If you attached the anode of an LED onto the Zn side and the cathode to the copper (in place of the voltometer - w/ 10ohm protection resistor in series) it will light up. This also makes it a great "circuit theory" lab. Most new engineers(and the DEA) still don't understand why they have to take Chemistry, well where do they think electricity from a battery comes from? The electrons oxidized from the solid Zinc must travel through the voltometer before they reach the copper cation to reduce it to solid copper. This is a redox reaction. (It may even be the solution to free energy that they need for their radar guns, if they stop throwing engineers in jail as suspected terrorists/drug dealers).
@@complexsimplelife199 BTW, batteries in our phones work on same principle but it can be recharged again by reversing the reaction with dc current(our charger)
Would it work with a smaller amount of each solution? If I wanted to make a series circuit, would I connect the beakers with more wires or more salt bridges, please?
the Zn decreases because he start turning to Zn(+2) which cannot exist as a solid and he become aqueous,and about the cu he increases since The Cu(+2) turn into Cu,who can become part of the "bar"
Zn has the tendency of oxidising into the solution of say solution ZnSO4 and forms Zn2+ ion that's why it's size decreases and say solution CuSO4 has the tendency to reduce itself into Cu2+ and deposits itself on Cu rod and thus it gains the size
Can we perform the same experiment with Copper (Cathode) in CuSO4 and Aluminium(Anode) in Aluminium nitrate? Kindly let me know if possible. Thanks in advance.
I have a question, here the voltmeter is coupled in series instead of parallel here. How does the current flow trough the voltmeter then? Isn't it a high-ohmic voltmeter? If so, the current in the circuit should be zero, and then according to the ohm law we shouldn't see any voltage loss. How can this be explained?
Well according to me, this experiment was simply shown to show how galvanic cell works in labs and how Salt bridge helps in continuous flow of current for a longer period of time. She didn't mention but it also concludes this:- Zn has the tendency of oxidising into the solution of say solution ZnSO4 and forms Zn2+ ion that's why it's size decreases and say solution CuSO4 has the tendency to reduce itself into Cu2+ and deposits itself on Cu rod and thus it gains the size
Hello. These videos are being used in Chem Lab. course at Middle East Technical University. Lab manual is provided by the department. So students can see what they should do in their lab day etc.
I have a question. Once you put the solution inside the glass tube salt bridge, did you block the holes with cotton wool? Tell me how did you do with that.
@@hussainmemon6563 , Salt bridge allows the flow back and forth of ions which keeps the concentration of ions in the cathode and anode relatively constant throughout the experiment.
This would have made a much better redox lab than just simply dipping solid Zinc into copper ion solution.(Who writes these boaring American college labs? -just kidding-)
after seeing this I understand more about the subject matter about voltaic cells
thank you very helpful 🙏
If you attached the anode of an LED onto the Zn side and the cathode to the copper (in place of the voltometer - w/ 10ohm protection resistor in series) it will light up. This also makes it a great "circuit theory" lab. Most new engineers(and the DEA) still don't understand why they have to take Chemistry, well where do they think electricity from a battery comes from? The electrons oxidized from the solid Zinc must travel through the voltometer before they reach the copper cation to reduce it to solid copper. This is a redox reaction. (It may even be the solution to free energy that they need for their radar guns, if they stop throwing engineers in jail as suspected terrorists/drug dealers).
You can power some legitimate things with this cell beyond that! It is not exactly portable though!
@Lana Lana Lana India's class 12 topic......we all know that
@@complexsimplelife199 our dry cell is portable
@@complexsimplelife199 BTW, batteries in our phones work on same principle but it can be recharged again by reversing the reaction with dc current(our charger)
But why the electrons must need to travel through voltmeter before they reach the copper cation?
Any neet aspirant here😀✋
🤚
Me too
Yaa
No
@@rishikeshpurohit9167 tuzse puchha hi nahi tha
Absolutely well done and definitely keep it up!!! 👍👍👍👍👍
love to see this shared by Turkish unis. To the top!!
Great topic for understend ing laboratory kind of exp. thermogalvanic cells for all kind of scientists and engineers.
Would it work with a smaller amount of each solution? If I wanted to make a series circuit, would I connect the beakers with more wires or more salt bridges, please?
Tebrik ederim güzel bir çalışma olmuş
Good job mrs, thank you.
may i include your video as part of my study video, for my students during this pandemic?
Thank you..
Yes, sure. You can use our videos as long as you give reference to METU OCW. Best.
@@METUOpenCourseWare thaks a lot,, :) sure,, i'll write reference of the video on description. Thank you.
Maam can you explain the final stage when the Zn plate decreases in size and Cu plate gains size?
the Zn decreases because he start turning to Zn(+2) which cannot exist as a solid and he become aqueous,and about the cu he increases since The Cu(+2) turn into Cu,who can become part of the "bar"
@@saritibi4247 ..now i got it...Thank you so much
@@saritibi4247 thanks ✨💝
Zn has the tendency of oxidising into the solution of say solution ZnSO4 and forms Zn2+ ion that's why it's size decreases and say solution CuSO4 has the tendency to reduce itself into Cu2+ and deposits itself on Cu rod and thus it gains the size
@@nayan5612 thanks Priya 😊
Very easy to understand.. loved it ❤️
Nice...you people are really doing a great job for humanity it will help lot of students
Thankyou ❤
Nice Experiment
Keep it up 🥰
❤❤
Thanks for your help and support
Can u use filter paper as a replacement for salt bridge
Thanks 🙏
Can we perform the same experiment with Copper (Cathode) in CuSO4 and Aluminium(Anode) in Aluminium nitrate? Kindly let me know if possible. Thanks in advance.
I have a question, here the voltmeter is coupled in series instead of parallel here. How does the current flow trough the voltmeter then? Isn't it a high-ohmic voltmeter? If so, the current in the circuit should be zero, and then according to the ohm law we shouldn't see any voltage loss. How can this be explained?
It won't as the electricity will be the same in parallel and series
Thanks....
Do you have worksheet for this experiment?
Awesome 👍😊
Hello..
May i Include/use this Experimental Video in our Regional Language[malayalam(in india) ] high School Level Class Video ..
Hello. Of course. You can use if you give reference to us.
adipolii
very very thanks...
What is the cost of salt bridge?
You could just build your own, no reason to buy such a salt bridge
Unless u got bank
You can just use a paper towel soaked in salt water if you just want to obtain a voltage.
Why noone show the ampere
Does anyone know the dimension? the mass of the metal strips??
zeg es wa het verschil is tussen het koper en het zinkplaatje in gedestilleerd water met zoutburg
Thanks
is their anyy function of KSO4
Yess
it acts as a electrolyte to connect the solutions
It neutralise the excess accumulated charge in both the beakers..
What are the objectives of this video?
Well according to me, this experiment was simply shown to show how galvanic cell works in labs and how Salt bridge helps in continuous flow of current for a longer period of time. She didn't mention but it also concludes this:- Zn has the tendency of oxidising into the solution of say solution ZnSO4 and forms Zn2+ ion that's why it's size decreases and say solution CuSO4 has the tendency to reduce itself into Cu2+ and deposits itself on Cu rod and thus it gains the size
Salt bridge contains which solution and what molarity
can be NaCl, KNO3 ok...
KCl is the best salt bridge because it doesn't react with the ions that it transfers. And salt bridge is in solid fotm not in aqeous form.
Raju seeram potassium chloride kcl is best
😊😊😊😊
thankssss
Great
What are the precautions in this experiment to get the most accurate result?
Hii
Super
Best
Nice
What is a salt bridge made of? Is it just a hollow tube?
Jepril Peña No, it isn't. Usually some sort of jelly with salts added in the making.
It's inert electolyte
No it is made up of inhert electrolyte like K2So4, KNO3, KCl
Could I use the graphite from pencil lead in place of the jelly salt bridge?
Jepril Peña Made of KCl
Neat
👏👏👏👏👏👏
Music in the video?
Will Watson it’s listed in the end credits. Michael Fix, Will I or Won’t I
👍👍👍👍
Aa odtü
Can someone tell me what's the objective of this video? Also the conclusion?
Hello. These videos are being used in Chem Lab. course at Middle East Technical University. Lab manual is provided by the department. So students can see what they should do in their lab day etc.
What is the salt bridge made of?
Glass
Are the solution must contain 0.5 M
Raju seeram
The lesser the molarity is, the faster the reaction will proceed.
Raju seeram ... are you a sick??
Not necessay
NO it depends to your solution but the best concentration in this type of experments is using 1M of solution
I have a question. Once you put the solution inside the glass tube salt bridge, did you block the holes with cotton wool? Tell me how did you do with that.
You leave it to harden (outside or even in the fridge). If you don't harden it, the solution will fall inside the beakers.
salt bridge make the solution nutral and to make close cirute
Salt bridge don't make a close circuit
@@hussainmemon6563 , Salt bridge allows the flow back and forth of ions which keeps the concentration of ions in the cathode and anode relatively constant throughout the experiment.
This would have made a much better redox lab than just simply dipping solid Zinc into copper ion solution.(Who writes these boaring American college labs? -just kidding-)
حلوو😍😍
10yıl önceki bilgileri zorla öğreten bizim bu eğtim sisteminde ##₺#@##
ആ
B''H, Christ, Jesus, Amen.
Thanks
Thanks...
Thanks
Thanks