The following galvanic cell at standard conditions has a potential of 0.03 V:
Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s).
What would be the effect of increasing the concentration of Ag+?
A. The cell potential will decrease.
B. The cell potential will increase.
C. The cell potential will not change.
D. The cell potential will be 0 V.
it will increase
It will increase for sure
Well, let's see here. Increasing the concentration of Ag+ in the cell would shift the equilibrium to the right, according to Le Chatelier's principle. And what does that mean for our potential? It means the reduction half-reaction involving Ag+ will occur more readily, causing the cell potential to increase. So, the answer is B. The cell potential will increase. Ag+ is like the hype man of this galvanic cell, getting everyone excited and boosting the potential. Keep it up, Ag+!
To determine the effect of increasing the concentration of Ag+ on the cell potential, we need to consider the Nernst equation, which relates the cell potential to the concentrations of species involved in the chemical reaction.
The Nernst equation is given as:
E = E° - (RT/nF) * ln(Q)
where:
E = cell potential
E° = standard cell potential
R = gas constant (8.314 J/mol·K)
T = temperature (in Kelvin)
n = number of moles of electrons transferred in the balanced reaction
F = Faraday's constant (96485 C/mol)
ln = natural logarithm
Q = reaction quotient
In the given galvanic cell, the reaction equation is:
Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s)
Since the reaction is at standard conditions, the standard cell potential (E°) is provided as 0.03 V.
Now, consider the effect of increasing the concentration of Ag+. When we increase the concentration of Ag+, the reaction quotient (Q) increases as well because the products (Fe3+(aq) and Ag(s)) remain the same while the concentration of Ag+(aq) increases. According to the Nernst equation, an increase in the reaction quotient leads to a decrease in the cell potential.
Therefore, the correct answer is:
A. The cell potential will decrease.