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Consider an electrochemical cell based on the reaction: 2H+(aq) + Sn(s) = Sn2+(aq) + H2(g). Which of the following actions would NOT change the measured cell potential?

1. lowering the pH in the cathode compartment
2. addition of more tin metal to the anode compartment
3. any of the changes listed here will change the measured cell potential.
4. increasing the pressure of hydrogen gas in the cathode compartment.
5. increasing the [Sn2+] in the anode compartment

Respuesta :

Answer:

2. addition of more tin metal to the anode compartment

Explanation:

For the given cell reaction:

Hydrogen is undergoing reduction

Sn is undergoing oxidation

The cell potential of a cell depends upon

a) the temperature

b) the concentration of aqueous species

c) the pressure of gaseous species

It is independent of the amount of the solid present or taken

The dependence of cell potential on concentration and temperature is given in the form of Nernst's equation:

[tex]E_{cell{=E^{0}_{cell}-\frac{RT}{nF}log(\frac{anode]}{[cathode]} )[/tex]

Where

n = number of electrons

T = temperature

F= Faraday;s constant

R= gas constant

For given cell reaction the equation will be:

[tex]E_{cell{=E^{0}_{cell}-\frac{RT}{2XF}log(\frac{[Sn^{+2}][P_{H2}]}{[H^{+}]^{2}} )[/tex]

Thus the action that would not change the measured cell potential would be: 2. addition of more tin metal to the anode compartment

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