The reaction 2NO(g) + O2(g) → 2NO2(g) exhibits the rate law Rate = k[NO]2[O2] Which of the following mechanisms is consistent with thus rate law? a, NO+O2 → NO2+O slow O+NO → NO2 slow b. NO+O2 ⇌ NO3 Fast equilibrium NO3+NO → 2NO2 slow c. 2NO → N2O2 slow N2O2+ O2 → N2O4 Fast N2O4 → 2NO2 Fast d. 2NO ⇌ N2O2 Fast Equilibrium N2O2 → NO2+O2 slow O+NO → NO2 Fast

Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.55M 0.638M 14.0M/s 0.601 M 0.638M 2.10M/s 1.55M 1.92M 127.M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 ▬ x10 X 00 5

Determine the rate law and calculate the rate constant for this reaction: 2 NO (g) + Br₂(1)→2 NOBr (g) Initial [Br₂]/M Expt. 1 2 3 Initial [NO]/M 0.10 0.20 0.20 0.10 0.10 0.30 Initial rate/M.s-¹ 1.30 x 10-³ 5.20 x 10-³ 1.56 x 10-²

16.  The decomposition of hydrogen bromide is 2 HBr(g)    →    H2(g)  +  Br2(g) The reaction has rate constants of 7.23 x 10-8 M-1 s-1 at 5.00 x 102 K and 9.14 x 10-6 M-1 s-1 at 6.00 x 102 K. What  is the activation energy in kJ/mol? Group of answer choices 136 kJ/mol none of the answers are correct 145 kJ/mol 107 kJ/mol 121 kJ/mol