# Does water freely absorb atmospheric CO2?

So, there has been a fairly groundbreaking new invention that can convert CO2 dissolved in water to Ethanol1. At face value, it's cheap, easy, and relatively energy-lightweight. All it requires is the catalytic surface and CO2 to be dissolved in water.

I'm just curious, this invention looks like the holy grail of Green news, but not being a chemist, and doubting that the reporters are (all) chemists, I have to ask "Where's the catch", and the best I can find is how quickly CO2 dissolves in water, so, is this step of the above process fairly easy, or would it require additional research?

Note: This question is about how quickly atmospheric CO2 dissolves in water. Comments on the discovery would probably be better served as a comment then an answer.

• There is indeed a catch. Have a look at the ChemSelect paper and a previous article by Adam Rondione, where the making of the electrodes is described. All this is very impressive, but at the moment, we're taking about lab scale, not about huge setups necessary for an industrial application. – Klaus-Dieter Warzecha Oct 20 '16 at 18:44

Er, the quick, simple technical answer is "Yes, water will absorb $\ce{CO2}$". However, there is a "but" coming. Actually, two "buts".

First, plain water will not be able to absorb much $\ce{CO2}$. Henry's Constant for $\ce{CO2}$ in $\ce{H2O}$ is $K_H=29.76 \mathrm{atm\over mol/L}$. Considering the partial pressure of $\ce{CO2}$ in air is roughly $3.5\times10^{-4}~\mathrm{atm}$, one liter of water can absorb, at best $1.18\times10^{-4}~\mathrm{mol}~\ce{CO_2}$ which is only about $0.1$% of a gram of $\ce{CO2}$. Not very much. (Note, I'm ignoring the conversion to carbonate, $\ce{CO3^{2-}}$, and bicarbonate, $\ce{HCO3^{-}}$, because in otherwise neutral water, they don't exist in appreciable quantities (see: Carbonic Acid)

Second, that's the thermodynamic best you can do. However, you have to contend with the kinetics and diffusion limitations as well. Basically, it takes time for the $\ce{CO2}$ to go from the air to the water, and then to get well mixed within the water.

Now, there's a couple things you can do to help $\ce{CO2}$ absorption. First, instead of using neutral water, use and alkaline solution. For example, if you add $\ce{NaOH}$ to your water, the equilibrium will shift toward the carbonate ion, $\ce{CO3^{2-}}$:

$$\ce{2NaOH + CO2->Na2CO3 + H2O}$$

This allows orders of magnitude more $\ce{CO2}$ to be absorbed than would possible, basically, you become limited by the amount of sodium hydroxide you have and the kinetics.

Speaking of kinetics, how can we help that out? Packed bed towers! Imagine having a tall column filled with beads. Blow your air up from the bottom, while allowing the alkaline solution to flow from the top. This will maximize contact between the two phases and enhance the transfer of $\ce{CO2}$ from the gas to liquid.

And that is basically how scrubbers work in chemical plants, and one method of carbon sequestration. However, the very low concentration of $\ce{CO2}$ in air ($\sim\!400~\mathrm{ppm}$) makes pulling appreciable amounts of $\ce{CO2}$ from the air infeasible and an inefficient use of resources.