A white powder is added to a solution. The images show observations made before the powder is added, just after the powder has b

Answer: The cell potential for the given reaction stands at 0.50 V

Explanation:

The provided cell reaction is:

The half-reactions are:

Anode oxidation half reaction:  

Cathode reduction half reaction:  

Initially, we need to find the cell potential for this reaction.

Utilizing the Nernst equation:

where,

F = Faraday's constant = 96500 C

R = gas constant = 8.314 J/mol·K

T = room temperature =

n = electrons exchanged in oxidation-reduction = 2

= standard electrode potential for the cell = +0.63 V

= cell potential for the reaction =?

= concentration of Zn²⁺ = 3.5 M

=

Now substituting all known values into the equation, we arrive at:

So, the resulting cell potential for this reaction is 0.50 V

The formula for Molarity is given by:

                                  M = moles / V
To isolate V,
                              V = moles / M ------------------(1)
Moles can also be calculated as:
                                  moles = mass / M.mass -------------(2)
Substituting the value of moles from equation 2 into equation 1 yields:
                                  V = (mass / M.mass) / M
Plugging in the numbers gives:
                                  V = (45 g / 164 g/mol) / 1.3 mol/dm³

                                       V = 0.21 dm³.