r = L [A] [B] ²x2 x 2r=k [2A) [21] ²8x bigger than2 + 4 = 812. Consider a reaction of the form 2A + BC. The data for this reaction is given below:Initial rate of formation of C M/sInitial [A]Initial [B]4.0 x 10-²0.300.102.0 x 10-²0.500.056.0 x 10-²0.500.151.0 x 10-²0.025a. What rate law is consistent with this data?0.40b. Calculate k and specify units.How long will it take for the concentration of C to equal to 0.10 molar if the initial concentration of allthe species are [A] = 0.4 M, [B] = 0.3 M and [C] = 0.0 M?

2+4=8 ale 12. Consider a reaction of the form 2A + BC. The data for this reaction is given below: Initial rate of formation of C M/s Initial [A] Initial [B] 4.0 x 10-² 2.0 x 10-² 6.0 x 10-² 1.0 x 10-² a. What rate law is consistent with this data? b. Calculate k and specify units. 0.30 0.50 0.50 0.40 0.10 0.05 0.15 0.025 How long will it take for the concentration of C to equal to 0.10 molar if the initial concentration of all

2+4=8 ale 12. Consider a reaction of the form 2A + BC. The data for this reaction is given below: Initial rate of formation of C M/s Initial [A] Initial [B] 4.0 x 10-² 2.0 x 10-² 6.0 x 10-² 1.0 x 10-² a. What rate law is consistent with this data? b. Calculate k and specify units. 0.30 0.50 0.50 0.40 0.10 0.05 0.15 0.025 How long will it take for the concentration of C to equal to 0.10 molar if the initial concentration of all

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The following data was collected for the reaction: A + B + C = Products Experiment Initial concentration (mM) Initial Rate (mM.s-1) A B C 1 1.25 1.25 1.25 8.7 2 2.5 1.25 1.25 17.4 3 1.25 3.02 1.25 50.8 4 1.25 3.02 3.75 457 5 3.01 1.00 1.15 ? Write the rate law for the reaction What is the order for the reaction? Use the data to predict the reaction rate for experiment 5
3. You have a reaction that is run at 273°C and has a rate constant of 2.52 x 10/s. The same reaction is run at 157 °C and has a rate constant of 1.0 x 10-/s. What is the activation energy for this reaction? (R = 8.314 J/mol K) %3D 0.00898mols 102 sec 4. w for ate= k[NO2]?. The rate constant for this reaction: If yo tion for 5 minutes urd be the concentra
3. Reaction A  products was monitored as a function of time. If a plot of 1/[A] vs. time yield a straight line with slope 0.0050 M-1 s-1. If initial concentration [A]0 = 0.250 M, calculate the concentration of A after 20 seconds
Select the rate law that corresponds to the data shown for the following reaction A + B --> C Exp. _Initial [A] Initial [B] Initial Rate 1 0.012 0.035 0.10 2 0.024 0.070 0.80 3 0.024 0.035 0.10 4 0.012 0.070 0.80 A. Rate = k[A]3 B. Rate = k[A][B]3 C. Rate = k[A]2[B]2 D. Rate k[B]3
For the following reaction 5 experiments have been run and the data collected is in the following table: 4 HBr(g) + O2(g)--->2 Br2(g) + 2 H2O(g) Experiment [HBr], M [O2 ], M Rate, M/s (aka mol/L.s) 1 0.120 0.490 0.0267 2 0.142 0.120 0.00190 3 0.120 0.630 0.0442 4 0.230 0.630 0.0846 5 0.630 0.863 0.435 a)Write the rate expression. b) Calculate the rate constant, k c) If the concentration of HBr and O2 are 1.5 x 10-3 M and 3.25 x 10-3 respectively, what is the rate of the reaction?
Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 2.00 x 10-6 4.00 x 10-6 6.00 x 10-6 Determine the value and units of the rate constant. units:
Consider the reaction shown below and the tabulated experimental data on initial rates. A +B +2 C→D+ E Table 1. Initial concentrations of reactants and the corresponding rates at 25 °C Rate (M/s) [A]; (M) [B]; (M) [C]; (M) 0.390 0.10 0.10 0.30 0.130 0.10 0.10 0.10 0.975 0.10 0.25 0.30 0.585 0.15 0.10 0.30 A. Determine the reaction order with respect to A, B, and C. B. Calculate the average rate constant for the reaction. C. What is the rate law for the reaction and the overall reaction order? . D. Calculate the activation energy (E.) for the reaction assuming that the frequency factor (A) is 1.23 x 010 /M²s. ( E. What is the rate constant at 50 °C?
If the order of the reaction is first order for both reagents then using the rate law and the following data solve for K. Rate 1.9 X 10^-6 [I-] = 0.45 M [H2O2] = 0.125 M O A. 1.1 X 10^-5 O B.3.4 X 10^-5 O C. 3.4 X 10^-4 O D. 1.1 X 10^-7
The rate constant for the formation of hydrogen iodide from the elements H₂(g) + 1₂(g) → 2Hİ(g) is 2.7 x 10-4 L/(mol-s) at 600 K and 3.5 x 10-3 L/(mol·s) at 650 K. a. Find the activation energy Ea. J/mol b. Then calculate the rate constant at 719 K. L/(mol.s)
4. Consider the following data for the decomposition of hydrogen peroxide 2 H.Ог (аq) —> 2 H.О (1) + Оz (g) Concentration H2O2, mol/L (y axis) Time, s (x axis) 2.32 1.86 300 1.49 600 0.98 1200 0.62 1800 0.25 3000 a. Prepare a graph of concentration H,O2 vs time. b. Prepare a graph of log [H2O2] vs time. c. Determine the slope of the line for the graph in (b).
14. Consider the following reaction: 2 N₂O(g) → 2 N2(g) + O2(g) rate - k[N₂O] For an initial concentration of N₂O of 0.50 M, calculate the concentration of N₂O remaining after 2.0 min ifk -6.8 x 10³ s¹¹. A) B) 0.98 M 0.39 M C) 0.86 M D) 0.22 M E) 0.75 M