i) According to the equation `Cu^(2+)+2e^(-)rarrCu`, how many moles of copper are deposited when 965C of electricity is passed through a solution of `Cu^(2+)` ions?
`(1F=96500 C)`. 

How does ammonia reacts with a solution of Cu^(2+) ?

What weight of copper will be deposited by passing 2 Faradays of electricity through a cupric salt ( At wt. of Cu = 63.5 ) ?

Find the mass of copper deiposited on cathode when a current of 1.5A is passed through copper sulphate solution for 5 minutes (At. Mass of Cu=63.5).

How many faraday of electricity is required to reduce 1 mole of MnO_(4)^(-) ions to Mn^(2+) ions?

How many coulombs of electricity are consumed when a 100 mA current is passed through a solution of AgNO_(3) for half an hour during an electrolysis experiment ?

When a quantity of electricity is passed through CuSO_(4) solution, 0.16 g of copper gets deposited. If the same quantity of electricity is passed through acidulated water, then the volume of H_(2) liberated at STP will be [given : at.wt. of Cu = 64].