NO2 (g) reacts with O2 4 NO2 (g) + O2(g) to produce N2 O5 (g) as shown by the equation below: (g) = 2 N2 O5 (g). Experimentally the rate orders were determined and rate law written as shown below: Rate = k [NO2]2[O2 ].
Calculate the value of k if the initial concentration of NO2 was 0.250 M and initial
concentration of O2 (g) was 0.150 M. The initial rate was 1.25 x 10-2 M. s-1 .

Answer asap need by wednesday morning explain how a buffer works, using an ethanoic acid/sodium ethanoate system including how the system resists changes in ph upon addition of a small amount of base and upon addition of a small amount of acid respectively. include the following calculations in your i. calculate the ph of a solution made by mixing 25cm3 0.1m ch3cooh and 40cm3 0.1m ch3coo-na+. [ka = 1.74 x 10-5 m] ii. calculate the ph following the addition of a 10cm3 portion of 0.08 m naoh to 500cm3 of this buffer solution. iii. calculate the ph following the addition of a 10cm3 portion of 0.08 m hcl to 200cm3 of the original buffer solution.