For a gas-phase reaction 2NO(g) +H2(g) N2O(g) +H2O(g), the rate law can be expresseddp (N₂O)asdtkpop₂The data in table have been obtainedRunp°(NO)/kPa p°(H₂)/kPa Half-time/sT/K180.01.3319.21093280.02.6619.2109331.3380.0830109342.6680.04151093580.01.33101113(The runs are at constant temperature and volume)(a) Determine the order of the reaction (a and b) with explanation.(b) Estimate k at 1093 K.

(a) Determine the order of the reaction (a and b) with explanation. Determining the Order of the…

Answered: For a gas-phase reaction 2NO(g) +H2(g)…

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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Consider the reaction data. A⟶productsA⟶products ? (?)T (K) ? (?−1)k (s−1) 275275 0.3800.380 675675 0.7470.747 a)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 value x1=? x2=? y1=? y2=? b)Determine the rise, run, and slope of the line formed by these points. c)What is the activation energy of this reaction?
In a study of the gas phase decomposition of nitrosyl chloride at 400 K NOCI(g)NO(g)+½ Cl½(g) the following data were obtained: NOCI], M seconds 2.54x10-2 3.75x104 1.27x10-2 1.13×105 6.35x103 2.63x105 5.08×10-2 0 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 5.08x10² M is Js and when the starting concentration is 2.54×10-2 Mis (2) The average A(1/[NOCI]) / At from t= 0 s to t = 3.75×104 s is The average A(1/[NOCI]) / At from t= 3.75x104 s to t= 1.13×105 s is| (3) Based on these data, the rate constant for this| | order reaction is
I just need to know if all my work/calculations with this lab report are correct, thank you so much!
For the reaction 2HI (g) = H2 (g) + I2 (g) we have the following data T/k K (dm3 mol-1s-1) 556 3.52 X 10-7 781 3.95 X 10-2 Determine: 1) The fraction of molecules with enough energy to react at 700k. 2) The time required for the reaction to be 80% complete at 600k if [HI]0 = 0.020 mol/dm3
The rate law for the decomposition of A→P is investigated by measuring the initial rate of the reaction for several concentrations of A. The data are shown below. Assuming that the rate law is of the form v=k[A]n, use a graphical method to determine the value of n. [A]/M Initial Rate/(Torr s-1) [A]/M Initial Rate/(Torr s-1) 1.000 0.1422 0.700 0.0718 0.950 0.1248 0.650 0.0625 0.900 0.1123 0.600 0.0518 0.850 0.0983 0.550 0.0445 0.800 0.0857 0.500 0.0382 0.750 0.0782
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For the gas phase decomposition of t-butyl acetate, CH3COOC(CH3)3→(CH3)2C=CH2 + CH3COOH the rate constant has been determined at several temperatures. When In k in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.04x10* K and a y-intercept of 30.7. The activation energy for the gas phase decomposition of t-butyl acetate is kJ/mol.
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.
tab esc slock ||| = OKINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism with an initi.... Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) + O₂ (g). -NO₂(g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O5 (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. BE 1 Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Explanation Q A @ 2 Check W S X # 3 E 0 rate = k 14 D $ 4 rate constant > R F % 5 © Stv T MacBook Pro 6 G We Y & 7 H 0-0 U 00 Ⓒ2022 McGraw Hill LLC. All R You * 00 00 8 S a (
1. For the reaction A + B D+E the following mechanism was suggested k1 A+ B 20 k3 A +D k4 2B E Derive the rate low by applying any inequalities condition you deem appropriate! 2. The reaction 3Ce* + Cr* 3Ce* + Cr* has an experimentally determined rate aw given by: d[Cr®* ] = k dt [Cr* ][Ce* J° [Ce* ] ex Show that the mechanism ki Ce4+ + Cr³+ Cr++ + Ce3+ k2 Ce4+ + Cr+ - Cr+ + Ce3+ k3 Ce+ + Cr*+ Cró+ + Ce³+ will account for the empirical rate low provided certain inequalities exist and by applying the steady-state approximation (SSA).
Please solve correctly, find value of x,y,z

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