In a study of the decomposition of ammonia on a tungsten surface at 1100 °CNH3 1/2 N₂ + 3/2 H₂the following data were obtained:[NH3], Mseconds5.91x10-3 2.96x10-304401.48x10-36617.40x10-4(4)Based on these data, the rate constant for this772Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 5.91×10-3 M isconcentration is 2.96x10-3 M isS.(2)The average rate of disappearance of NH3 from t = 0 s to t = 440 s is(3)The average rate of disappearance of NH3 from t = 440 s to t = 661 s isorder reaction isM s 1.Ms¹.M s-1s and when the starting

In a study of the decomposition of ammonia on a tungsten surface at 1100 °C NH3 1/2 N₂ + 3/2 H₂ the following data were obtained: [NH3], M seconds 5.91x10-3 2.96x10-3 0 440 Hint: It is not necessary to graph these data. 1.48x10-3 661 7.40x10-4 772 (1) The observed half life for this reaction when the starting concentration is 5.91x10-³ M is concentration is 2.96x10-³ M is S. (4) Based on these data, the rate constant for this (2) The average rate of disappearance of NH3 from t=0 s to t = 440 s is (3) The average rate of disappearance of NH3 from t = 440 s to t = 661 s is order reaction is Ms¹. Ms1 Ms1 s and when the starting

In a study of the decomposition of ammonia on a tungsten surface at 1100 °C NH3 1/2 N₂ + 3/2 H₂ the following data were obtained: [NH3], M seconds 5.91x10-3 2.96x10-3 0 440 Hint: It is not necessary to graph these data. 1.48x10-3 661 7.40x10-4 772 (1) The observed half life for this reaction when the starting concentration is 5.91x10-³ M is concentration is 2.96x10-³ M is S. (4) Based on these data, the rate constant for this (2) The average rate of disappearance of NH3 from t=0 s to t = 440 s is (3) The average rate of disappearance of NH3 from t = 440 s to t = 661 s is order reaction is Ms¹. Ms1 Ms1 s and when the starting

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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In a study of the decomposition of ammonia on a tungsten surface at 1100 °C NH3- →1/2 N₂ + 3/2 H₂ the following data were obtained: [NH3], M seconds 6.33x10-3 3.17x10-3 1.59x10-3 440 661 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 6.33x10-³ M is starting concentration is 3.17x10-³ M is (4) Based on these data, the rate constant for thi 7.95x10-4 S. (2) The average rate of disappearance of NH3 from t = 0 s to t = 440 s is ✓ 772 (3) The average rate of disappearance of NH3 from t = 440 s to t = 661 s is zero first second order reaction is M s-¹. M s-¹. M s-¹. Is and when the Previous Nex
For the gas phase decomposition of hydrogen peroxide at 400 °C 2 H2O2 2 H2O + O2 the following data have been obtained: [H,O2], M 9.35x10-2 3.54x10-2 2.18×10-2 1.56x10-2 time, s 27.0 54.0 81.0 The average rate of disappearance of H,O2 over the time period from t = 27.0 s to t = 54.0 s is |Ms-!.
The following data are for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C. H2₂O₂(aq) > H₂O(l) + 12 O₂(g) [H₂O₂], M time, min 7.34x10-2 0 3.67x10-2 8.68 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is (2) Based on these data, the rate constant for this 1.84x10-2 9.20x10-3 17.4 min. 26.0 order reaction is min -1
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 decomposition of dinitrogen pentoxide gas at 318.15K is measured as the decrease of N2O5 concentration in partial pressures (mm): The data are shown graphically: Calculate the rate constant for the reaction.
The rate constant for a given reaction is k = 0.312 M1s1. If the initial concentration of reactant is 1.00 M, the what is the length of the third half-life (in seconds)?
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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.
56. For the first-order reaction 2 NO₂(g) + O₂(g) N₂O5(g) t1/2 = 22.5 h at 20 °C and 1.5 h at 40 °C. -1 (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.05 × 10¹³ s-¹, determine the value of k at 30 °C.
The following data are for the gas phase decomposition of sulfuryl chloride at 600 K. sO,C2(g)- - SO2(g) + Cl2(g) [ SO;Clz ], M 2.89x103 1.45x103 7.25x104 3.63x104 time, min 168 336 504 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 order reaction is min
In a study of the decomposition of nitrous oxide at 565 °C N2₂O(g) N₂(g) + ½ O₂(g) the following data were obtained: [N₂0], M seconds 0.750 0 0.375 1.50x10³ 0.188 4.47x10³ Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.750 M is concentration is 0.375 M is S. (2) The average A(1/[N₂0])/ At from t = 0 s to t = 1.50x10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47x103 s is (3) Based on these data, the rate constant for this 9.40×10-2 1.04x104 M-1 S-1. order reaction is M-1 S-1. M-¹ S-1. s and when the starting
A student obtained the following data for the gas phase decomposition of phosphine at 120 °C. PH3(g) 1/4 P4(g) + 3/2 H₂(g) 9.40x10-2 [PH3], M time, s 0 4.70x10-2 29.9 2.35x10-2 1.18x10-2 89.7 59.8 (1) What is the half-life for the reaction starting at t = 0 s? What is the half-life for the reaction starting at t = 29.9 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? (2) Is the reaction zero, first, or second order? (3) Based on these data, what is the rate constant for the reaction?