Question

What is the mass of metallic silver produced by a 1.50

ampcurrent passed through a solution of silver nitrate for
20minutes?

Answer 1

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

Step-by-step explanation:

Moles of electron = 1 mole

According to mole concept:

1 mole of an atom contains
`6.022* 10^(23)` number of particles.

We know that:

Charge on 1 electron =
`1.6* 10^(-19)C`

Charge on 1 mole of electrons =
`1.6* 10^(-19)* 6.022* 10^(23)=96500C`

To calculate the time required, we use the equation:

`I=(q)/(t)`

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:

`1.50A=(q)/(1200s)`

`q=1800C`

`AgNO_3\rightarrow Ag^++NO_3^-`

`Ag^++e^-\rightarrrow Ag`

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 =
`(108)/(96500)* 1800=2.0` g of silver

The mass of metallic silver is 2.0 g