Kinetics of the reaction Br + CH2ClBr <-> CHClBr + HBr (1, -1) were studied experimentally in the forward direction. The absolute reaction kinetics method of laser flash photolysis coupled with Br atom resonance fluorescence detection and three different relative-rate methods with gas-chromatographic analysis were applied to carry out the experiments. The rate constants determined were found to obey the Arrhenius law in the wide temperature range of T = 293-785 K providing the kinetic expression k(1) = (2.8 +/- 0.1) x 10(13) exp[-47.6 +/- 0.3) kJ mol(-1)/RT] cm(3) mol(-1) s(-1) (the errors given refer to 1 sigma precision). An ab initio direct dynamics method was used to study reaction (1,-1) theoretically. The electronic structure information including geometries, gradients, and force constants was obtained at the MP2 level of theory; and energies were improved at higher theoretical levels. Rate constants were calculated using the canonical variational transition state theory with small-curvature tunneling correction over the temperature range 200-1000 K. Theory substantially underestimates k(1) compared to experiment. The agreement was found good with k(-1) reported previously predicting positive temperature dependence. The experimental kinetic parameters were utilized in thermochemical calculations yielding the recommended standard enthalpy of formation of Delta H-f degrees(298) (CHClBr) = (140 (4) kJ mol(-1) (with 2 sigma accuracy given).