Question

Suppose a current of is passed through an electroplating cell with an aqueous solution of agno3 in the cathode compartment for seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.

Answer 1

The given question is incomplete. The complete question is:

Suppose a current of 0.920 A is passed through an electroplating cell with an aqueous solution of agno3 in the cathode compartment for 47.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.

Answer: 0.0484 g

Step-by-step explanation:

`Q=I* t`

where Q= quantity of electricity in coloumbs

I = current in amperes = 0.920 A

t= time in seconds = 47.0 sec

`Q=0.920A* 47.0s=43.24C`

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

`Ag^++e^-\rightarrow Ag`

96500 Coloumb of electricity electrolyzes 1 mole of Ag

43.24 C of electricity deposits =
`(1)/(96500)* 43.24=0.00045moles` of Ag

`\text{ mass of Ag}={\text{no of moles}* {\text{Molar mass}}=0.00045mol* 108g=0.0484g`

Thus the mass of pure silver deposited on a metal object made into the cathode of the cell is 0.0484 g