In the refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal. Write down the reaction involved.

In a diffraction phenomenon , radius of the central bright region is given as r_(0)=(1.22lambdaf)/(2a) , where lambda is wavelength of the light , f is the focal length of the lens used and 2a is the diameter of the aperture .Show that in order to observe two objects clearly by a microscope , the minimum separation between them must be (1.22lambda)/(2sinbeta) , where beta is the angle between principal axis of the objective and the ray of light from the object to the apex of the lens .

Describe the role of SiO_2 in the extraction of Copper from Copper matte.

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknonw concentration. It other half cell consists of a zinc electrode dipping in 1.0M solution of Zn(NO_3)_2 . A voltage of 1.48V is measure for this cell. Use this information to calculate the concentration of silver nitrate solution used (E_(Zn^(2+)//Zn)^0=-0.76V,E_(Ag^+//Ag)^0=+0.80V)

A copper silver cell is set up. The copper ion concentration is 0.10M . The concentration of silver ion is not known. The cell potential when measured was 0.422V. Determine the concentration of silver ions in the cell. (Given) E_(Ag^(2+)//Ag)^@=+0.80V,E_(Cu^(2+)//Cu)^@=+0.34V

Two electrolytic cell containing AgNO_3 solution and dilute H_2SO_4 solution were connected in series. A steady current of 2.5 ampre was passed through them till 1.078g of silver was deposited. (Ag = 108 u, IF = 96500 C). How much electricity was consumed?

Two electrolytic cell containing AgNO_3 solution and dilute H_2SO_4 solution were connected in series. A steady current of 2.5 ampere was passed through them till 1.078g of silver was deposited. (Ag = 108 u, IF = 96500 C). What was the weight of oxygen gas liberated?

Since we do not ass any change in be sike2- C, we can infer that copper is not able to replace wine from zinc sulphate. But why? When zinc can replace copper in beaker 'A' why cannot copper replace zinc in beaker'C'?

Three electolytic cells A,B,C containing solutions of ZnSO_4 , AgNO_3 and CuSO_4 respectively are connected in series. A steady current of 1.5 amperes was passed throught them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

Why Zinc not extracted from Zinc oxide through reduction using CO?