I recently carried out a laboratory experiment for my general chemistry 2 lab to
ID: 975507 • Letter: I
Question
I recently carried out a laboratory experiment for my general chemistry 2 lab to experimentally determine the faraday constant. It involved the redox reaction Cu(s) + 2H+(aq)-->Cu2+ + H2(g). We used an electrolytic cell and collected H2 gas in a buret. Then, we proceeded to calculate the partial pressure of H2 gas, the ideal gas law to calcualte moles of H2 gas, then e- transferred and so on. I am currently trying to determine at least two possible sources of error for this experiment and how they would affect the determined faraday constant? (i.e. would it be higher or lower). Thank you in advance for any assistance or direction you can give.
Explanation / Answer
Per mole of Cu to convert to Cu2+ requires the release of 2 electrons and thus 1 mole of H2 is formed.
Now,
Faraday's constant = charge required for transfer/acceptance of 1 mole of electron to take place.
If number of electron transfer taking place is assumed higher,Faraday's constant will be calculated higher and vice versa.
If moles of H2 formed is higher, the Faraday's constant will be calculated higher and vice versa.