Final answer:
The question involves calculating the Ecell of a voltaic cell at 25°C using the Nernst equation and then determining the maximum work possible. Standard reduction potentials are required to find E°cell, which is then used with ion concentrations to calculate Ecell and subsequently the maximum work.
Step-by-step explanation:
The question at hand relates to the electrochemistry subject in high school level chemistry, focusing on calculating the electromotive force (EMF) or Ecell of a voltaic cell and the maximum work that can be obtained from the cell at 25°C. The voltaic cell described consists of a Pb/Pb2+ half-cell and a Cu2+/Cu half-cell, with respective molar concentrations of 0.10 M and 2.00 M. To determine the Ecell, you would apply the Nernst equation:
Ecell = E°cell - (RT/nF) * ln(Q)
where:
- E°cell is the standard cell potential
- R is the gas constant (8.314 J/mol·K)
- T is the temperature in kelvin (298K for 25°C)
- n is the number of moles of electrons transferred
- F is Faraday's constant (96485 C/mol)
- Q is the reaction quotient
To find E°cell, we look up the standard reduction potentials for both half-cells and calculate:
E°cell = E°(Cu2+/Cu) - E°(Pb2+/Pb)
Q can be calculated using the ion concentrations given by:
Q = [Pb2+]2/[Cu2+]
Plugging in the numbers and solving for Ecell will give the voltage of the cell. The maximum work (W) possible from the cell can be calculated using the formula:
W = nFEcell
The correct option for maximum work will be determined using the calculated value of Ecell.