Answer: The mass of metallic silver produced by a 1.50
amp current passed through a solution of silver nitrate for 20 minutes is 2.0 g
Explanation:
Moles of electron = 1 mole
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]
Charge on 1 mole of electrons = [tex]1.6\times 10^{-19}\times 6.022\times 10^{23}=96500C[/tex]
To calculate the time required, we use the equation:
[tex]I=\frac{q}{t}[/tex]
where,
I = current passed = 1.50 A
q = total charge = ?
t = time = 20 minutes = 1200 s (1min=60 s)
Putting values in above equation, we get:
[tex]1.50A=\frac{q}{1200s}[/tex]
[tex]q=1800C[/tex]
[tex]AgNO_3\rightarrow Ag^++NO_3^-[/tex]
[tex]Ag^++e^-\rightarrrow Ag[/tex]
According to stoichiometry:
1 mole of electrons deposit = 108 g of silver
i.e 96500 C of electricity deposit = 108 g of silver
Thus 1800 C of electricity deposit = [tex]\frac{108}{96500}\times 1800=2.0[/tex] g of silver
The mass of metallic silver is 2.0 g
