Answer to Question #97690 in Chemistry for belle

Question

Calculate the mass of silver deposited by electrolysis of A.gNo3 placed in series with a Cuso4 solution when 0.37g of copper are deposited on the copper place

(cu=64,Ag=108,F=96500c )

Answer 1

The balanced reaction equation is; AgNo3 +CUSo4 = AgSO4 +CUNo3. Therefore, the mole ratio is 1:1.

First, we determine the number of moles of CU.

$Moles = mass/RFM$

$CU moles= 0.37/64= 0.0058 moles$

Then we find the charge used to deposit 0.37g of CU. From faradays law 1mole contains 965000 coulombs (charge), therefore 0.0058moles of CU will have a charge of 559.7c. From the mole ratio then the same amount of charge is expected to deposit silver in its place. Hence the same number moles of Ag as CU are deposited. The mass of Ag deposited is calculated as;

$Mass= moles*RFM$

$Mass = 0.0058 *108= 0.6264g$

Mass of Ag deposited is 0.6264g