2. The initial rate of the reaction of P +Q→ products was experimentally determined. [P], M [Q], M Initial rate, M/s 3.35 x 10 1.35 x 10 Reaction Trial 1. 0.185 0.144 2 0.185 0.288 0.370 0.144 6.75 x 10 4 0.370 0.288 2.70 x 10 a. What is the order of the reaction with respect to A? b. What is the order of the reaction with respect to B? c. What is the overall reaction order? d. What is the value of the rate constant, k?

Experimental data for the reaction A + 2B → C have been plotted in the following three different ways. 0.05 -3.0 0.04 0.03 0.02 0.01 0 IvI 0 2 Time (s) 1/[A] 100 80 40 20 0 In[A] -3.5 -4.0 -4.5 -5.0 0 2 Time (s) 2 Time (s) What is the order of the reaction, and what was the initial concentration of A? O first-order, initial concentration = 10 M second-order, initial concentration = 10 M zero-order, initial concentration = 10 M O second-order, initial concentration = 0.1 M O first-order, initial concentration = 0.1 M

Some measurements of the initial rate of a certain reaction are given in the table below. [N-] N2 H2 initial rate of reaction 1.27M 0.589М 22.0M/s 1.27 M |0.149 М 5.57 M/s 0.445 M 0.589M 2.70M/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 |I| х10 k =

Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.

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) =

The following data were collected for a certain reaction of the type A +B → products. Determine the specific rate constant for this reaction. [A]o, mol L-1 [B]o, mol L-1 Initial rate, mol L-1 s-1 Run i 0.200 0.300 2.44 x 10-2 ii 0.200 0.450 2.44 x 10-2 i 0.300 0.450 5.49 x 10-2 O A. 0.610 L mol s-1 B. 0.960 L mol1 s-1 C. 0.271 L mol-1 s-1 D. 0.407 L mol-1 s-1 O E. 0.120 L mol-1 s-1

Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A] (M) 0.00 0.450 0.50 0.300 1.00 0.225 1.50 0.180 2.00 0.150 2.50 0.130 3.00 0.115 3.50 0.100 4.00 0.090

What is the rate of the reaction when A=0.43M and B=0.31M?

Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A](M) 0 0.5 1.5 0.42 3 0.335 4.5 0.25 6 0.17 7.5 0.085 9 0.003