1. The problem statement, all variables and given/known data 2 KClO3 (s) + heat --> 2 KCl (s) + 3 O2 (g) If 0.20 g of KClO3 (s) decomposes in 2.8 s, at what rate is oxygen O2 (g) released over this time at SATP? 2. Relevant equations n = PV/RT 3. The attempt at a solution Converted KClO3 to mol. .20 x 1 / 122.5495g = 0.001632 mol KCl Find rate of decomposition : .001632 mol in 2.8 sec --> 2 mol in 3431.37 sec 2/3431.37 = .000583 mol/s The rate of decomposition of KClO3 is .000583 mol/s I'm stuck at this part. I know I need to use some sort of n = PV/RT since it tells me that it is at SATP. Can I have some hints or help?