4) The following reaction is second order with respect to NO and zero order in O2:2NO+O22NO2. If the rate constant is 4.67103M1s1, find the following if the initial concentration of NO=0.750M : a. The concentration of NO after 500 s have passed. b. How much time has passed for the concentration to be reduced to 1/2 of the initial? c. The time when the [NO] will be 0.500M. d. The initial reaction rate. 5) The proposed mechanism for the reaction in question 2 is as follows: NO+NOk1k1N2O2(equalandfast)N2O2+H2H2O+N2O(slow)N2O+H2N2+H2O(fast) a. Which is the rate determining step? b. Identify any intermediates in the reaction. c. Sum together the three steps to verify you get the same reaction from question 2 . d. Determine the rate law using the mechanism above. Remember, the rate law cannot be written with intermediates