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Specialty Chemistry Forums => Citizen Chemist => Topic started by: blahblahblah on July 30, 2015, 04:02:20 PM

Title: reduction of tin(II) oxide (stannous oxide)
Post by: blahblahblah on July 30, 2015, 04:02:20 PM
I need to reduce tin (II) oxide, could ammonia act as a reducing agent. if not what reducing agents could reduce tin oxide to elemental tin?

Also I was considering using hydrogen as a reducing agent. I have researched this a little. Could diatomic hydrogen do this, or would i have to use atomic(nascent hydrogen).

I have a solution (more of a slurry since SnO isnt that soluble) of tin(II) oxide. Could i just bubble hydrogen into the  mixture to reduce the compound to elemental tin 
Title: Re: reduction of tin(II) oxide (stannous oxide)
Post by: Arkcon on July 30, 2015, 04:49:13 PM
Quote from: blahblahblah on July 30, 2015, 04:02:20 PM
I have a solution (more of a slurry since SnO isnt that soluble) of tin(II) oxide. Could i just bubble hydrogen into the  mixture to reduce the compound to elemental tin

No, that's not going to work.  That's essentially blowing a mist of hydrogen over metal flakes, with some water around.  And that's not how hydrogen reduction works. 

I'm glad you've read "some" about this topic.  Try to read some more, and see if you can come up with some other ideas that may work.
Title: reduction of tin(II) oxide with electrical current
Post by: blahblahblah on July 30, 2015, 05:26:02 PM
In the case of this video what would be the half reactions at the anode and cathode:

https://www.youtube.com/watch?v=sD8_IAbnmLM

Note also in the video the uploader commented : Tin(II) chloride is notorious to get into aqueous solution.  So the pH of the solution was adjusted to be less than 2 using hydrochloric acid.  Overall concentration of tin(II) chloride is 0.2 M if I remembered correctly.

How was HCL or water involed in the redox reaction?

Thanks
Title: Re: reduction of tin(II) oxide (stannous oxide)
Post by: PhotoElectroMaterials on July 30, 2015, 10:19:51 PM
If you can make it to powder form, you can reduce it with H2 gas in a tubular furnace.  Reduction using hydrogen is usually done at high temperature and an atmosphere of hydrogen is created by continuously passing H2 through the furnace.    You can find the exact temperature in the journals or even google. 

Combination of hydrogen and high temperature is extremely dangerous and you definitely need some help to hand such experiment.
Title: Re: reduction of tin(II) oxide (stannous oxide)
Post by: Intanjir on July 31, 2015, 02:12:17 AM
Smelt it!
Title: Re: reduction of tin(II) oxide with electrical current
Post by: Borek on July 31, 2015, 03:08:03 AM
Take a close look at the anode. Especially about 2:20 it is obvious what is happening.

And it is absolutely not surprising, that's what one should expect.