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.

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.

  0.0484 g

Explanation:

where Q= quantity of electricity in coloumbs

I = current in amperes = 0.920 A

t= time in seconds = 47.0 sec

96500 Coloumb of electricity electrolyzes 1 mole of Ag

43.24 C of electricity deposits = of Ag

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

h let me think

it is a solid

explanation: