When `6.25 times 10^18e^-` are passed through aqueous Silver nitrate, '0.00112' grams of Silver is deposited. Then electrochemical equivalent of Ag is `"x times 10^-3` then `"x"` =

If 0.5 amp current is passed through acidified silver nitrate solution for 10 minutes. The mass of silver deposited on cathode, is (eq. wt. of silver nitrate = 108 ).

A current o f1.5 A is passed through a silver voltameter for 35 minutes .The mass of silver deposited during electrolysis is 3.528 g Calculate the electrochmical equivalent of silver.

The charge equivalent to 6times10^(18) electrons is .

One ampere current flows for one minute through a silver voltameter. It deposits 0.067 g of silver on the cathode. Calculate (i) the electrochemical equivalent of copper. (ii) how much charge will flow to deposited 108 g of silver ? (iii) how much charge is carried by a silver ion ? ( Avagadro's number, N =6.024xx10^(23) ).

X is a divalent metal. The value of its electrochemical equivalent is 5.25xx10^(-4) g. Its atomic mass will be:

Two voltameters, one of copper and another of silver, are joined in parallel. When a total charge q flows through the voltameters, equal amount of metals are deposited. If the electrochemical equivalents of copper and silver are Z_1 and Z_2 respectively the charge which flows through the silver voltameter is