Harry_-

Sorry I don't have lots of time to write a reply at the moment I'm working on a lab. However if you can find the redox potentials for the cell you could use: ΔGo= nFE n is the number of moles used in the balanced equation F is faraday's constant of 96500 Cmol-1 E is your cell potential under standard conditions (reduction - oxidation potentials) If you need help ask or there are lots of good online videos on that equation. Regards, Harry

Thanks so much. I'm preparing a lab experiment and can't really reference that, are there any papers that I could use? Also I notice that the yield for that experiment is 72% whereas without ammonium nitrate and with a lot more cupric acetate monohydrate the yields on the other paper are 90%. Why is this?

They say nitric acid can be used but nothing about ammonium nitrate

What about the ammonium Nitrate. I can't find any papers on it being used in this reaction

Does anyone know how this reaction proceeds with the following reactants? Glacial acetic acid (i presume solvent) Cupric acetate monohydrate Ammonium Nitrate

Hello, I'm researching into the 2019 Nobel Prize for chemistry, and therefore lithium ion batteries. Wittingham's battery was a lithium anode, a titanium disulfide cathode and a lithium perchlorate in dioxolane electrolyte. I have always thought that batteries rely on a displacement reaction split into two halves. However in animations that I have seen show the electrons at the cathode being picked up by the very lithium ions that released them and that have just moved from the anode to the cathode. This doesn't make sense to me as if the lithium is picking up the electrons it just gave away what was the cause for this reaction to take place? I would have expected the electrons to be picked up by the electrolyte. What is happening here? Any help would be greatly appreciated, Harry

Yes, I did take these into account, I can't remember what the exact values were for each compound but I used the value on the bottle. However if the bottles were contaminated/ not pure (very possible as I was using school chemicals which students in practicals can just scoop out what they need directly from the bottle using a spatula) wouldn't this cause my entire gradient to be off as in dilution I wouldn't be making the concentrations of the solutions I thought I was making. I also was only using a 2 d.p scale (only one I have) so I cannot expect each solution to be the exact same concentration.

This is also weird to me as if the electrometer was in parallel, I would expect a slightly lower value for standard emf (due to the lost volts not completely being cancelled out by the resistor) however if the electrometer was in series I would have expected a very precise value of E0. What if the ZnSO4 or my CuSO4 wasn't perfectly pure therefore each of my subsequent solutions were slightly off so even my standard emf (if [reducing agent] was larger than [oxidising agent]) would be lower than expected. As I added water to my solutions to make them more dilute this could have changed the shape of my graph. I'm also having a hard time believing I would put a voltmeter in series 😂

Unfortunately I do not have the equipment anymore. My circuit drawing is setup for measuring current and not voltage, It has been a while since I did this experiment so I'm not sure if I put the electrometer in series with the resistors or if I set it up the correct way. Its embarrassing I know. However, even if my electrometer was in series with the resistor (100M Ohm) the voltmeter's impedance is 5x1013. Compared with 100x106 of my resistor in series, shouldn't this mean that my results should still be accurate to the degree that I have.

My concentrations that I wanted to use started at molarity 2 and were tested against the other electrolyte of molarity 1.5 and 1. I had an issue with creating 2 molarity solutions and the solutions were saturated, so I doubled the volume to make molarity 1 solutions as a start. I could be possible that I made up the solutions wrongly as I was working very fast

Standard Electrode potentials: Zinc= -0.76 copper= 0.34 (both of these should account for the reaction using/ taking 2 moles of electrons) 0.34--0.74=1.1v It is weird that I am pretty much exactly a factor of 2 off, which is why it makes me believe that iit is a calculation error rather than a practical one. For example, if I was only using 1 mole of electrons in the balanced ionic equation my value for F would be perfect. Here is the electrometer I used's manual: http://physics-astronomy-manuals.wwu.edu/Keithley 614 Electrometer Manual.pdf Here is a diagram of the apparatus setup, the electrometer being in series shouldn't be a problem should it? I assumed it had internal parallel circuits to record voltage as it also records current. Finally, my x-axis was ln([Oxidising Agent] / [Reducing Agent])

I'm not sure what you mean by 'zero point' please could you expand. I used my electrometer to measure the voltage, it was zero-checked before the experiment and then connected to my circuit. What do you believe to be off in the recorded voltages? From my calculations the standard emf should be 1.1v, the value I got experimentally was 1.06 (mainly due to insufficient resistance in the circuit to negate internal lost volts).

Thanks

@studiot

Hi, I know it has been a while, so much has been going on. I have just been writing up my results from this experiment and have come across some trouble with my calculated value for Faraday's constant. It is almost perfecty half what it should be, one of two problems could have occured: 1) In my stupidity I created the wrong concentrations of solution (not very probable as all sorts of anomalous points would be created when I then made my more diluted/concentrated solutions) 2) Something is wrong in my calculations Could any off you check these calculations to see if there are any problems. I used a Zinc anode and Copper cathode so my value for number of electrons transferred in the balanced ionic equation should be 2. If you require any more info, just say :). Hope you are all well. Harry

Thanks so much for your continued help, I will look into all of these in the coming weeks. Your questions are also very helpful, I have upcoming interviews where they will be asking me questions similar to as you have just posed. I don't think my answer to Q2 was quite satisfactory and this is mainly as I don't think I understand the question, could you clarify the question further?

Ok so this question took me longer than expected but I think I have an answer. I looked into the phase diagrams of water and found that at high pressures/ low temperatures , the liquid and gas state merge into something in between. I looked into it just a little and its called a super critical fluid, that's as far as I have got. As for this question, I have just read 'A brief introduction to superconductivity' in which it explains that superconductivity is a quantum phenomena. I'll be honest, a lot of the quantum mechanics were too complicated for me however I learnt that in this superconducting state electrons work as pairs to flow through a superconductor. Is this an example of particles not acting as molecules/ atoms?

These are all good points. I have maths and physics A-level. Ok so random number won't work, has anyone got a topic which will be enjoyable? I have the 11th edition.

Hi, I am a student in high school, wanting to study Chemistry at university. I am doing a challenge to read into a new chemical topic every week. I have here an Atkins Physical Chemistry textbook and would love it for whoever is reading to give me a random number between 10 and 850, this will be a page number and I will research that topic for that week. This forum will be an account of my progress and a place to get help on the topic. Thanks

Thank you for your advice. I have two university interviews coming up for chemistry and your expertise is greatly appreciated. I will probably make a post looking for tips or interview questions which I could have a go at in my own time. As for anode/cathode. I know that for a galvanic cell, reduction happens at the cathode. Therefore electrons flow to the cathode and is consequently positively charged. In an electrolytic cell i believe it is the other way round.

I was wondering, why do batteries slowly run out over time? I presume in electronics such as a torch that the circuit is broken when unused so why does this occur?

Also I was wanting to let each student do this mini kids version. Here, yeast is the catalyst, does anyone know the exact decomposition reaction which is happening here? https://www.thoughtco.com/kid-friendly-elephant-toothpaste-demo-604164

Attached is my practical proposal. It has a link at the bottom that should explain things. Also here is a youtube link : Elephants Toothpaste Experiment.docx Ok so I have seen these but my plan is to scale it down so each student can have a mini experiment. Also I need to work out the volume I will create as if I make mess my teacher will kille me

Hi, I am in secondary school studying chemistry. I chair the school's STEM society and am wanting to give a talk and practical on the elephants toothpaste that you may have seen online. Elephants toothpaste is large amounts of oxygen trapped in soap. To make a plume of this, you use hydrogen peroxide and a catalyst that releases the oxygen at an increased rate such as potassium Iodide (iodide ions are our catalyst). I am wanting to give this demonstration to other students and need to work out the volume of 'bubbles' that will be made so that I do not make too much. I will be using 100 volumes H2o2 Also I understand volume as a measurement of concentration in this case, however a lot of online sources use percentage. Do I take this as percentage by mass or by volume. Thanks

I am also happy to get away from the electronics :) As for temperature, my maximum resolution is 0.1 kelvin due to equipment av available. Obviously this isn't ideal with my level of precision of voltage but without that precision I wouldn't see any change in voltage and therefore would have no results to show. As for concentration I believe the school's are 5% error, which again isn't great but it will have to do. Unfortunately waste will not be accepted by my teachers and they don't want several dm(3) of solution lying around. I will try and make as large quantities as they will allow (probably 250cm(3) for each electrolyte), using a volumetric flask. Your physical problems are very interesting and I have never come across any of them before. I theorise with random radio pickup I may have fluctuating values of milivolts and therefore I should take an average of these. As for the other two, I do not believe there is much I can do to minimise these with the equipment I have (and with the level of accuracy I have will these matter?). Nevertheless you have given me many topics which sound fascinating and I will look into contact potentials especially. As for results, I cannot hope to get completely theoretical values due to systematic errors such as concentration and resistance. However as they are systematic, although my graph my have a slightly incorrect gradient and y-intercept, I should find a trend similar to that of the nernst equation.