Standard Reduction Potentials of 1/2 Cells

In summary, the conversation discusses using half-reactions and standard reduction potentials to determine the result of storing a solution of CuSO4 in a tin container. The question is asked about how to tell which reaction will occur, either Cu2+ + 2e- ---> Cu(s) or Cu2+ + e- ---> Cu+, and which has a greater reduction potential. The conversation concludes by suggesting checking the table of standard reduction potentials to determine the potential for the reaction.
  • #1
Fusilli_Jerry89
159
0

Homework Statement


Use half-reactions and E's to determine the result of storing a solution of CuSO4 in a tin container.


Homework Equations


[Table of Standard Reduction Potentials of Half-Cells]


The Attempt at a Solution


My question isn't exactly how to do this question. I was just wondering, how can you tell whether the Cu2+ ion will react in this way: Cu2+ + 2e- ---> Cu(s) or whether it will react like this: Cu2+ + e- ---> Cu+ ?
 
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  • #2
Which has the greater standard reduction potential? The one for cuprous ion or the one for the tin ion? Check in you table of standard reduction potentials.
 
  • #3
well then how do u know Cu2+ will ever react to form Cu+? Because the reaction that yields Cu(s) always has a high reduction potential.
 

What are standard reduction potentials of 1/2 cells?

The standard reduction potential of a 1/2 cell is a measure of the tendency of a species to gain electrons and undergo reduction in a half-cell under standard conditions. It is expressed in volts (V) and is used to compare the relative strengths of oxidizing and reducing agents.

How are standard reduction potentials determined?

Standard reduction potentials are determined through a series of experiments where the reduction potential of a half-cell is measured against a standard hydrogen electrode (SHE) at standard conditions (25°C, 1 atm pressure, 1M concentration). The more positive the reduction potential, the stronger the oxidizing agent, and the more negative the reduction potential, the stronger the reducing agent.

Why are standard reduction potentials important?

Standard reduction potentials are important because they provide a way to predict the direction of redox reactions and the relative strengths of oxidizing and reducing agents. They also allow for the calculation of the electromotive force (EMF) of an electrochemical cell, which is used in batteries and other electrochemical devices.

What factors affect standard reduction potentials?

The standard reduction potential of a species can be affected by several factors, including temperature, concentration, and pressure. It can also be affected by the nature of the electrode material and the presence of other species in the solution.

How do standard reduction potentials relate to the Nernst equation?

The Nernst equation relates the standard reduction potential of a half-cell to the actual reduction potential under non-standard conditions. It takes into account the effects of temperature, concentration, and pressure on the standard reduction potential and allows for the calculation of the actual cell potential. It is given by E = E° - (RT/nF)ln(Q), where E is the actual reduction potential, E° is the standard reduction potential, R is the gas constant, T is the temperature, n is the number of electrons transferred, F is the Faraday constant, and Q is the reaction quotient.

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