How long a current of 3 amperes has to be passed through a solution of AgNO3 to coat a metal surface of 80 cm2 with a 0.005 mm thick layer. (Density of Ag is 10.5 g cm- 3 ).

Question

How long a current of 3 amperes has to be passed through a solution of AgNO3 to coat a metal surface of 80 cm2 with a 0.005 mm thick layer. (Density of Ag is 10.5 g cm- 3 ). (A) 125.09 sec (B) 1.251 sec (C) 12.51 sec (D) 12.61 sec

Tardigrade Admin · Accepted Answer

Weight of Ag deposited = Volume × density =(.Area× thickness.)× density =80× 5× 10- 11× 10.5=0.42 g t=(W × F/E × i)=(0.42 × 96500/108 × 3)=125.09 sec.

Q. How long a current of 3 amperes has to be passed through a solution of $A g N O_{3}$ to coat a metal surface of 80 $c m^{2}$ with a 0.005 mm thick layer. (Density of Ag is 10.5 g $c m^{- 3}$ ).

125.09 sec

1.251 sec

12.51 sec

12.61 sec

Weight of Ag deposited = Volume $\times$ density

$= (A re a \times t hi c kn ess) \times d e n s i t y$

$= 80 \times 5 \times 1 0^{- 11} \times 10.5 = 0.42$ g

$t = \frac{W \times F}{E \times i} = \frac{0.42 \times 96500}{108 \times 3} = 125.09$ sec.

Q. How long a current of 3 amperes has to be passed through a solution of AgNO3​ to coat a metal surface of 80 cm2 with a 0.005 mm thick layer. (Density of Ag is 10.5 g cm−3 ).