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### Topic: Electrochemistry Problem  (Read 469 times)

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#### hilsenna

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##### Electrochemistry Problem
« on: July 31, 2020, 06:19:39 AM »
Hello,

I have tried to use Faraday formula here, but i cannot solve it probably because of wrong inputs. Answer is supposed to be 0,02 F. Would be appreciated if you guys could help me.

Q: In the electrolysis of 200 ml of 0.15 mol/l CuSO4 solution using platinum electrodes, 0.16g of oxygen gas evolved to the anode. How many faradays of charge was passed through the solution? (Atomic weights: H:1.0, O:16.0, S:32.0, and Cu:63.5)

Photo shows how i tried to solve the question

#### mjc123

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##### Re: Electrochemistry Problem
« Reply #1 on: July 31, 2020, 10:17:32 AM »
That is not at all clear. What are the quantities in your equations?
Why don't you do it the simple way? (hint: you don't need the moles, or mass, or ANYTHING to do with the copper sulfate. You mustn't assume it all reacts!)

#### hilsenna

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##### Re: Electrochemistry Problem
« Reply #2 on: July 31, 2020, 12:46:39 PM »
That is not at all clear. What are the quantities in your equations?
Why don't you do it the simple way? (hint: you don't need the moles, or mass, or ANYTHING to do with the copper sulfate. You mustn't assume it all reacts!)

OOOH okay, Should we say 0,16 gr oxygen is equal to 0,005 moles. While water releases oxygens, it also releases 4e- at the same time. Thus, 4*0.005=0.02 moles which is also equal to 0.02 F, right?

#### mjc123

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##### Re: Electrochemistry Problem
« Reply #3 on: August 01, 2020, 04:06:58 PM »
Correct.