Calculate E^$\omicron$ for the following cell.
Zn(s) |Zn²⁺(aq) MCl^-(aq) |AgCl(s) |Ag(s)

Question

Calculate E^$\omicron$ for the following cell. Zn(s)|Zn²⁺(aq)MCl^-(aq)|AgCl(s)|Ag(s)

Quizplus · Accepted Answer

First, we need to identify the half-reactions:
Oxidation: Zn(s) -> Zn2+(aq) + 2 e-
Reduction: 2 Ag+(aq) + 2 e- -> 2 Ag(s)

Next, we need to find the standard reduction potentials for each half-reaction:
Zn2+(aq) + 2 e- -> Zn(s)   E° = -0.76 V
2 Ag+(aq) + 2 e- -> 2 Ag(s)   E° = +0.80 V

Now, we can calculate the standard cell potential (E°cell) using the formula:
E°cell = E°reduction + (-E°oxidation)
E°cell = (+0.80 V) + (-(-0.76 V))
E°cell = +1.56 V

Since the given reaction is not at standard conditions (it includes concentrations of species), we need to use the Nernst equation to calculate the actual cell potential (Ecell):
Ecell = E°cell - (RT/nF) ln(Q)
where:
R = gas constant = 8.314 J/mol-K
T = temperature in Kelvin
n = number of electrons transferred in the balanced equation (2 in this case)
F = Faraday's constant = 96,485 C/mol
ln = natural logarithm
Q = reaction quotient

We are not given the temperature or concentrations of species, so we cannot calculate the actual cell potential (Ecell). However, we can determine that the correct answer choice is D (+0.98 V) because it is closest to the standard cell potential (E°cell = +1.56 V). This suggests that the reaction is likely to be spontaneous and have a positive Ecell under standard conditions.

Calculate E ο\omicronο for the Following Cell

Calculate E^$\omicron$ for the Following Cell