Home
Class 12
CHEMISTRY
Calculate the mass of Ag deposited at ca...

Calculate the mass of Ag deposited at cathode when a current of 2 ampere was passed through a solution for 15 minutes.

Text Solution

Verified by Experts

The correct Answer is:
2.014 g
Reaction at cathode is :
`underset(1F(1xx96500" C"))(Ag^(+)(aq))+e^(-) to underset(1" mol"(108 g))(Ag(s))`
96500C of charge is required to deposit Ag=108 g.
1800 C of charge required to deposit `Ag=(108 g)xx((1800 C))/((96500C))=2.014 g`.
Promotional Banner

Topper's Solved these Questions

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise COMPLETION QUESTION|2 Videos

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise NCERT In-Text Questions|9 Videos

  • ALDEHYDES AND KETONES

    DINESH PUBLICATION|Exercise Interger|5 Videos

Similar Questions

Explore conceptually related problems

(a) Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO_(3) for 15 minutes (Given : Molar mass of Ag = 108 g mol^(-1) 1F = 96500 C mol^(-1) ) (b) Define fuel cell

the Amonut of Ag (atomic mass =108) deposited at the cathode when a current of 0. amp is passed through a solution of Ag CO_(3) for 1 hour is closest to

Calculate the time to deposit 1.5 g of silver at cathode when a current of 1.5 A is passed through the solution of AgNO_(3) .

How much copper is deposited on the cathode if a current of 3A is passed through aqueous CuSO_(4) solution for 15 minutes?

The mass of Cl_(2) produced when 1A current is passed through NaCl solution for 30 minute is

The amount of metal deposited at cathode on passing electric current of 0.75 ampere in aqueous ferris sulphate solution for 30 mintes, will be. (atomic weight of Fe=56)