The rate constant of the elementary reaction CH3CONH2(g)CH2CO(g)+NH3(g) is k=7.08103s1 at 679C, and the reaction has an activation energy of 307kJ/mol. Compute the rate constant of the reaction at a temperature of 746C. k=7.64s1 At a temperature of 679C,9.79101s is required for half of the CH3CONH2 originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 746C ? t=s