Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
Unfortunately my confusion is only deepening ... There is more CO2 in the np system - but I thought it was meant to be H2CO3, not CO2. There is HCO3- on the nickel - but no bicarbonate in the system. If the solution is acidic (ie, there is lots of H+ in the solution), where is the acidity coming from if not from dissociation of carbonic acid: H2CO3 + H2O = H+, HCO3- = 2H+, CO3= ? But you say only carbonic acid present. Oliver. On 07/02/2013 23:51, gaurav bhaduri wrote: Dear all Thank you for your interest in our work and your comments. To clarify some of the misunderstanding in the process conditions that I'd like to clarify. When we bubble CO2 in water with and without the nanoparticles, we observed that there is more CO2 in the nanoparticle system than in pure water. We also observed that there was HCO3- ions on the surface of the Ni nanoparticles surface, we thus explained that this enhancement could be due to adsorption of the HCO3- (from the acid) onto the Ni surface. We in no place claim the formation of CO3-- ions, to be clear on this point the system we are addressing in this article is at a acidic pH (5). Thus there is only carbonic acid species present no bicarbonate or carbonate system as they exist at higher pH values. Now coming to the point of mineralization. We are currently working on this (as explained by Dr Siller, previously) and would like to use silicates as our metal source (Ca2+ or Mg2+). Regarding the confusion of sea or oceanic system. We do not tend to imply the use of Ni nanoparticles in the ocean or any thing around it. The relation with sea urchin (or the marine environment) is just that, the use of Ni to study the hydration reaction we triggered by the studies done on the sea urchin by Dr Siller and my other colleagues. Our major application is to use this system as a satellite unit (plant) to an operational point source emitter (for example a power plant). The carbonate mineral thus produced would be used as landfill or in any other useful application. As mentioned above, we are working on the use of silicate sources (terrestrial) for the source of the alkali earth metals (Ca2+ or Mg2+), thus ruling out acidification of the ocean or any relation to the ocean. Hope I was able to explain the application of our technology. If you still have any doubts, please feel free to ask. We will try our level best to clarify any confusion. Thanks to all Kind regards Gaurav On Thursday, 7 February 2013 18:49:41 UTC, Greg Rau wrote: Thanks for responding. I really don't follow this. If I have a beaker of water fully equilibrated with air (CO2) and add your Ni particles, you are saying that more HCO3- and ultimately CO3s will spontaneously be produced. This won't happen unless thermodynamically favored, and if that water if fully equilibrated with air CO2 there is no thermodynamic condition that will force a change in the C chemistry. If your Ni particles are somehow consuming H+ or producing OH- then you've got a driving force, but you still need a source cations to make CaCO3s (am very interested to learn how you cheaply extract cations from silicates.) Otherwise, adding a catalyst to a system at thermodynamic equilibrium does nothing. On the other hand, adding something to seawater that overcomes the natural, chemical inhibition of abiotic CaCO3s precipitation could really cause some serious precipitation and CO2 injection into the atmosphere. No? -Greg From: lidija...@gmail.com javascript: lidija...@gmail.com javascript: Reply-To: lidija...@gmail.com javascript: lidija...@gmail.com javascript: Date: Thursday, February 7, 2013 8:32 AM To: geoengineering geoengi...@googlegroups.com javascript: Subject: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) With presence of Ni we have increases at the same time trapping of CO2 and increased the rates of conversion to carbonic acid on room temperature and on the atmospheric pressure. We still working to find the best mineralisation pathway - we will use silicates (magnesium calcium silicates) as a source of Ca2+ or Mg2+. While nickel nanoparticles are toxic as already mentioned in the paper we do not propose to spread this around in the enviroment but to have local disposal next to power plant or industrial plant. We made brief cost - 8$ per ton of CO2 if we can recover Ni 99% yield based on current price of nickel. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineerin...@googlegroups.com javascript:. To post to this group, send email to geoeng...@googlegroups.com
Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
Dear Oliver, I think it is not so trivial as you wrote - different steps of reactions which you wrote are prefered at different pH. Please for example see this web link and graph on the bottom of the web page: http://ion.chem.usu.edu/~sbialkow/Classes/3650/Carbonate/Carbonic%20Acid.html best wishes, Lidija On Friday, 8 February 2013 11:52:15 UTC, Oliver Tickell wrote: Unfortunately my confusion is only deepening ... There is more CO2 in the np system - but I thought it was meant to be H2CO3, not CO2. There is HCO3- on the nickel - but no bicarbonate in the system. If the solution is acidic (ie, there is lots of H+ in the solution), where is the acidity coming from if not from dissociation of carbonic acid: H2CO3 + H2O = H+, HCO3- = 2H+, CO3= ? But you say only carbonic acid present. Oliver. On 07/02/2013 23:51, gaurav bhaduri wrote: Dear all Thank you for your interest in our work and your comments. To clarify some of the misunderstanding in the process conditions that I'd like to clarify. When we bubble CO2 in water with and without the nanoparticles, we observed that there is more CO2 in the nanoparticle system than in pure water. We also observed that there was HCO3- ions on the surface of the Ni nanoparticles surface, we thus explained that this enhancement could be due to adsorption of the HCO3- (from the acid) onto the Ni surface. We in no place claim the formation of CO3-- ions, to be clear on this point the system we are addressing in this article is at a acidic pH (5). Thus there is only carbonic acid species present no bicarbonate or carbonate system as they exist at higher pH values. Now coming to the point of mineralization. We are currently working on this (as explained by Dr Siller, previously) and would like to use silicates as our metal source (Ca2+ or Mg2+). Regarding the confusion of sea or oceanic system. We do not tend to imply the use of Ni nanoparticles in the ocean or any thing around it. The relation with sea urchin (or the marine environment) is just that, the use of Ni to study the hydration reaction we triggered by the studies done on the sea urchin by Dr Siller and my other colleagues. Our major application is to use this system as a satellite unit (plant) to an operational point source emitter (for example a power plant). The carbonate mineral thus produced would be used as landfill or in any other useful application. As mentioned above, we are working on the use of silicate sources (terrestrial) for the source of the alkali earth metals (Ca2+ or Mg2+), thus ruling out acidification of the ocean or any relation to the ocean. Hope I was able to explain the application of our technology. If you still have any doubts, please feel free to ask. We will try our level best to clarify any confusion. Thanks to all Kind regards Gaurav On Thursday, 7 February 2013 18:49:41 UTC, Greg Rau wrote: Thanks for responding. I really don't follow this. If I have a beaker of water fully equilibrated with air (CO2) and add your Ni particles, you are saying that more HCO3- and ultimately CO3s will spontaneously be produced. This won't happen unless thermodynamically favored, and if that water if fully equilibrated with air CO2 there is no thermodynamic condition that will force a change in the C chemistry. If your Ni particles are somehow consuming H+ or producing OH- then you've got a driving force, but you still need a source cations to make CaCO3s (am very interested to learn how you cheaply extract cations from silicates.) Otherwise, adding a catalyst to a system at thermodynamic equilibrium does nothing. On the other hand, adding something to seawater that overcomes the natural, chemical inhibition of abiotic CaCO3s precipitation could really cause some serious precipitation and CO2 injection into the atmosphere. No? -Greg From: lidija...@gmail.com lidija...@gmail.com Reply-To: lidija...@gmail.com lidija...@gmail.com Date: Thursday, February 7, 2013 8:32 AM To: geoengineering geoengi...@googlegroups.com Subject: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) With presence of Ni we have increases at the same time trapping of CO2 and increased the rates of conversion to carbonic acid on room temperature and on the atmospheric pressure. We still working to find the best mineralisation pathway - we will use silicates (magnesium calcium silicates) as a source of Ca2+ or Mg2+. While nickel nanoparticles are toxic as already mentioned in the paper we do not propose to spread this around in the enviroment but to have local disposal next to power plant or industrial plant. We made brief cost - 8$ per ton of CO2 if we can recover Ni 99% yield based on current price of nickel. -- You received this
Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
There is nothing trivial about ocean chemistry! Many a salt water aquarium owner knows this all too well. Thanks for the link, Oliver. On 08/02/2013 14:01, lidijasil...@gmail.com wrote: Dear Oliver, I think it is not so trivial as you wrote - different steps of reactions which you wrote are prefered at different pH. Please for example see this web link and graph on the bottom of the web page: http://ion.chem.usu.edu/~sbialkow/Classes/3650/Carbonate/Carbonic%20Acid.html http://ion.chem.usu.edu/%7Esbialkow/Classes/3650/Carbonate/Carbonic%20Acid.html best wishes, Lidija On Friday, 8 February 2013 11:52:15 UTC, Oliver Tickell wrote: Unfortunately my confusion is only deepening ... There is more CO2 in the np system - but I thought it was meant to be H2CO3, not CO2. There is HCO3- on the nickel - but no bicarbonate in the system. If the solution is acidic (ie, there is lots of H+ in the solution), where is the acidity coming from if not from dissociation of carbonic acid: H2CO3 + H2O = H+, HCO3- = 2H+, CO3= ? But you say only carbonic acid present. Oliver. On 07/02/2013 23:51, gaurav bhaduri wrote: Dear all Thank you for your interest in our work and your comments. To clarify some of the misunderstanding in the process conditions that I'd like to clarify. When we bubble CO2 in water with and without the nanoparticles, we observed that there is more CO2 in the nanoparticle system than in pure water. We also observed that there was HCO3- ions on the surface of the Ni nanoparticles surface, we thus explained that this enhancement could be due to adsorption of the HCO3- (from the acid) onto the Ni surface. We in no place claim the formation of CO3-- ions, to be clear on this point the system we are addressing in this article is at a acidic pH (5). Thus there is only carbonic acid species present no bicarbonate or carbonate system as they exist at higher pH values. Now coming to the point of mineralization. We are currently working on this (as explained by Dr Siller, previously) and would like to use silicates as our metal source (Ca2+ or Mg2+). Regarding the confusion of sea or oceanic system. We do not tend to imply the use of Ni nanoparticles in the ocean or any thing around it. The relation with sea urchin (or the marine environment) is just that, the use of Ni to study the hydration reaction we triggered by the studies done on the sea urchin by Dr Siller and my other colleagues. Our major application is to use this system as a satellite unit (plant) to an operational point source emitter (for example a power plant). The carbonate mineral thus produced would be used as landfill or in any other useful application. As mentioned above, we are working on the use of silicate sources (terrestrial) for the source of the alkali earth metals (Ca2+ or Mg2+), thus ruling out acidification of the ocean or any relation to the ocean. Hope I was able to explain the application of our technology. If you still have any doubts, please feel free to ask. We will try our level best to clarify any confusion. Thanks to all Kind regards Gaurav On Thursday, 7 February 2013 18:49:41 UTC, Greg Rau wrote: Thanks for responding. I really don't follow this. If I have a beaker of water fully equilibrated with air (CO2) and add your Ni particles, you are saying that more HCO3- and ultimately CO3s will spontaneously be produced. This won't happen unless thermodynamically favored, and if that water if fully equilibrated with air CO2 there is no thermodynamic condition that will force a change in the C chemistry. If your Ni particles are somehow consuming H+ or producing OH- then you've got a driving force, but you still need a source cations to make CaCO3s (am very interested to learn how you cheaply extract cations from silicates.) Otherwise, adding a catalyst to a system at thermodynamic equilibrium does nothing. On the other hand, adding something to seawater that overcomes the natural, chemical inhibition of abiotic CaCO3s precipitation could really cause some serious precipitation and CO2 injection into the atmosphere. No? -Greg From: lidija...@gmail.com lidija...@gmail.com Reply-To: lidija...@gmail.com lidija...@gmail.com Date: Thursday, February 7, 2013 8:32 AM To: geoengineering geoengi...@googlegroups.com Subject: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) With presence of Ni we have increases at the same time trapping of CO2 and increased the rates of conversion to
RE: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
OK, so what is happening is that you are adding NiO and/or NiO is formed once Ni is added to oxygenated water, which is then hydrated to form Ni(OH)2. This then neutralizes the H2CO3 to form Ni(HCO3)2. You are adding or forming a chemical base to/in the system, not necessarily a catalyst. If it were purely a catalyst the carbon content in the +Ni and -Ni treatments would be identical, only the +Ni treatment would attain max [C(inorg)] faster. This then begs the question why not add cheaper metal oxides e.g., FeO or CaO to do the same thing, the latter explored by Kheshgi (1995)? Then there's the C footprint of reduced metal and/or metal oxide production -Greg From: geoengineering@googlegroups.com [geoengineering@googlegroups.com] on behalf of lidijasil...@gmail.com [lidijasil...@gmail.com] Sent: Thursday, February 07, 2013 3:26 PM To: geoengineering@googlegroups.com Cc: lidijasil...@gmail.com Subject: Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) Yes there is a driving force - we see OH and HCO3 on surface of nickel particles . Due to large surface area of particles the Ni-HCO3 plays large part how much of CO2 in total can be stored in this system. If you need a paper I can send you via my university account- lidia.sil...@ncl.ac.ukmailto:lidia.sil...@ncl.ac.uk. Regarding the mineralisation part we are working on this. ohttp://o -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out.
[geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
With presence of Ni we have increases at the same time trapping of CO2 and increased the rates of conversion to carbonic acid on room temperature and on the atmospheric pressure. We still working to find the best mineralisation pathway - we will use silicates (magnesium calcium silicates) as a source of Ca2+ or Mg2+. While nickel nanoparticles are toxic as already mentioned in the paper we do not propose to spread this around in the enviroment but to have local disposal next to power plant or industrial plant. We made brief cost - 8$ per ton of CO2 if we can recover Ni 99% yield based on current price of nickel. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out.
Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
Thanks for responding. I really don't follow this. If I have a beaker of water fully equilibrated with air (CO2) and add your Ni particles, you are saying that more HCO3- and ultimately CO3s will spontaneously be produced. This won't happen unless thermodynamically favored, and if that water if fully equilibrated with air CO2 there is no thermodynamic condition that will force a change in the C chemistry. If your Ni particles are somehow consuming H+ or producing OH- then you've got a driving force, but you still need a source cations to make CaCO3s (am very interested to learn how you cheaply extract cations from silicates.) Otherwise, adding a catalyst to a system at thermodynamic equilibrium does nothing. On the other hand, adding something to seawater that overcomes the natural, chemical inhibition of abiotic CaCO3s precipitation could really cause some serious precipitation and CO2 injection into the atmosphere. No? -Greg From: lidijasil...@gmail.commailto:lidijasil...@gmail.com lidijasil...@gmail.commailto:lidijasil...@gmail.com Reply-To: lidijasil...@gmail.commailto:lidijasil...@gmail.com lidijasil...@gmail.commailto:lidijasil...@gmail.com Date: Thursday, February 7, 2013 8:32 AM To: geoengineering geoengineering@googlegroups.commailto:geoengineering@googlegroups.com Subject: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) With presence of Ni we have increases at the same time trapping of CO2 and increased the rates of conversion to carbonic acid on room temperature and on the atmospheric pressure. We still working to find the best mineralisation pathway - we will use silicates (magnesium calcium silicates) as a source of Ca2+ or Mg2+. While nickel nanoparticles are toxic as already mentioned in the paper we do not propose to spread this around in the enviroment but to have local disposal next to power plant or industrial plant. We made brief cost - 8$ per ton of CO2 if we can recover Ni 99% yield based on current price of nickel. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.commailto:geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.commailto:geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out.
Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
Yes there is a driving force - we see OH and HCO3 on surface of nickel particles . Due to large surface area of particles the Ni-HCO3 plays large part how much of CO2 in total can be stored in this system. If you need a paper I can send you via my university account- lidia.sil...@ncl.ac.uk. Regarding the mineralisation part we are working on this. o -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out.
Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
Dear Dr Rau, Thank you for your response towards our research, I appreciate your comments on our work. To explain about the saturation experiments; we tried to saturate the CO2 within water and with and without the nanoparticles present in the system and found that there was more CO2 in the nanoparticle solution in that of pure water.We do not claim in the paper that we are getting CO3-- in our system at all. We have observed that the concentration of the acid in the nanoparticle solution is higher than that of pure water. We observed that here was HCO3- species on our nanoparticle surface and the possible explanation (for this increase) we suggested was that there might me adsorption of HCO3- ions (from the acid) on the nanoparticle surface. As all this is happening at a pH in the acidic range (5) thus according to chemistry of CO2 in water at this pH range there is acid system and none of the basic system of bicarbonates or carbonates exist. As mentioned by Dr Siller, previously we are yet experimenting on the method of carbonate mineral formation with; possibly silicate sources. We do not tend to use sea water or oceanic system in our work at all. The idea to use Nickel for this reaction was taken from the sea urchin studies conducted by Dr Siller and other my other colleagues. We do not dump anything into the sea or use the oceanic system into the process. We suggest using a mineral source (terrestrial) for the metal ion (Ca2+ or Mg2+) to form corresponding mineral carbonate. The concept is to use it as a satellite unit for point source emission (power plants for example) trapping. On Thursday, 7 February 2013 18:49:41 UTC, Greg Rau wrote: Thanks for responding. I really don't follow this. If I have a beaker of water fully equilibrated with air (CO2) and add your Ni particles, you are saying that more HCO3- and ultimately CO3s will spontaneously be produced. This won't happen unless thermodynamically favored, and if that water if fully equilibrated with air CO2 there is no thermodynamic condition that will force a change in the C chemistry. If your Ni particles are somehow consuming H+ or producing OH- then you've got a driving force, but you still need a source cations to make CaCO3s (am very interested to learn how you cheaply extract cations from silicates.) Otherwise, adding a catalyst to a system at thermodynamic equilibrium does nothing. On the other hand, adding something to seawater that overcomes the natural, chemical inhibition of abiotic CaCO3s precipitation could really cause some serious precipitation and CO2 injection into the atmosphere. No? -Greg From: lidija...@gmail.com javascript: lidija...@gmail.comjavascript: Reply-To: lidija...@gmail.com javascript: lidija...@gmail.comjavascript: Date: Thursday, February 7, 2013 8:32 AM To: geoengineering geoengi...@googlegroups.com javascript: Subject: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) With presence of Ni we have increases at the same time trapping of CO2 and increased the rates of conversion to carbonic acid on room temperature and on the atmospheric pressure. We still working to find the best mineralisation pathway - we will use silicates (magnesium calcium silicates) as a source of Ca2+ or Mg2+. While nickel nanoparticles are toxic as already mentioned in the paper we do not propose to spread this around in the enviroment but to have local disposal next to power plant or industrial plant. We made brief cost - 8$ per ton of CO2 if we can recover Ni 99% yield based on current price of nickel. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineerin...@googlegroups.com javascript:. To post to this group, send email to geoeng...@googlegroups.comjavascript: . Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out.
Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
Dear all Thank you for your interest in our work and your comments. To clarify some of the misunderstanding in the process conditions that I'd like to clarify. When we bubble CO2 in water with and without the nanoparticles, we observed that there is more CO2 in the nanoparticle system than in pure water. We also observed that there was HCO3- ions on the surface of the Ni nanoparticles surface, we thus explained that this enhancement could be due to adsorption of the HCO3- (from the acid) onto the Ni surface. We in no place claim the formation of CO3-- ions, to be clear on this point the system we are addressing in this article is at a acidic pH (5). Thus there is only carbonic acid species present no bicarbonate or carbonate system as they exist at higher pH values. Now coming to the point of mineralization. We are currently working on this (as explained by Dr Siller, previously) and would like to use silicates as our metal source (Ca2+ or Mg2+). Regarding the confusion of sea or oceanic system. We do not tend to imply the use of Ni nanoparticles in the ocean or any thing around it. The relation with sea urchin (or the marine environment) is just that, the use of Ni to study the hydration reaction we triggered by the studies done on the sea urchin by Dr Siller and my other colleagues. Our major application is to use this system as a satellite unit (plant) to an operational point source emitter (for example a power plant). The carbonate mineral thus produced would be used as landfill or in any other useful application. As mentioned above, we are working on the use of silicate sources (terrestrial) for the source of the alkali earth metals (Ca2+ or Mg2+), thus ruling out acidification of the ocean or any relation to the ocean. Hope I was able to explain the application of our technology. If you still have any doubts, please feel free to ask. We will try our level best to clarify any confusion. Thanks to all Kind regards Gaurav On Thursday, 7 February 2013 18:49:41 UTC, Greg Rau wrote: Thanks for responding. I really don't follow this. If I have a beaker of water fully equilibrated with air (CO2) and add your Ni particles, you are saying that more HCO3- and ultimately CO3s will spontaneously be produced. This won't happen unless thermodynamically favored, and if that water if fully equilibrated with air CO2 there is no thermodynamic condition that will force a change in the C chemistry. If your Ni particles are somehow consuming H+ or producing OH- then you've got a driving force, but you still need a source cations to make CaCO3s (am very interested to learn how you cheaply extract cations from silicates.) Otherwise, adding a catalyst to a system at thermodynamic equilibrium does nothing. On the other hand, adding something to seawater that overcomes the natural, chemical inhibition of abiotic CaCO3s precipitation could really cause some serious precipitation and CO2 injection into the atmosphere. No? -Greg From: lidija...@gmail.com javascript: lidija...@gmail.comjavascript: Reply-To: lidija...@gmail.com javascript: lidija...@gmail.comjavascript: Date: Thursday, February 7, 2013 8:32 AM To: geoengineering geoengi...@googlegroups.com javascript: Subject: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) With presence of Ni we have increases at the same time trapping of CO2 and increased the rates of conversion to carbonic acid on room temperature and on the atmospheric pressure. We still working to find the best mineralisation pathway - we will use silicates (magnesium calcium silicates) as a source of Ca2+ or Mg2+. While nickel nanoparticles are toxic as already mentioned in the paper we do not propose to spread this around in the enviroment but to have local disposal next to power plant or industrial plant. We made brief cost - 8$ per ton of CO2 if we can recover Ni 99% yield based on current price of nickel. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineerin...@googlegroups.com javascript:. To post to this group, send email to geoeng...@googlegroups.comjavascript: . Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit
[geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
BBC News quotes http://www.bbc.co.uk/news/science-environment-21320666co-author Lidija Siller: You bubble CO2 through the water in which you have nickel nanoparticles and you are trapping much more carbon than you would normally - and then you can easily turn it into calcium carbonate. It seems too good to be true, but it works, The Newcastle University press releasehttp://www.ncl.ac.uk/press.office/press.release/item/could-the-humble-sea-urchin-hold-the-key-to-carbon-capture#.URLBKB3CZ8E quotes Siller the result was the complete removal of CO2. NU PR states the group has patented the process and are looking for investors. PhD student lead author Gaurav Bhaduri is quoted: [the nickel catalyst] is very cheap, a thousand times cheaper than carbon anhydrase Chemistry World, i.e.: Sea urchin inspires carbon capture catalysthttp://www.rsc.org/chemistryworld/2013/02/sea-urchin-exoskeleton-nickel-carbon-capture quotes Siller: 'The current challenge that we are addressing is to quantify the process. We would like to determine the reaction kinetics and exact yields. Once we have this information we plan to do a small continuous process in a lab-scale pilot plant. And they've dug up a skeptic: 'This work represents an incremental addition to CO2 capture where the catalytic dimension is relevant,' comments Mark Keanehttp://www.cre.hw.ac.uk/Mark%20A%20Keane.html, who investigates catalysis engineering at Heriot-Watt University in Edinburgh, UK. 'True innovation, however, should harness catalytic action in the conversion of CO2 to high value products, such as carbamates. On Tuesday, February 5, 2013 11:03:52 AM UTC-8, andrewjlockley wrote: http://pubs.rsc.org/en/content/articlelanding/2013/cy/c3cy20791a Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage Gaurav A. Bhaduri and Lidija ŠillerCatal. Sci. Technol., 2013, Advance Article DOI: 10.1039/C3CY20791A Abstract The separation and storage of CO2 in geological form as mineral carbonates has been seen as a viable method to reduce the concentration of CO2 from the atmosphere. Mineralization of CO2 to mineral salts like calcium carbonate provides a stable storage of CO2. Reversible hydration of CO2 to carbonic acid is the rate limiting step in the mineralization process. We report catalysis of the reversible hydration of CO2 using nickel nanoparticles (NiNPs) at room temperature and atmospheric pressure. The catalytic activity of the NiNPs is pH independent and as they are water insoluble and magnetic they can be magnetically separated for reuse. The reaction steps were characterized using X-ray photoemission spectroscopy and a possible reaction mechanism is described. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out.
RE: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing)
While spontaneous carbonate precip from water is claimed, perhaps they meant seawater. I might believe this if the nannoparticles somehow override the significant chemical inhibition of CaCO3 precip (CaCO3 is supersaturated in SW by 4-6x). Still this would generate CO2g and CaCO3s at the expense of SW Ca(HCO3)2aq, so don't see the CO2 mitigation angle. Another sighting of the Calera effect? -Greg From: geoengineering@googlegroups.com [geoengineering@googlegroups.com] on behalf of Ken Caldeira [kcalde...@gmail.com] Sent: Wednesday, February 06, 2013 4:24 PM To: jrandomwin...@gmail.com Cc: geoengineering@googlegroups.com Subject: Re: [geo] Re: Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage - Catalysis Science Technology (RSC Publishing) Where does the Ca2+ or Mg2+ (or other cations) come from that you would need to make the carbonate minerals. The challenge is to find bases that can be extracted without causing substantial environmental damage. Usually things that sound too good to be true are too good to be true. Ken Caldeira kcalde...@carnegiescience.edumailto:kcalde...@carnegiescience.edu +1 650 704 7212 http://dge.stanford.edu/labs/caldeiralab Typed on an all-thumbs keyboard On Feb 7, 2013, at 8:17, David Lewis jrandomwin...@gmail.commailto:jrandomwin...@gmail.com wrote: BBC News quoteshttp://www.bbc.co.uk/news/science-environment-21320666 co-author Lidija Siller: You bubble CO2 through the water in which you have nickel nanoparticles and you are trapping much more carbon than you would normally - and then you can easily turn it into calcium carbonate. It seems too good to be true, but it works, The Newcastle University press releasehttp://www.ncl.ac.uk/press.office/press.release/item/could-the-humble-sea-urchin-hold-the-key-to-carbon-capture#.URLBKB3CZ8E quotes Siller the result was the complete removal of CO2. NU PR states the group has patented the process and are looking for investors. PhD student lead author Gaurav Bhaduri is quoted: [the nickel catalyst] is very cheap, a thousand times cheaper than carbon anhydrase Chemistry World, i.e.: Sea urchin inspires carbon capture catalysthttp://www.rsc.org/chemistryworld/2013/02/sea-urchin-exoskeleton-nickel-carbon-capture quotes Siller: 'The current challenge that we are addressing is to quantify the process. We would like to determine the reaction kinetics and exact yields. Once we have this information we plan to do a small continuous process in a lab-scale pilot plant. And they've dug up a skeptic: 'This work represents an incremental addition to CO2 capture where the catalytic dimension is relevant,' comments Mark Keanehttp://www.cre.hw.ac.uk/Mark%20A%20Keane.html, who investigates catalysis engineering at Heriot-Watt University in Edinburgh, UK. 'True innovation, however, should harness catalytic action in the conversion of CO2 to high value products, such as carbamates. On Tuesday, February 5, 2013 11:03:52 AM UTC-8, andrewjlockley wrote: http://pubs.rsc.org/en/content/articlelanding/2013/cy/c3cy20791a Nickel nanoparticles catalyse reversible hydration of carbon dioxide for mineralization carbon capture and storage Gaurav A. Bhaduri and Lidija ŠillerCatal. Sci. Technol., 2013, Advance Article DOI: 10.1039/C3CY20791A Abstract The separation and storage of CO2 in geological form as mineral carbonates has been seen as a viable method to reduce the concentration of CO2 from the atmosphere. Mineralization of CO2 to mineral salts like calcium carbonate provides a stable storage of CO2. Reversible hydration of CO2 to carbonic acid is the rate limiting step in the mineralization process. We report catalysis of the reversible hydration of CO2 using nickel nanoparticles (NiNPs) at room temperature and atmospheric pressure. The catalytic activity of the NiNPs is pH independent and as they are water insoluble and magnetic they can be magnetically separated for reuse. The reaction steps were characterized using X-ray photoemission spectroscopy and a possible reaction mechanism is described. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.commailto:geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to geoengineering@googlegroups.commailto:geoengineering@googlegroups.com. Visit this group at http://groups.google.com/group/geoengineering?hl=en. For more options, visit https://groups.google.com/groups/opt_out. -- You received this message because you are subscribed to the Google Groups geoengineering group. To unsubscribe from this group and stop receiving emails from it, send an email to geoengineering+unsubscr...@googlegroups.com. To post to this group, send email to
