Respuesta :
This is a incomplete question. The complete question is :
Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive) layer of a precious metal, such as silver or gold. In essence the metal object is made the cathode of an electrolytic cell in which the precious metal cations are dissolved in aqueous solution. Suppose a current of 0.270 A is passed through an electroplating cell with an aqueous solution of [tex]Ag_2SO_4[/tex] in the cathode compartment for 72 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell. Be sure your answer has a unit symbol and the correct number of significant digits.
Answer: 0.219 g
Explanation:
According to mole concept:
1 mole of an atom contains [tex]6.022\times 10^{23}[/tex] number of particles.
We know that:
Charge on 1 electron = [tex]1.6\times 10^{-19}C[/tex]
To calculate the charge passed, we use the equation:
[tex]I=\frac{q}{t}[/tex]
where,
I = current passed = 0.272 A
q = total charge = ?
t = time required = 72.0 s
Putting values in above equation, we get:
[tex]0.272A=\frac{q}{72}\\\\q={0.272A}\times 72.0=19.6C[/tex]
[tex]Ag_2SO_4\rightarrow 2Ag^+SO_4^{2-}[/tex]
[tex]Ag^++e^-\rightarrow Ag[/tex]
108 g of silver is deposited by 1 mole of electrons
96500 C deposits = 108 g of dilver
Thus 19.6 C deposits =[tex]\frac{108}{96500}\times 19.6=0.0219g[/tex]
Thus the mass of pure silver deposited on a metal object made into the cathode of the cell is 0.0219 g
