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

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:

Where

n = number of electrons

T = temperature

F= Faraday;s constant

R= gas constant

For given cell reaction the equation will be:

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

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.