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(a) Calculate the mass of Ag deposited a...

(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

Text Solution

Verified by Experts

Time, `t = 15 xx60 = 900` sec,
Charge = Current `xx` Time
`= 2A xx 900s = 1800 C`
According to the reaction,
`Ag^(+)(aq) +e^(-) to Ag(s)`
So, we need 1F or 96500 C to deposit one mole or 108 g of silver, so, by 1800 C, the mass of silver deposited would be:
`=108"g mol"^(-1) xx (1800C)/(96500"C mol"^(-1))`
`=2.014g`
So, 2014 g of silver is deposited in 15 minutes.
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