The amount of Zn plated from a [tex]Zn^{2+}[/tex] solution is [tex]1.07[/tex]×[tex]10^{-1}[/tex] grams.
In this question, it is given that of 317.7 coulombs was used in an electrolytic cell, i.e,
The amount of charge = 317.7 coulombs
The amount of charge of 1 mole of electrons = 96485.3 coulombs (FARADAY’S CONSTANT)
Now, the number of electrons = amount of charge given / charge of 1 mole of electrons
The number of electrons = [tex]\frac{317.7}{96485.3}[/tex] = [tex]3.29[/tex]×[tex]10^{-3}[/tex]
According to reaction occurring, 2 moles of electrons are required to convert 1 mole of to Zn which is plated on the electron, so the moles of Zn plated will be half the moles of electrons, i.e.,
[tex]\frac{3.29}{2}[/tex]×[tex]10^{-3}[/tex] = 1.645×[tex]10^{-3}[/tex]
Now, we know that the molar mass of zinc is 65.38gm/mole,
Number of moles = mass in grams / molar mass
Mass in grams = number of moles × molar mass
Mass in grams = ([tex]1.645[/tex]×[tex]10^{-3}[/tex]) × 65.38 = 0.1075 gm.
CONCLUSION: It concludes that the amount of Zn plated from a solution is [tex]1.07[/tex]×[tex]10^{-1}[/tex] gm.
#SPJ4
https://brainly.com/question/15729041
