Chemical Kinetics

 76) [NO] = 0.040 M          [O₂] = 0.035 M

       Rate = -Δ[NO]/Δ t = -9.3 x 10^-5 M/s

       2NO(g) + O₂(g) 2NO₂(g)

       (a) Rate = -Δ[O₂]/Δ t = -1/2Δ[NO]/Δ t = -1/2 x -9.3 x 10^-5 M/s = 4.6 x 10^-5 M/s

       (b) Rate = k[NO]²[O₂]

             -9.3 x 10^-5 M/s = k x (0.040 M)² x 0.035 M

             k = 1.7 M^-2s^-1

       (c) M^-2s^-1

       (d) Rate = k[NO]²[O₂]

            -9.3 x 10^-5 M/s = 1.7 M^-2s^-1 x (0.040 M)² x 0.035 M

            -3.1 x 10^-4 M/s = 1.7 M^-2s^-1 x (0.040 M x 1.8)² x 0.035 M

            Rate2/Rate1 = -3.1 x 10^-4 M/s/-9.3 x 10^-5 M/s = 3.3

            Rate2 increases by a factor of 3.3 (1.8²) when NO increases by a factor of 1.8.