I want to Syntesis TiCl4, here I find this reaction:

TiO2 + 2Cl2 + C > TiCl4 + CO2

I know that this reaction occurs around 900 degree celcius.

If you think that this reaction is possible with borosilicate glassware please tell my.

 

 

30122929-Titanium-Compounds-Inorganic.pdf

I want to Syntesis TiCl4, here I find this reaction:

TiO2 + 2Cl2 + C > TiCl4 + CO2

I know that this reaction occurs around 900 degree celcius.

If you think that this reaction is possible with borosilicate glassware please tell my.

 

 

30122929-Titanium-Compounds-Inorganic.pdf

 

I've always been told by professors that borosilicate glassware reaches its "softening" point around 800-830 C. So I wouldn't try it. The titanium dioxide will still be solid at this temperature, but I still wouldn't want a room full of chlorine (the product will also be a nasty hot, volatile liquid). I bet there's a way to catalyze this reaction at a lower temperature...

 

EDIT: 830 C, not 330 C, sorry

Edited September 12, 201015 yr by mississippichem

Wiki also says it will soften at about 820C.

In principle, you could use fused quartz but is it really worth it?

I'm pretty sure it would be easier to prepare it from Ti metal scrap and Cl2. Even then you are still going to be playing with hot chlorine and TiCl4 - both are bad for you.

I wanted to do this reaction with a type of test tube under an atmosphere of chlorine under pressure (because of the production of chlorine, which is produced in an Erlenmeyer flask) at 900 degree Celsius and condensing the gas into another test tube which has at -20 degrees Celsius.

 

I know the hazard of chlorine, titanium dioxide and TiCl4.

 

Edited September 12, 201015 yr by TiI4

I wanted to do this reaction with a type of test tube under an atmosphere of chlorine under pressure (because of the production of chlorine, which is produced in an Erlenmeyer flask) at 900 degree Celsius and condensing the gas into another test tube which has at -20 degrees Celsius.

 

I know the hazard of chlorine, titanium dioxide and TiCl4.

 

 

You're making the chlorine in situ? That's two hazardous reactions going on at the same time, brave.

I wanted to do this reaction with a type of test tube under an atmosphere of chlorine under pressure (because of the production of chlorine, which is produced in an Erlenmeyer flask) at 900 degree Celsius and condensing the gas into another test tube which has at -20 degrees Celsius.

 

I know the hazard of chlorine, titanium dioxide and TiCl4.

 

 

 

OK, so you plan to use chlorine under pressure in a tube about 80 degrees above it's melting point then magically stop it all disappearing onto a cold trap.

And you think you know about the hazards.

Would you understand if I were to say that I think that you don't know about the hazards and, until you do, you shouldn't try this.

be watching the comments, I think I'll do a test in a test tube filled with chlorine , the gas formed will condense in another test tube, the gas that will not be condensing (chlorine CO2 and a bit of TiCl4) will be dissolved in water is 3-5 degrees Celsius because TiCl4 reacts violently with the water has a temperature of 15 degrees Celsius and higher.