Inthe electrolysis of `AgNO_3` solution 0.7g of Ag is deposited after a certain period of time.Calculate the quantity of electricity required in coulomb. Molar mass of Ag is `107.9 g mol^(-1)`.

In the elctrolysis of AgNO_3 solution 0.42g of Ag is produced of cathode after o certain period of time. Calculate the quantity of electricity required (molar weight of Ag is 107.9 g mol^-1)

Calculate the volume in litres occupied by 7.4g of ammonia at STP(molar mass of NH_3 = 17 g mol^-1 ).

How long will it take to produce 2.415 g of Ag metal from its salt solution by passing a current of 3A?Howmany molesof electrons are required? Molar mass of Ag is 107.9 g mol^(-1) .

In a certain electrolysis experiment 0.79 g of Ag was deposited in one cell containing aqueous AgNO_3 solution, while 0.231 g of an unknown metal X was deposited in another cell containing aqueous XCI_2 solution in series with AgNO_3 cell. Calculate the molar mass of X. Molar mass of Ag is 107.9 g mol^(-1) .

Solubility product of AgCl is 1.8 xx 10^(-10) . Calculate its molar solubility and solubility in g/L. Molar mass of AgCl is143.5 g mol^(-1) .