`0.1F` charge is supplied to a solution of `Ni(NO_(3))_(2)`. Then the amount of `Ni` deposited (in mol) at the cathode will be:

When 0.1 Faraday of electricity is passed in aqueous solution of AlCl_(3) . The amount of Al deposited on cathode is

When 0.1 Faraday of electricity is passed in aqueous solution of AlCl_(3) . The amount of Al deposited on cathode is

A current of 3.7 ampere is passed for 6 hours between platinum electrodes in 0.5 litre of a 2 M solution of Ni(NO_(3))_(2) . What will be the molarity of the solution at the end of electrolysis ? What will be the molarity of the solution if nickel electrodes are used ? (1 F=96500 coulomb, Ni=58.7)

A current of 3.7 A is passed for six hours between Ni electrodes in 0.5 L of 2M solution of Ni(NO_(3))_(2) . The molarity of solution at the end of electrolysis will ___________.

A current of 3.7 A is passed for 6hrs. Between Ni electrodes in 0.5 L of 2 M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis?

Calculate the amount of electricity required to deposite 1 mol Cu atom at the cathode.

A strip of nickel metal is dipped in a 1 molar solution of Ni (NO_(3))_(2) and a strip of silver metal is dipped in a 1 molar solution of AgNO_(3) . An electrochemical cell is created when the two solutions are joined by salt bridge and two strips are joined by wire to a voltmeter. Answer the following questions. Calculate the cell potential (E_("cell")) at 25^(@)C for the cell if the initial concentration of Ni (NO_(3))_(2) , is 0.100 molar and the initial concentration of AgNO_(3) is 1.00 molar. [E_(Ni^(2+)//Ni)= -0.25V, E_("Ag^(+)//Ag)=0.80V, log 10^(-1)= -1]

0.35 mole of electron was passed through AgNO_3 solution. Calculate amount of Ag metal deposited at the cathode.