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

calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2

gas

explanation:

smoke is the matter of a gas