2 years ago

Please help .....................

Chemistry

1 answer:

Advocard [28]2 years ago

8 0

Answer:

Explanation:

The photo is not there :o

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Suppose a current of is passed through an electroplating cell with an aqueous solution of agno3 in the cathode compartment for s

WARRIOR [948]

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

Explanation:

$Q=I\times t$

where Q= quantity of electricity in coloumbs

I = current in amperes = 0.920 A

t= time in seconds = 47.0 sec

$Q=0.920A\times 47.0s=43.24C$

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

$Ag^++e^-\rightarrow Ag$

96500 Coloumb of electricity electrolyzes 1 mole of Ag

43.24 C of electricity deposits = $\frac{1}{96500}\times 43.24=0.00045moles$ of Ag

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

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

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