0
You visited us 0 times! Enjoying our articles? Unlock Full Access!
Question

Three electrolytic cells A,B,C containing solutions of ZnSO4,AgNO3 and CuSO3, respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

Solution
Verified by Toppr

Cell B: Ag++eAg at cathode.
1 mole (108 g) of Ag is deposited by 96500 C.
1.45 g of Ag will be deposited by 96500×1.45108=1295.6C.
Now,
Q=It
1295.6=1.5×t
t=864s
Cell A: Zn2++2eZn
2 moles of electrons (2×96500 C of current) produces 1 mole (63.5 g) of zinc.
1295.6 C of electricity will deposit 65.32×96500×1295.6=0.438 g of zinc
Cell C: Cu2++2eCu
2 moles of electrons (2×96500 C) of current will produce 1 mole (63.5 g) of Cu.
1295.6 C of current will deposit 63.5×1295.62×96500=0.426g of copper

Was this answer helpful?
120
Similar Questions
Q1
Three electrolytic cells A,B,C containing solutions of ZnSO4,AgNO3 and CuSO3, respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?
View Solution
Q2

Three elctrolytic cells A,B,C containing solutions of ZnSO4,AgNO3 and CuSO4 respectively are connected in series. A steady current of 1.5 ampere was passed through them until 1.45 g of silver deposited at the cathode3 of cell B. How long did the current flow ? What mass of copper and zinc were deposited ? [Atomic masses; Cu = 63,5, Zn = 65.3; Ag = 108]

View Solution
Q3
Three electrolytic cells A, B and C containing electrolytes ZnSO4, AgNO3 and CuSO4 respectively were connected in series. A steady current of 1.50 ampere was passed through them until 1.45 of Ag were deposited at the cathode of cell B. How long did the current flow? What mass copper and zinc were deposited? (Atomic weight of Cu=63.5, Zn=65.3, Ag=108)
View Solution
Q4
Two electrolytic cells containing silver nitrate & copper sulphate solution are connected in a series. The steady current of 2.5A was passed thought them till 1.018g of silver were deposited. How long did the current flow & what is the mass of Cu deposited?
View Solution
Q5
(a) A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO4 and ZnSO4 until 2.8g of Fe deposited at the cathode of cell X .How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y . ( Molar mass :Fe=56g/mol ,Zn=65.3g/mol ,1 F=96500C/mol)

(b) In the plot of molar conductivity (Λm) vs square root of concentration (C)1/2 following
curves are obtained for two electrolytes A and B :
View Solution