Reaction Mechanisms for the Electrochemical Reduction of CO2 to CO and Formate on the Cu(100) Surface at 298 K from Quantum Mechanics Free Energy Calculations with Explicit Water

Copper is the only elemental metal that reduces a significant fraction of CO 2 to hydrocarbons and alcohols, but the atomistic reaction mechanism that controls the product distributions is not known because it has not been possible to detect the reaction intermediates on the electrode surface experimentally, or to carry out Quantum Mechanics (QM) calculations with a realistic description of the electrolyte (water). Here, we carry out QM calculations with an explicit description of water on the Cu(100) surface (experimentally shown to be stable under CO 2 reduction reaction conditions) to examine the initial reaction pathways to form CO and formate (HCOO – ) from CO 2 through free energy calculations at 298 K and pH 7. We find that CO formation proceeds from physisorbed CO 2 to chemisorbed CO 2 (*CO 2 δ− ), with a free energy barrier of Δ G ⧧ = 0.43 eV, the rate-determining step (RDS). The subsequent barriers of protonating *CO 2 δ− to form COOH* and then dissociating COOH* to form *CO are 0.37 and 0.30 eV, respectively. HCOO – formation proceeds through a very different pathway in which physisorbed CO 2 reacts directly with a surface H* (along with electron transfer), leading to Δ G ⧧ = 0.80 eV. Thus, the competition between CO formation and HCOO – formation occurs in the first electron-transfer step. On Cu(100), the RDS for CO formation is lower, making CO the predominant product. Thus, to alter the product distribution, we need to control this first step of CO 2 binding, which might involve controlling pH, alloying, or changing the structure at the nanoscale.