CBSE Class 12 Chemistry 2017 Delhi Set 1 Solved Paper

Question : 12 of 26

Marks: +1, -0

(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}, 1 {\F}=

96500 {\C} {\mol}^{-1}

)
(b) Define fuel cell.

Solution:

(a)

\;t=900 {\ s}

\;\;\text " Charge "\;=\;\text " Current "\; × \;\text " Time "\;

=2 × 900

\;=1800 {\C}

According to the reaction

{\Ag}^{+} \;\text "(aq) "\;+ {\e}^{-} → {\Ag}( {\ s})

We require

1 {\F}

to deposit

1 {\mol}

108 {\g}

{\Ag}

For

1800 {\C}

, the mass of

{\Ag}

deposited will

\;\text " be "\;=\;{108 × 1800}/{1 × 96500}=2.0145 {\g}

(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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