Daniell Cell
This experiment demonstrates a copper-zinc cell (Daniell cell), as an example of a of electrochemical cell. A zinc sheet and a copper sheet are put into their appropriate ion solution: Zinc into zinc sulphate and copper into copper sulphate. Zinc is less noble than copper and the solution tension is higher. Thus, a relatively large number of zinc ions enter the solution at the zinc sheet, i.e., zinc atoms are oxidized to zinc ions. The electrons remain in the zinc sheet (surplus of electrons), which is charged negatively. On the other hand, only a few copper ions detach themselves from the copper sheet. Electrons flow to the copper sheet via the cable that connects the metal sheets to a voltmeter. The copper ions of the copper sulphate absorb these electrons and attach to the sheet as solid copper, i.e., the copper is reduced. Since positive zinc ions are in the solution on the left and copper is deposited on the right, a charge equalization must take place. To allow such an electric current, both half-cells are connected with a salt bridge - realized by a paper towel dipped in sylvite. Sulphate ions move to the left and zinc ions to the right.
This is an experiment from the first-semester lecture "Electricity and Magnetism" given by Christian Bettstetter in the bachelor program "Informationstechnik" at the University of Klagenfurt, Austria.
Link to the lecture: bettstetter.com/teaching/epgi/
Video made by Judith Wieser.
Text by Christian Bettstetter and Judith Wieser.
Supported by Stefan Amlacher in the laboratory of HTL Mössingerstraße, Klagenfurt.
(c) 2021 Universität Klagenfurt
Пікірлер: 29
Perfect explanation ❤
you helped a lot ❤
Awesome 👍😊
Thanks brother ❤️ helped a lot ✨
Thanks!!
Thank u so much❤ I was unable to understand this topic
Thanks
Is copper electrode compulsory? We use copper ions to reduce but missing the importance of copper electrode
Nice
Ty
It was informative and I learn more concept from the textbook of my college thanks ❤️❤️
Hi, I repeated the same experiment for a school project, but only got a multimeter reading of 0.61V. I utilized a KCl salt bridge and sanded the electrodes before use. Could you give any insights as to why it was lower?
@bettstetter
2 жыл бұрын
Which concentrations of the solutions did you use?
@anish9411
2 жыл бұрын
@@bettstetter Both concentrations were 0.5M.
@bettstetter
2 жыл бұрын
@@anish9411 We took 0.1 mol/l for the zinc and copper sulfate solution, more common is 1 mol/l. I am not sure exactly what concentration we took for the KCl, but our study assistant thinks 0.5 mol/l (it must be higher than the concentration of the zinc and copper sulfate solutions).
@anish9411
2 жыл бұрын
@@bettstetter I was able to fix it. I initially used electrode rods with a very small surface area, and the electrode plates performed much better instead. Thanks anyways!
@philosophic-gajar
3 ай бұрын
Why not use the salt bridge of NaCl instead of KCl
What a experiment by you😯😯😯😯😲😲😲😲😳😳
Why did Copper gained electron because we were told metals Only Lost electron?
@krrishjoshi83
Жыл бұрын
The standard electrode potential is higher for copper that's why copper experienced reduction while zinc was oxidised Or you can understand it through by Zinc is more reactive than copper
@lakshyakamal1748
Жыл бұрын
It is not the copper atom on the electrode that gains electrons but the Cu+2 ions in the solution get reduced to Cu atoms.
لطيف
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2:00 who wrote this 🤣