1. Exactly 0.200 mole electrons is passed through two electrolytic cells in series. One contains silver ion, and the other, zinc ion .assume that the only cathode reaction in each cell is the reduction of the ion to the metal. How many grams of each metal will be deposited? (at. Mass of zn = 65, ag = 108) a. 108g ag and 65 g zn. b. 108 ag and 32.5g zn. c. 21.6 ag and 6.5 g zn. d. 21.6 g ag and 13 g zn. 2. A steady current of 30.0A for 70.2 min corresponds to a passage of a. 1.26 10^5 electrons. b. 1.26×10^5 f. c. 1.31 f. d. 1.31 c. 3. Cu+ is not stable and undergoes disproportion. E for cu+ disproportionation. (E ° cu2+/cu =0.153V , E ° cu+/cu=0.53V).

							
Hi
Ans 1: 
For silver , the conversion is Ag+ + e- -> Ag
Therefore 1 mole of electrons are reqd to make 1 mole i.e 108 gm of silver. hence .2 moles of electron will make .2x108 = 21.6 gm of silver.
 
For zinc, the connversion is Zn2+ + 2e- -> Zn
Therefore 2 moles of elctrons are reqd to make 1 mole i.e 65 gm of zinc, hence .2 mole electrons shall make .2x65/2 = 6.5 gm of zinc.
						

							
Hi
Ans 2:
For a steady flow, the current I in amperes can be calculated with the following equation:
 
where
Q is the electric charge in coulombs transferred 
t is the time in seconds 
More generally, electric current can be represented as the time rate of change of charge, or
. 
therefore, Q= 30 A x 70.2 x 60 sec = 126360 coulombs
1 faraday = 96 485.3415 coulombs
 
Therefore answer is 126360/96485.3415 = 1.31 faraday
						

							
Hi
Please repost the third question, the question is not clear.
						

							
1)       for silver deposition :       Ag+     +     e-             ------>   Ag
                                                                     1 mole                   1 mole
         so , 0.2 moles of Ag is deposited i.e., 0.2*108 = 21.6 grams
        
         for zinc deposition :   Zn2+     +   2e-                ------>    Zn
                                                              2 mole                       1 mole
        so , 0.1 moles of Zn is deposited i.e., 0.1*65 =  6.5 grams
        So option is C
 
2)   Electric current is the rate of charge flow past a given point in an electric circuit, measured in Coulombs/second which is named Amperes
     so Q = i*t
       Q=30*70.2*60
     Q = 126360 Coulombs
    but 1 faraday = 96485 Coulombs
    So its Q = 1.31 faraday
    So option is C
 
 
3) I want to make a small correction to question reg. elecric potential of  cu2+/cu+ ( taken frm standard books )



Its cu2+/cu+ =0.153V  i.e.,                     cu2+ + e-   ------>  cu+            E0 = 0.153 V



Now going into problem:  Cu+ solutions, tend to give a disproportion reaction:



                                                       2Cu+ ----- >   Cu + Cu2+



                       

                     cu+ + e-    ------>  cu                                E0 = 0.53 V        so,  nE0 = 0.53 V    



                     cu+            ------>  cu2+ + e-               E0 = - 0.153 V       so,   nE0 = - 0.153 V 



on adding above rxns we get   

 2Cu+ ----- >   Cu + Cu2+                  with  E0 = +0.377 V