The reaction A+2B+C Products has a rate law of Rate =k[A]2[B]. By what factor would the reaction rate change if [B] is tripled? The decomposition of ethylene oxide (CH2)2O(g)CH4(g)+CO(g) is a first order reaction with a half-life of 58.0min at 652K. The activation energy of the reaction is 218kJ/mol. Calculate the half-life at 629K. What is the concentration of A after 50.7 minutes for the second order reaction A Products when the initial concentration of A is 0.250M ? (k=0.117M1min1) The gas phase decomposition of NO2(g) 2NO2(g)2NO(g)+O2(g) obeys the second order rate law, Rate =k[NO2]2, with a rate constant k =0.543M1s1 at 300C. Starting with [NO2]=0.250M, how long will it take for the [NO2] to decrease to 5.00% of its starting value