1. The problem statement, all variables and given/known data CH3OCH3(g) ---> CH4(g) + H2(g) + CO(g) The reaction is conducted at 777.15 K, at constant volume beginning with pure ether. Code (Text): t(hours) 0 390 777 1195 3155 +inf P (torr) 312 408 488 562 779 931 Determine the order of the reaction and approximate the rate constant. 2. Relevant equations 1) PV = nRT 3. The attempt at a solution I know I need a number of moles. Pressure is related to moles as stated by equation 1. Unless I assign an arbitrary value to V, I cannot calculate a value for n. I have written this table: Code (Text): A --------------> 3B t=0 a 0 t a-x +3x t=+inf 0 3a I know I have to convert P(tot) in P(ether) using: P(tot) = (nA + nB) RT/V and P(ether) = nA RT/V But erm.... major brainfreeze. (as is usually the case when trying to study after a big meal lol!) Thanks in advance.