During electrolysis of a solution of AgNO3, 9650 coulombs of charge is passed through the solution. What will be the mass of silver deposited on the cathode?

Question

During electrolysis of a solution of AgNO3, 9650 coulombs of charge is passed through the solution. What will be the mass of silver deposited on the cathode? (A) 108 g (B) 10.8 g (C) 1.08 g (D) 216 g

Tardigrade Admin · Accepted Answer

Ag+ + underset text1Fe- → underset text108 gAg Amount of Ag deposited by 9650 C =(108/96500)×9650 =10.8 g

Q. During electrolysis of a solution of $A g N O_{3}$ , $9650$ coulombs of charge is passed through the solution. What will be the mass of silver deposited on the cathode?

$108 g$

$10.8 g$

$1.08 g$

$216 g$

$A g^{+} + 1F e^{-} \to 108 g A g$
Amount of Ag deposited by $9650 C$
$= \frac{108}{96500} \times 9650$
$= 10.8 g$

Q. During electrolysis of a solution of AgNO3​, 9650 coulombs of charge is passed through the solution. What will be the mass of silver deposited on the cathode?

108g

10.8g

1.08g

216g