I posted this que before but got no answers pls help me :(
A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+ concentration is 2.0 ´ 10-5 M and by placing a Pt electrode in the other compartment, in which the H+ concentration is 3.4 M and = 1.00 atm.
And you have asked no question.
What is E for the cell at equilibrium?
Of course, I'll be happy to help you with your question about the voltaic cell.
In order to analyze the cell, we need to understand the concept of a standard reduction potential (E°). The standard reduction potential is a measure of the tendency of a half-reaction to occur as a reduction (meaning gaining electrons) under standard conditions.
To find the overall potential of the cell, we can use the Nernst equation, which relates the cell potential to the concentration of species involved in the redox reaction. The Nernst equation can be expressed as:
E = E° - (0.0592/n) * log(Q)
Where:
E is the cell potential
E° is the standard reduction potential
(0.0592/n) is the temperature-dependent conversion factor
log(Q) is the log of the reaction quotient
To apply the Nernst equation, we first need to balance the half-reactions and determine the value of the standard reduction potential for each half-reaction.
Based on your description, it seems like the cell consists of the following half-reactions:
1. Reduction half-reaction: Fe2+(aq) + 2e- -> Fe(s)
For this half-reaction, we can look up the standard reduction potential (E°) for the reduction of Fe2+ to Fe (s) from a table of standard reduction potentials.
2. Oxidation half-reaction: 2H+(aq) -> H2(g) + 2e-
Since the reaction involves H+ ions, we need to consider the standard reduction potential for the reduction of H+ to H2.
Once we have determined the standard reduction potentials for both half-reactions, we can calculate the cell potential using the Nernst equation.
If you provide me with the standard reduction potentials for these half-reactions, I can help you calculate the cell potential.