1. The problem statement, all variables and given/known data Lets say you have 1 liter of 2 mol/L methane and the same amount of chlorine. Lets also say that both are liquids since those are most likely to react. Now the only way they can both be liquids is if the temperature is as cold as an antarctic winter so this is not aqueous. Gases more often bump the wrong way and solids don't react unless it is oxidization or dissolving. Now the initiation step is forming the first molecule of HCl and Methyl. Now the methyl and chlorine atom really want to react and for chloromethane Now here are the questions. How much chloromethane, dichloromethane, trichloromethane, and tetrachloromethane will there be? How much of the more complicated alkanes like ethane and propane will there be? How many molecules made up of more complicated alkanes and chlorine will there be? Will at some point the chlorine go back to its normal state and the hydrogen go back to the carbon so that you have just methane, ethane, propane etc? 2. Relevant equations CH4 + Cl2 = HCl + CH3Cl(this continues up to tetrachloromethane) 2 CH3Cl = Cl2 + C2H6(this can continue for much longer than the previous one can) 3. The attempt at a solution 2 M CH4 + 2 M Cl2 = 2 M HCL + 2 M CH3 + 2 M Cl 2 M Cl + 2 M CH3 = 2 M CH3Cl 2 M CH3Cl * 2 CH3Cl = 1 M C2H6 + 1 M Cl2 2 M HCl = 2 M H2 + 2 M Cl2 This obviously can't happen because than we have more chlorine than we started out with. Why? well that 1 M Cl2 from ethane + 2 M Cl2 from HCl is = 3 M Cl2 and we started with 2 M Cl2. Just like the number of each element the molarity has to be balanced. This is where I am stuck is figuring out the molarity of each compound at each step of the process not the compounds themselves.