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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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
X Cut AaBbCcl AaBbCcDc AaBbCcD AaBbCcE AaB AaBb CcC Aa8be T No Spac. Heading 2 Calibri (Body) | AA Aa. E , 刻T Copy Paste Subtle Title Subtitle BIU abc x, x A - y- A- Heading 1 T Normal Format Painter Paragraph Styles Font Clipboard I 10 11 6. From the data variation of the reaction rate of the following temperatures: 1500 T (K) k (M1 second ) 500 1000 5,49 x 106 9,86 x 108 5,09 x 10° Specify: a. Amount of Activation Energy (Ea) b. Magnitude of the pre-exponential factor (A)
4. Determine the order of the following reactions from the rate constant. a. k= 1.3 x 104 s-1 b. k = 4.7 x 10-² mol L-'s'
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
PS. this is not graded.
For items 7 - 11. Select the correct answers on each item. PS. this is not graded.
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?
Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
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
Explain too do only a and b
Rate = k [A] [B]² Overall reaction order would be A. 0 В. 1 С. 3 D. 2 What is the connection between rate and temperature ? A. There is no connection between the two B. Rate is indirectly connected to temperature C. Rate is directly related to temperature in exothermic reactions and indirectly related to temperature in endothermic reactions D. Rate is directly connected to temperature E. Rate is indirectly related to temperature in exothermic reactions and directly related to temperature in endothermic reactions
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