State Farday's first law of electrolysis. For the electrode reaction `Zn^(+2)+2e^(-)rarrZn_((s))`, what quantity of electricity in coloumbs is required to deposite one mole of zinc. 

State the Faraday's first law of electrolysis. How many Faraday of electricity is required for the reduction of 1 mole of Mg^(2+) ions?

The amount of electricity required to deposit 0.9 g of aluminium when the electrode reaction is : Al^(3+) + 3e^(-) rarr Al (atomic mass of Al=27 )

100mL of 0.3 M Fe^(3+)(aq) ions were electrolyzed by a charge of 0.072F. In electrolysis, metal was deposited and O_(2)(g) was evolved. At the end of electrolysis, it is desired to oxidize the un - electrolyzed metal ion. Fe^(3+)+e^(-) rarrFe^(2+) Fe^(2+)+2e^(-)rarrFe The moles of Fe^(2+) ions left un - electrolyzed in the solution is a. 0.009" "b.0.021" "c.0.072" "d.0.042

For the cell reaction Zn(s) + Cu^(2+)(aq) rarr Cu(s) + Zn^(2+)(aq) E_("cell")^(@) = 1.10 V, DeltaG^(@) is :

For the cell reaction Zn(s) +Cu^(2+)(0.1M) rarr zn^(2+)(0.01M) + Cu(s) , If E^(@) is the strandard e.m.f. of the cell, then

(a) What type of a battery is the lead storage battery? Write the anode and the cathode reactions and the overall reaction occuring in a lead storage battery when current is drawn from it. (b) In the button cell, widely used in watches, the following reactions takes place: Zn(s)+Ag_2O(s)+H_2O(l) to Zn^(2+) (aq)+2OH^(-) (aq) Determine E^@ and Delta G^@ for the reaction: