Silver is electro-deposited on a metallic vessel of surface area 800 `cm^(2)` by passing a current of 0.2 ampere for 3 hours. Calculate the thickness of silver deposited given that its density is 10.47 g `cm^(-3)`. (At mass of Ag =107.92).

Silver is electro-deposited on a metallic vessel of surface area 800 `

1.	Silver is electro-deposited on a metallic vessel of surface area 800 `cm^(2)` by passing a current of 0.2 ampere for 3 hours. Calculate the thickness of silver deposited given that its density is 10.47 g `cm^(-3)`. (At mass of Ag =107.92).
Answer» Correct Answer - `2.88xx10^(4) cm` The charge ,Q on n moles of electrons is given by Q=nF where Faraday constant, `" " F=96500" C" mol^(-1)` Thus, quantity of electricity required to deposit 1 mole of Ag, `Q=1" mol"xx96500"C mol"^(-1)=96500" C " =9365xx10^(4)" C " `. Quantity of electricity actually used used`="Current in amperes"xx "Time in seconds"` `=0.2Axx(3xx60xx60)s` `=0.2xx3xx60xx60" As" =2160" C " " "(because As=C)` Molar mass fo Ag`=107.92" g mol^(-1)` `9.65xx10^(4)C` of charge produce silver=107.92 g `:.` 2160 C of charge produce silver`=((107.92 g))/((9.65xx10^(4)C))xx(2160" C")=2.4156 g` Volume of silver deposited`=("Mass")/("Density")=((2.4156 g))/((10.47 g cm^(-3)))=0.2307 cm^(3)` Thickness of silver deposited`=("Volume")/("Surface area")=((0.2307 cm^(3)))/((800 cm^(2)))=2.88xx10^(-4) cm`.

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Silver is electro-deposited on a metallic vessel of surface area 800 `cm^(2)` by passing a current of 0.2 ampere for 3 hours. Calculate the thickness of silver deposited given that its density is 10.47 g `cm^(-3)`. (At mass of Ag =107.92).

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