The direct reduction of esters to ethers offers an efficient pathway to ethers from renewable intermediates. This chemistry previously required homogeneous catalysts and utilized costly and unstable hydride reagents. Here, we elucidate pathways for reactions of propyl acetate (C5H10O2) in the presence of hydrogen (H2) over Pd nanoparticles supported on high-surface-area Nb2O5. Over Pd-Nb2O5, C5H10O2 reacts by three competing primary pathways: hydrogenation to form ethyl propyl ether (C5H12O) by apparent CO bond rupture, hydrogenolysis to form acetaldehyde and propanol (Cacyl–O bond rupture), and hydrolysis to form acetic acid and propanol. Secondary reactions yield other alcohols, esters, ethers, and hydrocarbons. Hydrogenation and hydrogenolysis rates do not change with the pressure of C5H10O2 and increase with a sublinear dependence on H2 pressure. Furthermore, these dependencies and apparent activation enthalpies remain similar for Pd nanoparticles with different mean diameters (4–22 nm), which shows that the extent of undercoordination of Pd does not significantly affect the mechanism or kinetics for C–O bond rupture steps. Ether formation rates remain constant when D2 replaces H2 as the reductant, which together with the rate dependence on H2 suggests that ethers form by kinetically relevant C–O bond cleavage in a partially hydrogenated intermediate (e.g., hemiacetal). Ex situ titration of Brønsted acid sites by exchange with K+ ions suppresses mass-averaged rates of C5H12O formation by sevenfold, and physical mixtures of Pd-SiO2 and Nb2O5 give rates more than 10 times lower than Pd-Nb2O5. These results demonstrate that C5H12O formation requires Brønsted acid sites that reside in close proximity to Pd nanoparticles. Collectively, these observations suggest a reaction mechanism for the reduction of esters that hydrogenates the carbonyl by stepwise addition of H* atoms to form a hemiacetal that dehydrates at proximal Brønsted acid sites or cleaves the Cacyl–O bond to form lower carbon number products. These findings reveal a pathway to convert renewable oxygenates, such as carboxylic acid derivatives, into value-added chemicals useful as surfactants and solvents.

Esters reduce to form ethers and alcohols on contact with metal nanoparticles supported on Brønsted acidic faujasite (M-FAU) that cleave CÀ O bonds by hydrogenation and hydrogenolysis pathways. Rates and selectivities for each pathway depend on the metal identity (M = Co, Ni, Cu, Ru, Rh, Pd, and Pt). Pt-FAU gives propyl acetate consumption rates up to 100 times greater than other M-FAU catalysts and provides an ethyl propyl ether selectivity of 34 %. Measured formation rates, kinetic isotope effects, and site titrations suggest that ester reduction involves a bifunctional mechanism that implicates the stepwise addition of H* atoms to the carbonyl to form hemiacetals on the metal sites, followed by hemiacetal diffusion to a nearby Brønsted acid site to dehydrate to ethers or decompose to alcohol and aldehyde. The rates of reduction of propyl acetate appear to be determined by the H* addition to the carbonyl and by the CÀ O cleavage of hemiacetal.

Esters reduce to form ethers and alcohols on contact with metal nanoparticles supported on Brønsted acidic faujasite (M‐FAU) that cleave C−O bonds by hydrogenation and hydrogenolysis pathways. Rates and selectivities for each pathway depend on the metal identity (M=Co, Ni, Cu, Ru, Rh, Pd, and Pt). Pt‐FAU gives propyl acetate consumption rates up to 100 times greater than other M‐FAU catalysts and provides an ethyl propyl ether selectivity of 34 %. Measured formation rates, kinetic isotope effects, and site titrations suggest that ester reduction involves a bifunctional mechanism that implicates the stepwise addition of H* atoms to the carbonyl to form hemiacetals on the metal sites, followed by hemiacetal diffusion to a nearby Brønsted acid site to dehydrate to ethers or decompose to alcohol and aldehyde. The rates of reduction of propyl acetate appear to be determined by the H* addition to the carbonyl and by the C−O cleavage of hemiacetal.