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The electrochemical equivalent of silver is 0.0012g/C…

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The electrochemical equivalent of silver is 0.0012g/C if 36.0g of silver is to be deposited by electrolysis on a surface by passing a steady current for 5.0 minutes, the current must be

A. 6000A

B. 100A

C. 10A

D. 1.0A

QUICK ANSWER…

B

DETAILS…

M = ZIT

Where M = mass of silver deposited = 36g

Z = electrochemical equivalent of silver = 0.0012g/C

I = current flowing through the electrolyte =?

And T = time duration of the electrolysis = 5 minutes = 5 X 60 = 300s

ZIT = M,

I = M/ZT = 36/(0.0012 X 300) = 36/0.36 = 100A

Now for the right answer to the above question:

  1. Option A is incorrect. the time must be in seconds and not in minutes.
  2. Option B is correct.
  3. C is incorrect.
  4. D is not the correct answer.

HELPFUL TIPS…

You may please note these/this:

  • Solving with time as 5 minutes without conversion to seconds will give 6000A, this is wrong, the time should be in seconds.
  • No need to convert the mass from g to kg, this is because the electrochemical equivalent of silver is given in terms of g.
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/ culled from 2016 JAMB-UTME physics past question 30 /

The electrochemical equivalent of silver is 0.0012g/C... » QuizTablet
The electrochemical equivalent of silver is 0.0012g/C... » QuizTablet

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