A chemical question: to what extent and how quickly can H2S dissolved in oil be oxidized to elemental sulfur upon contact with air?
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As the title suggests, this is a chemistry problem from practice; those who handle analysis in this section should be quite familiar with it. We suspect that the presence of H2S dissolved in the oil (lubricant fraction) is the cause of our failure in the copper corrosion test. Are there any requirements regarding sampling for conducting this copper corrosion test? Is nitrogen protection required for sampling? To what extent and how quickly is H2S, thiols, or COS dissolved in oil likely to be oxidized into elemental sulfur when exposed to air?
I’ll give you a website; check it out by yourself. http://www.stolaf.edu/depts/chemistry/courses/toolkits/247/practice/medialib/data/
The original poster’s question is very detailed, and it seems difficult to answer. The moderator provided a link; after taking a look at it, I thought it was good. My foreign language skills are not very good, so I was unable to find what I needed. However, I believe the question relates to electrochemistry. In my opinion, depending on the density and viscosity of the oil, the probability of dissolved oxygen being present is quite low; therefore, it’s likely that hydrogen sulfide will oxidize into sulfur when in contact with oxygen in the air. To what extent this occurs depends on the duration and amount of time that hydrogen sulfide is in contact with oxygen. I feel my answer isn’t very good, and I hope that those with relevant experience can share their insights
The original poster’s question is very detailed, making it difficult to answer