##### Admin

**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:**

**Option A is incorrect. the time must be in seconds and not in minutes.****Option B is correct.****C is incorrect.****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.**

**You can freely add your own answers below or click the golden ASK A QUESTION BOTTON down this page to raise new related questions… OUR COMMUNITY OF EXPERTS WILL BE MORE THAN HAPPY TO TACKLE IT…**

**/ culled from 2016 JAMB-UTME physics past question 30 /**

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