SATHEE: Redox Reactions And Electrochemistry Ques 636

Redox Reactions And Electrochemistry Ques 636

Question: 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 $80 c m^{2}$ and 0.005 mm thick layer. Density of Ag is $10.5 g, c m^{- 3}$

Options:

A) 125.1 seconds

B) 12.5 seconds

C) 155.2 seconds

D) 200 seconds

Show Answer

Answer:

Correct Answer: A

Solution:

[a] $V o l u m e = A r e a \times t h i c k n e s s$ $M a s s = V o l u m e \times d e n s i t y$
$∴$ Mass of Ag to be deposited $= \frac{80 \times 0.005}{10} \times 10.5 = 0.42 g$ $A m o u n t d e p o s i t e d = \frac{i \times t \times E . w t}{96500}$
$∴ 0.42 = \frac{108 \times 3 \times t}{98500} ∴ t = 125.1, s e c o n d s$

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Redox Reactions And Electrochemistry Ques 636

Question: How long a current of 3 amperes has to be passed through a solution of AgNO3 to coat a metal surface of 80cm2 and 0.005 mm thick layer. Density of Ag is 10.5g,cm−3

Options:

Answer:

Solution:

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Question: 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 $80 c m^{2}$ and 0.005 mm thick layer. Density of Ag is $10.5 g, c m^{- 3}$