Calculate the time required to coat a metal surface of `80 cm^(2)` with `0.005 mm` thick layer of silver (density `= 10.5 g cm^(3))` with the passage of `3A` current through silver nitrate solution.

The time required to coat a metal surface of 80 cm^(2) with 5 xx 10^(-3) cm thick layer of silver (density 1.05 g cm^(-3) ) with the passage of 3A current through a silver nitrate solution is:

The time required to coat a metal surface of 80 cm^2 with 5xx10^(-3) cm thick layer of silver (density 10.5 g cm^(-3) with th passage of 3A current through a silver nitrate solution is :

Calculate the time required to coat a metal surface of 50 cm2 with 0.01 mm thick layer of chromium (density = 7.19 g cm-3) by the passage of 5 A current.

A current of 4 A is passed through a solution of silver nitrate to coat a metal surface of 80 cm^(2) with 0.005 mm thick layers of silver. If the density of silver (molar mass: 108 g "mol"^(-1) )is 10.8 g cm^(-3) , the time for which the current is passed is about

How long a current of 3 ampere has to be passed through a soulution of silver nitrate to coat a metal. Surface of 80cm^(2) with a 0.005 mm thick layer? Density of Ag is 10.5gcm^(-3) . At wt. Ag=108.0u

How much time is required to deposit 1xx10^(-3) cm thick layer of silver (density is 1.05 g cm^(-3) ) on a surface of area 100 cm^2 by passing a current of 5 A through AgNO_3 solution?