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...

See similar textbooks

Similar questions

The reaction described by H, (g) + 1,(g) → 2 HI(g) has an experimentally determined rate law of rate = k [H2][I2] Some proposed mechanisms for this reaction are: Mechanism A (1) H, (g) + L,(g) 2 HI(g) (one-step reaction) Mechanism B (1) 1,(g) =2 1(g) (fast, equilibrium) k_1 (2) H, (g) + 2 I(g) –→ 2 HI(g) (slow) Mechanism C (1) I, (g) = 2 I(g) (fast, equilibrium) k_ k, (2) I(g) + H, (g) –→ HI(g)+H(g) (slow) (3) H(g)+I(g) → HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? O mechanism A O mechanism B O mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an I, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? O mechanism B O mechanism C O mechanism A
1. The rate of the homogeneous gas-phase reaction: A + 3B → 2X + Y has been studied. Some of the data are: Initial total pressure change rate (-dP/dt) / (torr/s) Initial pressure A P/ torr 352 289 Initial pressure B P/ torr Run 153 392 3.44 6.55 8.14 3 4 247 617 (a) What are the orders of the reaction with respect to A and with respect to B? (b) Assume that the gas mixture is ideal and find the relation between the usual rate of reaction, v, and dP/dt, where P is the total pressure. The volume is constant.
Want solution asap
Concentration-Time Relationships (See Section 15.4 and Examples 15.5-15.7.) 15. The rate equation for the hydrolysis of sucrose to fruc- tose and glucose CRH2O1(aq) + H¿O(€) → 2 C,H12O6(aq) is -A[sucrose]/At = k[C¡2H2O1]. After 27 minutes %3D at 27 °C, the sucrose concentration decreased from 0.0146 M to 0.0132 M. Find the rate constant, k.
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 reaction is described as follows: k1 X + Y The table below shown the initial rates of the formation of product Z (Vo) for various reactant concentrations. From the data given, answer the followings: [X], mol L- [Y], mol L-1 34 Vo (x 103 mol L-s') 22 1.00 70 45 4.20 8.08 71 89 (i) The rate law of formation of product Z, (ii) The overall rate order and the order with respect to each component, and (iii) The rate constant (state clearly its units and coefficients).
for this reaction (including orders). Also give the overall order for this reaction: rate law: overall order = %3D 3. Calculate the rate constant, k, for this reaction (use the data from Experiment #1, show all your work): wollood 4. Explain exactly what experiment(s) must be performed in order to
For the gas phase decomposition of ethyl acetate, CH;COOC,H,–CH,COOH + C2H4 the rate constant has been determined at several temperatures. When In k -1 in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.41x10* K and a y-intercept of 28.8. The activation energy for the gas phase decomposition of ethyl acetate is kJ/mol.
For a first-order reaction k A + B time t = 0 s 4.878 1.004 M time t = 19.84 s ? M when k = 0.030329 s-1 what is the concentration of B above in the question mark= _M? 3 sig. fig. normal format. Try to plot concentrations of A, B and rate over time in Excel.
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.
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y = mz +b. • Part A Order Integrated Rate Law Graph Slope [A] =- kt + [A]Jo -kt + In[A]o In[A] vs. t + = kt + TAT [A] vs. t -k The reactant concentration in a zero-order reaction was 7.00x102 M after 170 s and 3.00x102 M after 380 s. What is the rate constant for this reaction? 1 In[A] = -k Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. 1 - vs t JA 2 • View Available Hint(s) ? koih = Value Units Submit Prevlous Anawera Part B Complete previous part(s) • Part C The reactant concentration in a first-order reaction was 6.60x102 Mafter 30.0 s and 7.70x10 Mafter 100 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a…
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 (

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS