In a study of the decomposition of hydrogen iodide on a gold surface at 150 °CHI(g) ½ H2(g) + ½ 12(g)the following data were obtained:[HI], Mseconds0.44500.2235200.1127795.60x102911Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.445 M isstarting concentration is 0.223 M isS.(2)The average rate of disappearance of HI from t = 0 s to t = 520 s is(3)The average rate of disappearance of HI from t = 520 s to t = 779 s is(4)Based on these data, the rate constant for thisorder reaction isMs.MsMs1Is and when the

1) Half life time is the time required to convert half of the reactant into product.Here ,Initial…

Answered: In a study of the decomposition of…

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

6) The decomposition of reactant R was studied, and the data given below was obtained at 100.0 °C: R> products time (min) concentration (M) 0.120 35.6 5.83 17.8 25.6 0.0910 0.060 0.046 0.030 a) What is the half-life of the reaction in minutes? Explain. b) Various plots of the concentration of the reactant versus time are given below. What is the order of the reaction? Explain. ILD is 20 time (min) time (min) 05 -35 time (min) c) What is the value of the rate constant at 100.0 °C? d) Would you expect the half-life of the reaction to be longer, shorter, or the same at 60.0 °C? Explain. e) The activation energy in the forward direction is 95.0 kl/mol, and the enthalpy change for the forward reaction is 30.0 kl/mol. Sketch the reaction coordinate diagram for this reaction. ERER AR
Nitrous oxide, N20, decomposes on metal surfaces readily at high temperatures following first-order kinetics for the equation: 2 N20 (g) – 2 N2 (g) + O2 (g) The following data are obtained for a reaction at 850°C: t (min) [N,0] 15 0.0835 30 0.068 80 0.035 120 0.022 What was the initial concentration of N0 (t = 0)? O 0.0885 M 0.0940 M 0.101 M 0.112 M 0.123 M
49. The thermal decomposition of acetaldehyde, CH,CHO-CH+CO is a cond-onder reaction. The following data were obtained at 518°C. time, s Pressure CHICHO, mmHg 0 Chapter 13: Chemical Kinetics 364 330 290 132 Based on the data given, what is the half-life for the disappearance of acetaldehyde? A) 1.5 x 10's B) 410 s C) 5.4 x 10's D) 520s E) 305 s Category: Difficult Section: 13.3 42 105 720
At a certain temperature the rate of this reaction is first order in NH,OH with a rate constant of 0.00777 s : NH,OH (аq) — Nн; (ад) +н,о (аq) Suppose a vessel contains NH,OH at a concentration of 0.750M. Calculate the concentration of NH,OH in the vessel 87.0 seconds later. You may assume no other reaction is important. olo Round your answer to 2 significant digits. Ar | M x10
The activation energy of an uncatalyzed reaction is 86 kJ/mol. The addition of a catalyst lowers the activation energy to 61 kJ/mol Part A Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 24 °C? Express the ratio to two significant digits. ke/ku = 2.2 • 1o Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Part B Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 128 °C? Express the ratio to two significant digits. ? ke/k, = 2.9 • 10² Submit Previous Answers Request Answer X Incorrect; Try Again; 8 attempts remaining
The following data are for the decomposition of nitramide in aqueous solution at 25 °C. NH,NO2(aq) → N20(g) + H20(1) [ NH2NO2 ], 0.802 0.401 0.201 0.101 M time, min 175 350 525 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this O order reaction is min -1
In a study of the decomposition of nitrosyl bromide at 10 °CNOBrNO + ½ Br2the following data were obtained: [NOBr], M 0.249 0.125 6.25×10-2 3.13×10-2 seconds 0 6.16 18.5 43.2 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.249 M is s and when the starting concentration is 0.125 M is s.(2)The average (1/[NOBr]) / t from t = 0 s to t = 6.16 s is M-1 s-1.The average (1/[NOBr]) / t from t = 6.16 s to t = 18.5 s is M-1 s-1.(3)Based on these data, the rate constant for this order reaction is M-1 s-1.
Please provide the step by step solution for the question attached. Graphics must be included. Please make sure the graphics are visible.
Q2) Calculate the rate constant for the first order decomposition reaction of phosphine [PH3], M (at 120 °C): 4PH3(g)→ P4(g) + 6H₂(g)? .64 * 10 ^ - 2 Time (sec) a) 2.47 * 10 ^ - 2 * s ^ - 1 0 2.32 *10^ - 8 1.16 * 10 ^ - 2 (5.80 * 10 ^ - 3)/84 b) 28s ^ - 1 c) 4.64*10^ -2 overline s^ -1 56 d) 3.57 * 10 ^ - 2 * s ^ - 1
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °CHI(g)½ H2(g) + ½ I2(g)the following data were obtained: [HI], M 0.573 0.287 0.144 7.20×10-2 seconds 0 520 781 912 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.573 M is s and when the starting concentration is 0.287 M is s.(2)The average rate of disappearance of HI from t = 0 s to t = 520 s is M s-1.(3)The average rate of disappearance of HI from t = 520 s to t = 781 s is M s-1.(4)Based on these data, the rate constant for this _______zerofirstsecond order reaction is M s-1.
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)- →½ H2(g) + ½ I2(g) the following data were obtained: [HI], M seconds 1.48 0.740 0.370 0.185 750 2.25x103 5.25x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.48 M is 750 s and when the starting concentration is 0.740 M is 1500 S. (2) The average A(1/[HI]) / At from t = 0 s to t = 750 s is M-1 s-1. The average A(1/[HI]) / At from t 750 s to t = 2.25×103 s is M-1 s-1. (3) Based on these data, the rate constant for this 0 order reaction is M-1 s-1.
Give me a clear handwritten answer

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