Calculate the time to deposit `1.17g` of nickel at cathode when a current of `5A` was passed through the solution of `Ni(NO_(3))_(2)`. [Molar mass of `Ni=58.5g`, `F=96500C`]

Calculate the time required to deposit 1.27 g of copper at cathode when a current of 2A was passed through the solution of CuSO_(4) . ("Molar mass of "Cu=63.5g mol^(-1), 1F =96500 C mol^(-1)).

(a) Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO_(3) for 15 minutes (Given : Molar mass of Ag = 108 g mol^(-1) 1F = 96500 C mol^(-1) ) (b) Define fuel cell

How many moles of Pt may be deposited on the cathode when 0.80F of electricity is passed through 1.0M solution of Pt^(4+) ?

The atomic weight of Al is 27 . When a current of 5F is passed through a solution of Al^(+++) ions, the qeight of AL deposited is.

Mass of Nickel deposuited at cathode by passing 9.65 ampere of current for a period of 100 inute through molten NiCl_2 is (Atomic mass of Ni = 58.7 u)

The number of moles of Zn^(2+) ions deposited when a current of 1.5A is passed for 4 hours through a molten solution of a zinc salt. ( Assume current efficiency to be 90%)

Find out the oxidation state of tin in its salt, when 11.0 g of deposited when a current of 1.0 A is passed for 5 hours through molten salt. (Given atomic weight of tin = 119)

A current was passed for two hour through a solution of an acid that liberated 11.2 litre of oxygen at NTP at anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same time?

A current of 5.00 A flowing for 30.00 min deposits 3.048 g of zinc at the cathode. Hence, equilvalent mass of zinc is:

0.169 gram of copper is deposited on the cathode by a current of 32 milliamperes passing for 5 hours through a solution of copper sulphate. Determing the current efficiency. [ Atomic weight of Cu=63.6]