can you write out the formulas with the calculations please! im stuck on this one

15 Question (1 point) The reaction of NO2 with ozone produces NO3 in asecond-order reaction overall: NO2(g)+O3(g)NO3(g)+O2(g) 1st attempt Part 1 (0.3 point) What is the rate law for the reaction if the reaction is first order in each reactant. Choose one: rate=k[NO2][O3]rate=k[NO2]2[O3]rate=k[NO2]2[O3]2rate=k[NO2][O3]2 If the rate constant for the reaction is 1.91104M151 at 298K. What is the rate of the reaction when [NO2]=2.67103M and [O3]= 1.09107M ? 1025M/s= Part 3 ( 0.3 point) What is the rate of the appearance of NO3 under these conditions