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Perovskite quantum dots can capture light and supply energized charges for chemical reactions, but they do not do the whole job alone. In laboratory demonstrations, researchers pair them with catalysts or porous frameworks that help transfer charges, provide reaction sites, or protect the dots from water. Different combinations have produced carbon monoxide, methane, formic acid, and hydrogen peroxide; these are separate research systems, not one universal device.
How the quantum dots help drive chemical reactions
When light excites a perovskite quantum dot (QD), it creates energized electrons and positively charged holes. At a carefully designed interface, electrons can move from the dot to catalytic sites and participate in a reaction before they recombine with holes. The partner material can also affect how reactants reach those sites.
Metal-organic frameworks (MOFs) and covalent organic frameworks (COFs) are porous materials. Depending on their composition and arrangement, they can host the QDs, contribute catalytic sites, change charge transfer, or help shield the dots from water. A separate example pairs QDs directly with a catalyst, nickel-cobalt layered double hydroxide. The benefit depends on the particular combination: these studies do not establish that any framework or catalyst will improve every QD reaction.
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“Artificial photosynthesis” here refers to several distinct light-driven chemical processes. The table keeps the reported products and measurement types separate; the values are not directly rankable.
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| Study | QD and partner material | Reported reaction and result | Important condition or qualification |
|---|---|---|---|
| Wu et al., 2019 | MAPbI3 QDs encapsulated in the iron-porphyrin MOF PCN-221(Fex) | For MAPbI3@PCN-221(Fe0.2), the authors report a combined 1,559 μmol g−1 yield of CO and CH4, with a reported product split of 34% CO and 66% CH4. | Water was the electron source. The authors report the combined yield as 38 times that of PCN-221(Fe0.2) without QDs. This is that study’s comparison, not a general benchmark. The MOF encapsulation was reported to improve stability in water-containing reaction systems. |
| Wang et al., 2023 | All-inorganic CsPbBr3 QDs with NiCo-layered double hydroxide | CO evolution at 204.4 μmol g−1 h−1, with 100% selectivity reported over 35 hours. | The authors attribute photostability partly to oleylamine acting as a sacrificial electron donor. The system should not be described as relying only on water. |
| ACS Catalysis authors, 2024 | CsPbBr3 QDs anchored on a Schiff-based TPA-COF | Reported CO and CH4 formation rates are 41.2 μmol g−1 and 13.7 μmol g−1, respectively. | The reported units do not include an hourly denominator in the result summary, so they cannot be treated as hourly rates. The authors describe enhanced CO2 chemisorption and an S-scheme heterojunction, and report operation without a molecular cocatalyst or scavenger. |
| Applied Catalysis B authors, 2026 | CsPbBr3 QDs encapsulated in dual-metal-site MOFs; the reported sample is CsPbBr3@MOF-919-Cu2Co | CO2 photoreduction to formic acid (HCOOH), with an electron-consumption rate of 669.6 μmol g−1 h−1 and approximately 100% selectivity reported. | The authors compare the sample with pristine QDs, a Cu3 MOF, and a physical mixture; that comparison applies within their study. |
| Nature Communications authors, 2026 | CsPbI3 QDs embedded in a chlorine-functionalized COF | In seawater experiments, the authors report H2O2 production at 20.37 mmol h−1 g−1, a solar-to-chemical conversion efficiency of 1.38%, and stability for 20 hours. | The paper describes simultaneous oxygen reduction and water oxidation without sacrificial agents. In a separate natural-sunlight test, the authors report 11.7 mmol L−1 H2O2 after 10 hours; that concentration is a different metric from the production rate and efficiency. |
Why the performance figures cannot be ranked at a glance
The numbers describe unlike outcomes: a combined product yield, product-formation rates, an electron-consumption rate, an efficiency, a production rate, and a final concentration. Their denominators also differ or are absent. For example, the 2024 CO and methane figures are reported per gram but not per hour, while the 2023 CO figure is per gram per hour. Treating them as equivalent rates would change what the measurements mean.
A fair comparison would also need matching information about the light source and wavelength, electron source or sacrificial donor, product selectivity, test duration, and water composition. Those conditions are not fully specified in the study summaries here, and the reported experiments target different products. The figures therefore show what individual research teams reported, not which design is universally best.
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Water stability is still a practical hurdle
Lead-halide perovskite QDs can degrade in water. Encapsulating them in a framework or engineering an interface may help in a particular reaction system: Wu et al. reported improved stability for MOF-encapsulated MAPbI3 QDs in water-containing tests, and the 2026 seawater study designed its COF interface with aqueous degradation in mind.
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1Scan for outdated or missing drivers - takes under a minute2Repair Windows errors before they cause bigger problems3Fix the driver behind crashes, sound loss and screen glitchesThose results do not establish commercial operating life. A 20-hour stability result in one seawater experiment, for example, is evidence for that test—not proof of durability over months or years. Lead-bearing nanomaterials and bespoke frameworks also remain specialist research materials; the studies do not establish a consumer-ready artificial-photosynthesis device.
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Keep perovskite solar cells distinct from quantum-dot photocatalysts
A 2015 study reported solar-to-CO efficiency above 6.5% using perovskite photovoltaic cells with catalyst electrodes. That architecture uses a solar cell to generate electrical charge and is different from the QD photocatalyst composites described above. Its efficiency does not demonstrate that perovskite quantum dots caused the result.
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