The following mechanism for the gas phase reaction of nitrogen dioxide with carbon monoxide at temperatures above 225 °C is consistent with the observed rate law. step 1 fast: NO2+COONOCO step 2 slow: ONOCO>NO+CO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[Al\" [B]\"..., where \'T\' is understood (so don\'t write it if it\'s a \'I\') for m, n etc Rate- Solution 1) .NO2 + CO = NO + CO2 this is the overall reaction . 2). ONOCO intermediate. 3 ) . rate = k [NO2] [CO] ,this is the rate expression . . .