CBSE Class 12 Chemistry 2017 Delhi Set 1 Solved Paper

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Question : 12
Total: 26
(a) Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO3 for 15 minutes.
(Given : Molar mass of Ag=108gmol1,1F= 96500Cmol1 )
(b) Define fuel cell.
Solution:  
(a) t=900 s
Charge = Current × Time =2×900 =1800C
According to the reaction
Ag+(aq) +eAg( s)
We require 1F to deposit 1mol or 108g of Ag
For 1800C, the mass of Ag deposited will be =
108×1800
1×96500
=2.0145g

(b) Fuel cell is the name given to the galvanic cells which are designed to convert the energy of combustion of fuels like hydrogen, methane, methanol, etc. directly into electrical energy.
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