co2 diy idea

[basslover34]

It will work, the volume available is a drawback. Yeast/sugar is a slow, controllable reaction whereas vinegar/baking soda is quick and really needs a pressurized storage system. True, hard packing the soda or placing in a container and limiting the vinegar are possible, it will take alot of experimentation to get a good, usable flow.

With this much co2 available you do have to monitor your chemistry carefully.

Dr Joe

.

Perhaps best suited for a Larger system??

 

[haysanatar]

Perhaps best suited for a Larger system??

probably

so vinegar is usually 5% acetic acid

HC2H3O2(aq) + NaHCO3(aq)

NaC2H3O2(aq) + H2O(

) + CO2(g)

so a mole of acetic acid would create a mole of co2.
but as noted vinegar is 5%
The mass of one mole of HC2H3O2 (acetic acid) is 60.0 g

a drop of water weights about 0.05 g
.05 of that is vinegar
.0025
so... 4.16 10(-5) moles of acetic acid in a single drop
which will creat the same amount of co2 molecularly
under stp..
it would create 9.3 10(-4) liters of co2
so about a ml of co2 per drop.
thoughts on that?

 

[themancmt]

sounds good but i suck at math.
lol

 

[Oreo]

I don't think the quickness of the reaction would be nearly the issue that consistency would be. The ideal situation would be to have the baking soda & the vinegar both in separate storage containers & metered into a mixing chamber.

One problem I see is if you put lets say 2 cups of baking soda in a jar & dripped vinegar in on top, the vinegar would react with the baking soda on the surface & create an inert layer of mush on top of the dry powder below. Then the vinegar would pool up on top of that. Now, if that pool of vinegar seeps through, you could have a sudden voluminous burst of CO2.

Will baking soda dissolve in water? Perhaps drip them both into a 3rd container. If not baking soda, consider hydrated lime, or liquid caustic soda. Also maybe consider a stronger acid solution. Although it would speed up the reaction, I'd think a good strong acid would aid consistency.

 

[Oreo]

For example, the reaction between hydrochloric acid and calcium carbonate (limestone or chalk) is depicted below:

HCl + CaCO3 → CaCl2 + H2CO3

The H2CO3 then decomposes to water and CO2. Such reactions are accompanied by foaming or bubbling, or both. In industry such reactions are widespread because they can be used to neutralize waste acid streams.

 

[haysanatar]

I don't think the quickness of the reaction would be nearly the issue that consistency would be. The ideal situation would be to have the baking soda & the vinegar both in separate storage containers & metered into a mixing chamber.

One problem I see is if you put lets say 2 cups of baking soda in a jar & dripped vinegar in on top, the vinegar would react with the baking soda on the surface & create an inert layer of mush on top of the dry powder below. Then the vinegar would pool up on top of that. Now, if that pool of vinegar seeps through, you could have a sudden voluminous burst of CO2.

Will baking soda dissolve in water? Perhaps drip them both into a 3rd container. If not baking soda, consider hydrated lime, or liquid caustic soda. Also maybe consider a stronger acid solution. Although it would speed up the reaction, I'd think a good strong acid would aid consistency.

I'll do some tests with an eye dropper and a bunch of baking soda.
not really looking to do a stronger acid unless you mean more concentrated and I think I would add water to the baking soda.
I looked into lemon juice (citric acid)
its 5% too
approximately 0.03 moles/Liter

whats the ideal amount of co2/hour