decomposition reaction of atmospheric peroxyacetylnitrate (PAN) roducts was studied, and the following rates were obtained. Temperature, "C Rate constant, s .00 5.60x 10 100 3.20x 10 200 1.60 x 10 30.0 7.60- 10 Fit this data into the Arrhenius equation. Give the values of the owing pe Select mtercept ISelect arson coeficient (R) Select tivation energy of this reaction in k/mol Select

decomposition reaction of atmospheric peroxyacetylnitrate (PAN) roducts was studied, and the following rates were obtained. Temperature, "C Rate constant, s .00 5.60x 10 100 3.20x 10 200 1.60 x 10 30.0 7.60- 10 Fit this data into the Arrhenius equation. Give the values of the owing pe Select mtercept ISelect arson coeficient (R) Select tivation energy of this reaction in k/mol Select

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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Rate information was obtained for the following reaction at 33 °C; The value of the rate constant k = 2 x 10³ at 25°C. Cr(H₂O)6³+ + SCN ---> Cr(H₂O)5NCS²+ + H₂O(1) @33 °C Initial Rate 2.0x10-¹1 2.0x10-10 9.0x10-10 2.4x10-⁹ 1.4x10-10 [Cr(H₂O)6³*] 1.0x104 1.0x10-³ 2.0x10-³ 3.0x10-³ 1.0x10 [SCN"] 0.10 0.10 0.15 0.20 0.20
Consider the following complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.
The activation energy for a reaction is determined to be 389.9 kJ. The rate constant at 20.5ºC is equal to 4.06 x 10-6 s-1. What is the rate constant at 34.9ºC for the reaction? Report your answer to the tenths place and using scientific notation (e.g. 1.27 x 103 or -1.27 x 10-3) and do not include units
The chemical equation corresponding to the hydrolysis reaction can be written: R-CI+ H2O →R-OH+CI¯+ H* Let's call a the initial concentration in 2-chloro-2-methyl-butane and x the concentration of hydrochloric acid that is formed at time t. Water remains in large excess all over the course of the reaction. Then one can write: R-l + H20 Cexcess) > R-OH +d-+ht at to, a at t>0, a-se at tD, a a a 05: Recall the Arrhenius law and explain the meaning and unit of the individual terms. Deduce an expression of the activation energy as a function of two temperatures T1 and T2.
Can my answers be checked please thank you .
4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.
State the types of each catalyst whether it's homogeneous catalysis heterogeneous catalysis or Biocatalysis 1. fetts ɔ. febrs 4. Fe(OTF)2 5. FelCI O4)2 · x H2O 6. Pda. 7 PdCl2 CM CN)2 8. Pd cacac)2 9 Pd Clz (PPh3), 10. Pd COA c)z [1. NaHSOy H20 9 Nalsor Ho 12. CH 3 SO3 H 13. AI(NOs) 9 H20 14. H3 040 PW12. XH2O 15. Fe: (S04)3 •9 HzO 16 Sn Cly• 5H2 O
For the decomposition of nitramide in aqueous solution at 25 °C NH,NO,(aq)N,0(g) + H2O(1) the following data have been obtained: NH,NO2], M 9.12x10-2 217 2.69x10-2 651 0.168 4.95x10-2 434 time, min The average rate of disappearance of NH,NO, over the time period from t = 0 min to t= 217 min is M min!.
23 II. An experiment followed the decomposition. of nitregen dioxide to nitregen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |[NO₂] (M) 0.0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M G 2 XX 6.5 Hoa X019 201 2(x) = 2 (1.86) (3 (9)
How do you write the overall rate law with the k value specific to this reaction?
For the gas phase decomposition of hydrogen peroxide at 400 °C2 H2O22 H2O + O2the average rate of disappearance of H2O2 over the time period from t = 0 s to t = 7 s is found to be 1.61×10-2 M s-1.The average rate of formation of O2 over the same time period is ? (answer in M s-1.)
A reiction is described as follows: 2A (g) + 2B (g) -+C (g) Exp. (A). M Initial rate (x10* Ms') 0.15 0.15 0.15 1.24 2.46 4.95 2. 032 0.15 3 0.30 From the data given above, determine the followings: (1) The rate law formula in terms of formation of product C, (ii) The overall order and the order with respect to each component, (ii) The rate constant (state clearly its units and coefficients), (iv) Find the rate of reaction when (A] - [BI =0.20 M.