The kinetics of Al2O2+ + CH4 and Al2O2+ + C2H6 are measured from 300 to 600 K at pressures near ∼0.35 Torr in a Selected-Ion Flow Tube apparatus. The reaction with CH4 proceeds by hydrogen abstraction to yield an open chain AlOAlOH+ +CH3. The rate constant is nearly temperature-independent at 7 ± 2 × 10−11 cm3 s−1. This competes with association, which decreases sharply with temperature (k = 3.3 ± 0.8 × 10−10 (T/300 K)−3.1±0.2 cm3 s−1). The reaction with C2H6 primarily yields Al2O2H2+ + C2H4. The rate constant for this channel k300K = 4 ± 1 × 10−10 cm3 s−1 with a very slight negative temperature dependence. A second channel producing C2H5 + Al2O2H+ rises steeply with temperature (k = 10 ± 2 × 10−10 e−0.12 eV/kT cm3 s−1), and finally association decreases steeply with temperature (k = 6 ± 1.5 × 10−10 (T/300 K)−3.2±0.2 cm3 s−1). The reaction with methane is well-described using statistical theory based on reaction coordinates calculated using density functional theory. The total rate constant for the ethane reaction is also well-described using statistical theory, but the product branching is not, suggesting post-transition state non-statistical dynamics. One possibility is that the ethane reaction unexpectedly produces a higher energy C2v isomer of Al2O2H+. The results support the prior interpretation that Al2O2+ activates hydrocarbons via a proton-coupled electron transfer (PCET) mechanism and not a hydrogen-atom transfer (HAT) mechanism.