2) The following reaction occurs at 200 K: A + B + C → X Based on the tabulated data from experimentation, what is the experimental rate law? Experiment Initial Concentration, M Initial Rates, M . s-1 A B C 1 0.15 0.30 0.15 4.8*10-5 2 0.15 0.30 0.30 4.8*10-5 3 0.15 0.60 0.15 1.9*10-4 4 0.30 0.30 0.15 9.6*10-5       a) What is the order of the reaction for A, B, and C for the reaction above?  b) Write the rate law for the reaction A + B + C → X at 200 K.  c) Calculate the rate constant (k) for this reaction using the data from experiment 1 (make sure to use units).

Consider the reaction data.   A⟶products ?  (?) ?  (?−1) 325 0.391 575 0.735 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. x1= y1= x1= x2= Determine the rise, run, and slope of the line formed by these points. What is the activation energy of this reaction?

For the reaction A products, concentration and time data were collected. t (s) [A] (M) > 0.0 3.40 Enter these data into the graphing tool to determine the reaction order. 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] [V]

Consider this reaction:                        A    +    B    →    C    +    D Expt. [A] (M) [B] (M) Initial Rate (M/s) 1 0.100 0.100 0.152 2 0.100 0.200 0.152 3 0.200 0.200 0.305   What is the overall reaction order for this reaction?

ConstaEIThe taIDTE OT 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 0.600 0.50 0.325 1.00 0.178 1.50 0.095 2.00 0.050 2.50 0.028 3.00 0.015 3.50 0.008 4.00 0.004

The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 9.90 × 10-10 cm³ molecule-¹.s-¹ at 298 K. Convert the rate constant to units of M-¹.s-¹. k = k = Incorrect Convert the rate constant to units of Torr-¹.s-¹. 5.962 ×10¹7 Incorrect 2 3.208 ×10¹7 What is the order of this reaction? 0 M-¹.s Torr-g

Some measurements of the initial rate of a certain reaction are given in the table below. H2 12 initial rate of reaction 1.47M 1.17M 36.0M/s 1.47M 4.13M 127. M/s 0.591 M 1.17M 14.5 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| x10 k = 0

5. The reaction A →→ B + C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, h 0 1 2 4 8 10 12 [A]. M 1.50 x 10-¹ 1.27 x 10-1 1.07 x 10-1 7.66 x 10-² 3.91 x 10-² 2.80 x 10-2 2.00 x 10-2 (a) What is the average rate of reaction between 1 and 4 h? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 8 h. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.

Consider the hypothetical reaction: P+ Q product. Determine the rate law of the reaction using the provided information. Experiment no. [P]o (M) [Q]o (M) Initial rate (M/s) 1 0.150 0.240 1.54 x 10-3 0.300 0.240 3.08 x 10-3 0.300 0.480 6.16 x 10-3 Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Rate k[P] b. Rate = k[Q] Rate = k[P][Q] d Rate = k[P]? Rate = k[Q]? e

CHAPTER 12 Chemical Kinetics 81. The following data were obtained for the reaction 2A + B → C where rate = d{A]/dt [A](M) [B](M) Initial Rate(M/s) 0.100 0.0500 2.13 x 10-4 0.200 0.0500 4.26 x 10-4 0.300 0.100 2.56 x 10-3 Determine the value of the rate constant. a) 0.426 b) 0.852 c) 0.0426 d) 0.284 e) none of these