Consider the following data obtained in a second order reaction: NO2(g) N204(g) ---- Time (min) [NO2], M 1.20 2.3 0.88 5.0 0.67 6.4 0.60 9.0 0.50 10.6 0.45 12.8 0.30 What is the rate constant for the reaction?

A study of the rate of the reaction represented as 2 A → B gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 [A] (M) 1.00 0.776 0.603 The instantaneous rate for the reaction at t = 10.0 s is 30.0 0.468 0.363 0.282 0.219 M/s.

6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179

The reaction A → C was performed and the concentration vs. time data below collected.   time, s 0 1 2 3 4 5 6 7 8 [A], mol/L 0.9541 0.5884 0.3629 0.2238 0.1380 0.08512 0.05250 0.03238 0.01997   Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]x rate constant (without units) =

Consider the reaction: A + B --> products.  From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant:   [A] (M)                       [B] (M)                       Rate (M/s)   1.50                             1.50                             3.15 X 10-1 1.50                             2.50                             2.98 X 10 –1 3.00                             1.50                             5.50 X 10-1

Determine the rate order and rate constant for dinitrogen pentoxide. Time (minutes) [N2O5] 0 0.0165 10.0 0.0124 20.0 0.00930 30.0 0.00710 40.0 0.00530 50.0 0.00390 60.0 0.00290 Group of answer choices First-order, k = 0.0289 minute-1 First-order, k = 0.0126 M-1⋅minute-1 Second-order, k = 4.59 M-1⋅minute-1  Zero-order, k = 0.000200 M/minute Zero-order, k = 0.0148 M/minute Second-order, k = 30.8 M-1⋅minute-1

The decomposition of hydrogen peroxide was studied at a particular temperature. The following data were obtained, where Time (s) [H,O,] (mol/L) 1.00 120 0.91 300 0.78 600 0.59 1200 0.37 1800 0.22 2400 0.13 3000 0.082 3600 0.050 Determine the reaction order and the value of the rate constant.