potential with the change in conditions? The cell potential will be greater than 1.10 V. A new cell is constructed in which the copper concentration is raised to [Cu^2+]-2.0 M, the zinc concentration is held standard at [Zn^2+]-1.0 M, and the temperature is held the same. The cell potential will remain 1.10 V.

Non-Standard Cells
Cu^2+(aq) + Zn(s) ⇌ Cu(s) + Zn^2+(aq)

What happens to the cell potential with the change in conditions?
The cell potential will be greater than 1.10 V.

A new cell is constructed in which the copper concentration is raised to [Cu^2+]-2.0 M, the zinc concentration is held standard at [Zn^2+]-1.0 M, and the temperature is held the same.
The cell potential will remain 1.10 V.
Transcript text: Non-Standard Cells \[ \mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{Zn}(\mathrm{~s}) \rightleftharpoons \mathrm{Cu}(\mathrm{~s})+\mathrm{Zn}^{2+}(\mathrm{aq}) \] What happens to the cell potential with the change in conditions? The cell potential will be greater than 1.10 V . A new cell is constructed in which the copper concentration is raised to $\left[\mathrm{Cu}^{2+}\right]-2.0 \mathrm{M}$, the zinc concentration is held standard at $\left[\mathrm{Zn}^{2+}\right]-1.0 \mathrm{M}$, and the temperature is held the same. The cell potential will remain 1.10 V .
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Solution

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Solution Steps

Step 1: Analyze the Nernst Equation

The Nernst equation helps determine the cell potential under non-standard conditions: E = E° - (RT/nF) * ln(Q)

Where:

  • E is the cell potential under non-standard conditions
  • E° is the standard cell potential (1.10 V in this case)
  • R is the ideal gas constant
  • T is the temperature in Kelvin
  • n is the number of moles of electrons transferred in the balanced redox reaction (n=2 for this reaction)
  • F is Faraday's constant
  • Q is the reaction quotient
Step 2: Determine Q

The reaction quotient, Q, is calculated similar to the equilibrium constant, K, but using the current concentrations of the reactants and products: Q = [Zn²⁺]/[Cu²⁺] = (1.0 M)/(2.0 M) = 0.5

Step 3: Evaluate the Nernst Equation

Since the copper concentration is increased, and the zinc concentration is standard, the value of Q is less than 1. The natural logarithm of a number between 0 and 1 is negative. Thus, the term (RT/nF) * lnQ becomes negative, and subtracting a negative value is equivalent to adding a positive value. Therefore, the cell potential (E) under these non-standard conditions will be greater than the standard cell potential (E°).

Final Answer The cell potential will be greater than 1.10 V.

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