Summary of my undergraduate honors thesis chemical research I conducted. In this presentation, I give background to the significance of this research, a brief review of previous research done in the field, report the findings of this study, deliver several conclusions of the study, and propose further work that can be conducted in this research area.
3. Background:
Fossil Fuels Vs. Fuel Cells
■ Future of fossil fuels and internal combustion engines (ICEs)
– Environmental concerns
– Long-term economic/political ramifications
■ Fuel cells
■ H2, CH3OH
■ Oxygen Reduction Reaction (ORR)
■ CO
4. Background:
Fuel Cell Structure
Fig. 1. Hydrogen fuel cell design
Source: ”Thermodynamic Efficiency of Hydrogen Fuel
Cells”, MECH Tech. YouTube. Video. Accessed 16 June 2022
• Precious metal cost for
catalyst
• Pt
• ORR kinetics (sluggish)
5. Background: Examples
Fig. 2. Toyota Mirai: H2 Fuel Cell
Electric Vehicle (FCEV)
Source: “Preview: 2021 Toyota Mirai” Motor Authority.
Web.
https://www.motorauthority.com/news/1130013_2021-
toyota-mirai-price-specs-review-photos-info. Accessed 19
June 2022.
Fig. 3. General Motors (GM)
Chevrolet Equinox Fuel Cell: H2
FCEV
Image Source: “General Motors Hydrogen4 - Chevrolet
Hydrogen Fuel Cell Equinox Prototypes 2008”.
AutoConcept-Reviews. Web. http://www.autoconcept-
reviews.com/cars_reviews/gm/GM-hydrogen4-chevrolet-
hydrogen-fuel-cell-equinox-2008/cars_reviews-gm-
hydrogen4-chevrolet-hydrogen-fuel-cell-equinox-
6. Previous Work:
Humble Beginnings
■ Windsor, M. M.; Blanchard, A. A. Nickel Carbonyl. A Study of the Mechanism of
Its Formation from Nickel Sulfide and Carbon Monoxide. Journal of the
American Chemical Society 1933, 55 (5), 1877–1883.
– Observed reduction of Ni2+ sulfide or cyanide by carbon monoxide (CO)
under basic conditions to form Ni(CO)4
■ Hirsch, E.; Peters, E. Canadian Metallurgical Quarterly 1964, 3 (2), 137–151.
– Studied kinetics of oxidation of CO by Ni-amine complexes
– Mechanism:
Ni(NH3)+CO+OH−→[(NH3)−Ni−CO−OH]+4CO→Ni(CO)4+CO2+NH4+
7. Previous Work:
Progress
■ Jasinski, R. Nature 1964, 201 (4925), 1212–1213.
– Synthesis of Co-Phthalocyanine catalyst capable of reducing O2 in basic
conditions
Fig. 4. Synthetic relationship between phthalocyanine and
porphyrin.
Source: “Phthalocyanine” Wikipedia. Web.
https://en.wikipedia.org/wiki/Phthalocyanine Accessed 19
8. Previous Work:
Expanding The Canon
■ Gewirth, A. A.; Thorum, M. S. Electroreduction of Dioxygen for Fuel-Cell
Applications: Materials and Challenges. Inorganic
Chemistry 2010, 49 (8), 3557–3566.
– Markovic and co-workers used a Ni/Pt alloy of nanoparticles as the
catalyst for a proton exchange membrane fuel cell
■ Lo, W.; Hu, C.; Lumeij, M.; Dronskowski, R.; Lovihayeem, M.; Ishal, O.; Jiang,
J. [CoI(CN)2(CO)3]−, a New Discovery from an 80-Year-Old Reaction. Chemical
Communications 2013, 49 (67), 7382. https://doi.org/10.1039/c3cc43269f.
– Synthesis of two new novel Co1+ complexes w/mixed CO/cyanide (CN)
ligands under CO atmosphere
9. Previous Work:
Expanding the Canon
Fig. 5. ORTEP drawing of [CoI(CN)2(CO)3] (left) and
[CoI(CN)3(CO)2] (right) at the 50% ellipsoid level.
Source: Lo, W.; Hu, C.; Lumeij, M.; Dronskowski, R.; Lovihayeem, M.;
Ishal, O.; Jiang, J. [CoI(CN)2(CO)3]−, a New Discovery from an 80-Year-
Old Reaction. Chemical Communications 2013, 49 (67), 7382.
https://doi.org/10.1039/c3cc43269f.
10. Previous Work:
Further Expansion and Prototype Development
■ Chem. Commun., 2015, 51, 9432
– Jiang and co-workers expanded 2013 study and synthesized Ni0 cyano-
carbonyl complexes
– Used these Ni complexes to catalyze CO oxidation, reversible upon
addition of base to mixture under CO atmosphere
Fig. 6. ORTEP drawing of [Ni0(CN)(CO)3]- (left) and
[Ni0(CN)2(CO)2]2- (right) at the 50% probability level.
Source: Chem. Commun., 2015, 51, 9432
11. Previous Work:
Why CO?
Fig. 7. Catalytic cycle depicting CO oxidation
Source: Chem. Commun., 2015, 51, 9432
■ CO as reducing agent
– Nearly same energy content as H2
volume-wise in gas phase
(Bond dissociation energy = 1072 kJ/mol)
– Precedents in literature
Fig. 8. Two primitive CO-powered fuel cells
Source: Chem. Commun., 2015, 51, 9432
12. This Study:
Hypothesis
■ Optimize reaction conditions for conducting this chemistry
– Temperature
– Base concentration
– Solvent
– Ligand choice - safety
13. This Study:
Experimental Design
■ Criteria for ligands of choice in investigation
– Bind effectively to Ni
– Minimize steric hindrance for CO oxidation
■ Ligands chosen
– Phosphines (PR3)
– Ammonia (NH3)
– Tetra-amines
16. This Study:
Experimental Design
■ All syntheses in this study took place under aqueous conditions and 1 atm CO
atmosphere
Ligand (mmol) NiCl2*6H2O (mmol) NaOH (mmol) Dichloromethane
(mL)
PPh3, 1.00 ~1.00 ~50 (excess) 30
dppe, 1.00 ~1.00 ~50 (excess) 30
NH3, 1.00 ~1.00 ~50 (excess) 30
3,2,3-N2, N2, 1.00 ~1.00 ~50 (excess) 30
2,3,2-N2, N2, 1.00 ~1.00 ~50 (excess) 30
17. This Study: Results
Ligand Initial Observations Final Observations
(48-72 hrs)
Change in quantity
of CO present
PPh3 Colorless sol’n,
green precipitate
Colorless sol’n,
white precipitate
Decrease
1,2-
bis(diphenylphosphin
oethane) (dppe)
Cloudy orange sol’n,
no precipitate
Light orange sol’n,
some white
precipitate
Decrease
NH3 Purple/blue
homogeneous sol’n,
no precipitate
Purple/blue
homogeneous sol’n,
no precipitate
No change
3,2,3 – N2, N2 Purple homogeneous
sol’n, no precipitate
Colorless sol’n,
white precipitate
Unsure
2,3,2 - N2, N2 Purple homogeneous
sol’n, no precipitate
Colorless sol’n,
white precipitate
Unsure
18. This Study:
Results and Discussion
■ Increase in reaction temperature and base concentration led to quicker CO
volume decrease
– ~10%
■ Use of PPh3 as ligand led to significant CO volume decrease
– Very slow, inefficient due to heterogeneity of conditions
19. This Study:
Results and Discussion
■ Use of dppe as ligand led to significant CO volume decrease
– Quicker than PPh3,
– No Ni0[dppe](CO)2 IR spectroscopic data
■ Use of NH3 led to no CO volume decrease
– No consumption of CO (oxidation), verified by lack of color change
■ 3,2,3-N2, N2 led to significant CO volume decrease
– Quicker than PPh3, single peak observed on IR @ 2040 cm-1
20. Conclusions
■ Increasing temperature and base concentration decreased reaction time
■ dppe and 3,2,3-N2, N2 show encouraging progress as ligand alternatives to CN-
for using Ni complexes to catalyze CO oxidation
■ Future studies
– PPh3 and NH3 failure
– IR data for Ni0[dppe](CO)2
– Crystallographic data for dppe-Ni0 and tetra-amine-Ni0 complexes
– Alternate ligands
Good afternoon everyone
My name is Ilan Hirschfield, interviewing for prod chemist position today here @ Kodak
Presentation as part of visit to showcase my undergraduate research conducted for senior honors thesis, whose topic is CO fuel cell prototype mod through optimizing CO oxidation
Excited to discuss this w/you today b/c it’s an opportunity for me to shed light on understudied portion of inorganic co-ordination chemistry field and its implications for energy consumption
Overview of the structure of my presentation
-Background abt fuel cells and why they’re important, how they work
-Brief review of previous studies involving CO oxidation pointing in this direction
-Goals/design of this study, results/discussion
-Conclusions made from this project, brief period for Q’s at the end
-Fossil fuels make up backbone of energy economy, greenhouse gases produced from burning them and climate impact on them
-Volatile nature of crude oil price makes it difficult for world economies to shoulder burden of fuel price, esp. at current moment w/Russian invasion of Ukraine and sanctions from West buying their oil – true nat’l security issue of sufficient resources for running the economy and social stability
Fuel cells provide energy w/o burning fossil fuels; instead they use other fuels, such as hydrogen, MeOH, or even
So, how does a fuel cell work?
-Anode and cathode sections separated by electrolyte proton exchange membrane (PEM)
-H2 passed thru anode, O2 passed thru cathode
-Catalyst in anode (a) helps oxidize H2 into H+ ions and e-
-H+ passes thru membrane, e- can’t b/c neg charged
-To create equal charge on both sides, e- forced thru circuit to cathode and create electric current
-Catalyst in cathode (c) helps reduce O2 w/H+ and e- to H2O, only product emitted
-When you step back, it’s a brilliant design
-Problem w/cathode side – cost of catalyst (usually Pt, precious transition metal), ORR is very sluggish
Despite those challenges, FCEV’s have been commercialized ; here are 2 ex’s; Toyota Mirai (Mirai means future in Japanese), Chevy Equinox FCEV
Oxidizing H2 as e- source good, but would one of the other 2 fuels mentioned before work? As you could guess from my title, CO can work too!
Take you through previous academic work done that sets the stage for my study
-Windsor/Blanchard: CO oxidation by Ni2+ in basic sol’n possible; first hit, as it were
-Hirsch/Peters: M-COOH intermediate formed in rxn, ability to use this oxidation in catalytic cycle
-Jasinski: Use of non-precious metal catalysts to reduce O2, not able to do so in acidic conditions
-Gewirth/Thorum: greater interest in NPMC’s, particularly TMs, N-based, C-based
-JJ/co: Expanding the CO-atm created coordination complex canon by using CN as ligand
Show you what those complexes look like, trigonal bipyramidal, CN in axial position in both complexes
-Jiang/co(‘15): expanding ‘13 work, these Ni0 complexes under basic conditions and CO atmosphere like ’13
-Set up fuel cell prototypes w/this catalyst, salt bridge, anode/cathode, able to run a small LED for 7 days, ~5.5 mA of current
Catalytic cycle for CO oxidation proposed by JJ/co from ‘15 study, CO fuel cell prototypes underneath
-CO can be a good reducing agent
-BDE of 1072 kJ/mol, arguably strongest naturally-occurring covalent bond, or even naturally-occurring bond, period
-Preceden ce in literature, worth a shot to try moving this project forward
-Minimize reaction time while keeping yield high (fundamentally a kinetics problem)
-Temperature (molecules in rxn moving more quickly, more likely to collide and lead to successful rxn)
-Base concentration (more base molecules around, more likely to collide w/correct molecules to lead to successful rxn)
-Solvent (polarity of solvent, size of solvent molecules influences rxn yield and time taken as well)
-Ligand of interest is safety concern for consumers b/c CN is toxic; exposure leads to damage in central nervous, cardiovascular, and respiratory systems
-What are the conditions we need for choosing good ligands in this study?
-Bind effectively, EDG to maintain stability of metal complex
-Non-bulky motifs to facilitate the desired rxn
-Ligands chosen were:
-Phosphines (generally PR3, R meaning a non-H group) – see specific phosphines used on next slide, will explain the choice there
-Ammonia, basic ligand, small
-Tetra-amines, 4 amine groups on 1 molecule (NRH2, at least 1 R group)
PPh3: Trigonal pyramidal, all benzene rings away from P which binds to metal, clear access to metal center for chemistry to happen - axial positioning of CN it is replacing is key to note here
dppe: Similar to PPh3, but bidentate...usually equatorial position on metal center, still leaves open position for oxidation to happen
Tetra-amines: bidentate too, possibly @ terminal N’s
-Pot setup on L for synthesis rxn’s, Schlenk flask, rubber stopper, mineral oil bath, stir plate, stir bar; add ingredients to pot, close stopper, put on balloon w/CO; as CO used up, mineral oil level goes up on burette to indicate volume change
-FTIR machine on R for analysis of product once rxn is complete
-Setup of the rxn’s for forming new Ni complexes, fairly straightforward and easy to set up and run
-Ran everything under 50 C for the rxn, ran PPh3 again under 75 C or so to determine effect on rxn time
-Ran initial synthesis from ‘15 paper w/higher excess of base (10x)
Based on previous research, colorless sol’n w/white precipitate and decrease in quantity of CO present would indicate successful rxn (b/c valence state of Ni in these complexes would be 0, or neutral, so no color present)
-Results for our different ligands; didn’t have access to notebook w/tetra-amine volume changes when writing up due to COVID lockdown, wasn’t sure abt that part
-Successful w/increasing rxn temp and base concentration, meaningful increase
-PPh3 no good
-dppe great ligand, but no IR confirmation (w/more work it could be obtained)
-NH3 no good
-3,2,3-N2, N2 was good (CO peak that was strong/narrow was observed), didn’t get IR data from 2,3,2-N2, N2 to verify though...
-Optimizing rxn time by focusing on temp and base concentration and ligands
-Great candidates for CN substitutes in Ni complexes to catalyze CO oxidation
-Further studies to determine why PPh3/NH3 failed (computational, mechanistic, maybe...thermodynamics at play too)
-Confirm structures for successful complex formations via x-ray crystallography
-Investigate add’l alternate ligands (tetra-amine derivatives, less bulky phosphenes, etc.)
Thank you to my advisor, Prof. Jiang (goes by JJ) who supervised my work on this research project and whose input and feedback was instrumental in this project’s success
Thank you for your time, and I’ll be happy to take any questions from the audience