September 20, 2024, 06:14:17 PM
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Chemical Education and Careers / Essential tremor in the lab - your experience
« Last post by Incitatus on Yesterday at 05:09:45 PM »
Hi,

I am a undergraduate chemical engineering student. Because of my studies, I spend quite a lot of time in the chemistry lab. A year ago, I was diagnosed with essential tremor, also affecting my hands. Because of this, I had problems, mainly concerning the use of a pipette (another thing is that the analytical chemistry course was a speedrun). Outside the lab, the tremor has little effect on my life.

Has anyone else experienced this problem and works in a laboratory? What is your experience? Has the tremor worsened your accuracy / risked your safety? Do you have any good practices related to this?

I know you are can't judge the degree of my problem or decide anything for me. However, I would appreciate any response if you have experience with this problem. Thank you in advance!
Incitatus
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Generic Discussion / What is happening
« Last post by aimlesswonderer on Yesterday at 02:20:05 PM »
Ok. So I was trying to make a diamagnetic clay for an experiment.
My thought was add copper oxide to bleached clay mix and kiln.
But once I mixed the copper oxide to the clay water solution now it keep making a film . It bubbles and smells like bad breath.
So I filtered alot of the clay before bleaching and then rinsed the the bleached clay before adding copper oxide.
The liquid seems to be more acidic then anticipated the spoon I used to skim the film is now pretty corroded. It's a cheap spoon I think nickel plated. But from what I have researched it doesn't make sense why it just keeps reacting. I skim and shake to no end it keeps making the light clay colored film every time any suggestions on what could be taking place.
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Undergraduate General Chemistry Forum / Re: Question on the NO2/N2O4 equilibrium
« Last post by Borek on Yesterday at 02:52:16 AM »
Quote from: czmtzyddl on September 18, 2024, 08:43:24 PM
Hmm. So does it mean that although the reaction will consume more NO2, the volume shall shrink at the same time, causing the reaction to keep on going till the concentration turns back to the origin?

Exactly.

And yes, there is a formula - just for the equilibrium constant. In this particular case (one reagent, one product, it doesn't have to be identical for other cases) no matter what the initial composition of the mixture is (you can start with just NO2, just N2O4, or anything in between*) once the system gets to equilibrium partial pressures of both gases will have the same value - which also means identical concentrations and identical absorption of light (or the same color).

*technically preparing things like "pure NO2" or "pure N2O4" is impossible, as they immediately start to interconvert.
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Undergraduate General Chemistry Forum / Re: Question on the NO2/N2O4 equilibrium
« Last post by czmtzyddl on September 18, 2024, 08:48:12 PM »
Or is there an appropriate mathematical formula to explain this problem?
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Undergraduate General Chemistry Forum / Re: Question on the NO2/N2O4 equilibrium
« Last post by czmtzyddl on September 18, 2024, 08:43:24 PM »
Hmm. So does it mean that although the reaction will consume more NO2, the volume shall shrink at the same time, causing the reaction to keep on going till the concentration turns back to the origin?
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Analytical Chemistry Forum / Re: Appearance of IDMS calibration curve under ideal conditions
« Last post by Babcock_Hall on September 18, 2024, 07:33:30 PM »
If I understand correctly, one cause of nonlinearity is that there is an impurity in the standard that appears at the mass of the analyte, or vice versa.
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Undergraduate General Chemistry Forum / Re: Question on the NO2/N2O4 equilibrium
« Last post by Borek on September 18, 2024, 10:34:16 AM »
There is a very important hint in the problem: system is kept at the constant pressure.
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Undergraduate General Chemistry Forum / Re: Question on the NO2/N2O4 equilibrium
« Last post by czmtzyddl on September 18, 2024, 07:30:24 AM »
Well, from my perspective, when adding extra NO2 to the system, the concentration of NO2 increases. Therefore the color goes darker. However, according to Le Chatelier's principle, part of the NO2 should turn into N2O4 and the color should turn lighter correspondingly. And that’s the problem, the extent to which the color changes.
My friends and I both agree that the color should be darker than the origin, while our teacher believes the color should stay the same. Since I don’t have the equipment to conduct the experiment, I tried to calculate the Δc during the process. It seems to be so complicated that it confuses me even more.
So what’s really happening in the system? How should I think about a problem like this the next time? I hope the answer could include some fundamental logics of chemistry rather than some conclusions I don’t even know where they are derived from. And this is also why I posted this high school chemistry problem here. Thanks! :)
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Organic Chemistry Forum / Re: Isolation of Boronic Acid
« Last post by rolnor on September 18, 2024, 05:20:31 AM »

I dont understand what compound you are making. It sounds like an interesting project. Do you have a reference you are using, a paper? To isolate boronic acids can probably be a bit tricky, boron is different and can behave strangely.
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Undergraduate General Chemistry Forum / Re: Question on the NO2/N2O4 equilibrium
« Last post by billnotgatez on September 18, 2024, 01:18:09 AM »
read forum rules
We deleted your other copy of this question because you are not allowed to double post.
You should attempt to show some work before expecting help.
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