A 0.005 cm thick coating of copper is deposited on a plate of `0.5m^2` total area. Calculate the number of copper atoms deposited on the plate (density of copper = 7.2 g `cm^(-3)`, atomic mass = 63.5 )

Electric current is passed through two cells A and B in series. Cell A contains aqueous solution of Ag_(2) SO_(4) and platinum electrodes. Cell B contains aqueous solution of CuSO_(4) and copper electrodes. The current is passed till 1.6g of oxygen is liberated at the anode in cell A. Calculate the quantities of copper and silver deposited at the cathode of the two cells. [ Atomic mass, O = 16, Cu 63.5, Ag = 108]

Find the quantity of electricity needed to plate a metal of 100 cm^2 area and 10^-2cm thickness using CuSO_4 solution. (density of copper = 9.94 gm//cm^3 and atomic mass = 63.5)

Silver is electrolytically deposited on a metallic vessel of total surface area 900 c m^(2) by passing a current of 0.5A for 2h. Calculate the thickness of silver deposited . Given, density of silver =10.5 g c m^(-1) . Atomic mass of silver = 108u, F = 96500 C "mol"^(-1)

Calculate the r.m.s velocity of nitrogen molecule at N.T.P. if the density of nitrogen is 0.001293 g cm^(_3)

Calculate the number of moles in an iron bar dimension 10 cm xx 4 cm xx 2..5 cm density of iron being 7.85 gm/ cm^3

0.2 amp current flowing for 15 minutes deposits copper of 0.1978gm. Find the electro chemical equivalent of copper

The radius of a circle increases at a rate of 0.2 cm/s. Calculate the rate of the increase of the area, when the radius is 5 cm.

X-ray diffraction studies show that copper crystallises in a fcc unit cell with cell edge of 3.608 xx10^(-8) cm. In a separate experiment, copper is determined to have a density of 8.92 g//cm^(3) , calculate the atomic mass of copper.