The kinetics of the thermal decomposition of Sn2H6 have been studied in the temperature range of -9 to 52 degrees C and found to be first order over the entire range. Above 15 degrees C gas phase nucleation, similar to that observed in SiH4 and Ge2H6 pyrolyses, leads to erroneously high mass spectrometrically measured concentrations of Sn2H6 which precludes obtaining specific reaction rates for the decomposition above this temperature. Arrhenius behavior in the range of -9 to 15 degrees C leads to an activation energy of E-a = 1.28 +/- 0.14 kcal/mol and a preexponential factor of 1.6 +/- 0.5 s(-1) for the decomposition. No higher tin hydrides were observed which, coupled with the original report of Sn2H6 synthesis, indicates that the products are simply Sn(s) and H-2.